Chemistry Answers – Flashcards
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The sum of the atomic masses of all the atoms in a compound is called A. Formula mass B. empirical formula C. Molar volume D. Percentage composition
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A. Formula mass
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The number of atoms in one mole of an element is equal to A. A liter B. a gram C. A formula unit D. Avogadro's number
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D. Avogadro's number
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Which compound has a molar mass of 174.3 g/mol A. K2SO4 B. Al(NO3)3 C. MgCO3 D. Ca( NO3)2
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A. K2SO4
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Which is the correct molar mass for the compound FeSO4 A. 103.85 B. 151.85 C. 415.5 D. 247
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B. 151.85
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The simplest whole number ratio of atoms of the elements in a compound is given by the A. Formula mass B. molar mass C. Molecular formula D. Empirical formula
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D. Empirical formula
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The scale for expressing atomic masses is based on the mass of A. Hydrogen-1 B. Carbon-12 C. Oxygen- 16 D. Helium- 2
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B. Carbon-12
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The empirical formula for a compound is CH2O, and the molar mass in 180.2 g/mol. Which is the molecular formula for this compound A. c6h12o6 B. c7h16o5 C. C8H22O4 D. C3H6O3
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A. C6H12O6
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The molecular formula of a compound can be determined by comparing the empirical formula mass with the A. Molar mass of the compound B. Ratio of each element in the compound C. Number of molecules in a mole of the compound D. Percentage composition of the compound
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A. Molar mass of the compound
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Which is the correct molar mass for the compound CaBr2 A. 120 g/mol B. 200 miles C. 240 grams D. 200 g/mol
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D. 200 g/mol
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Which hydrocarbon pair below have identical percent composition of carbon A. C3H4 and C3H6 B. C2H4 and C3H4 C. C2H4 and C4H2 D. C2H4 and C3H6
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D. C2H4 and C3H6
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What is the SI base unit used to measure the amount of a substance A. Kelvin B. Kilogram C. Meter D. Mole
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D. Mole
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Which of the following can represent a molecular as opposed to an empirical formula A. P4O10 B. C2H2 C. C6H12O6 D. All of the above
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D. All of the above
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Which term is described as the percent by the mass of any element in a compound A. Hydrate B. molecular formula C. Empirical formula D. Percent composition
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D. Percent composition
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How many copper atoms are in 0.180 moles of Copper?
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1.08 x. 10^23 atoms Cu
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An experiment requires 64.38 of Ca(OH)2. How many particles of Ca(OH)2 are present in the experiment?
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5.230 x 10^23 particles Ca(OH)2
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A balloon contains 4.50 x 10^22 atoms of helium gas. Calculate the mass of helium in grams.
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0.299 g He
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How many grams of carbon dioxide are there in 1.1183 moles of carbon dioxide
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52.05 g CO2
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How many silver atoms are in 2.456 of Ag2CrO4?
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8.907 x 10^21 atoms Ag
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Hownmany moles are in 2.25 g sample of Mg(NO3)2
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0.0152 Mol Mg(NO3)2
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How many grams of Na2CO3 contain 1.773 x 10^17 sodium atoms?
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1.561 x10^-5 grams Na2CO3
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What is the empirical formula of a compound that contains 27.0% Sulfur, 13.4% and 59.6% Chlorine
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SOCl2
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What is the empirical formula of a compound that contains 29% sodium, 41% sulfur, and 30% oxygen
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Na2S2O3
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A compound that is composed of carbon, hyrdogen, and oxygen contains 70.6% Carbon, 5.9% Hydrogen, and 23.5% Oxygen. The molecular wight of the compound is 136 amu. What is the molecular formula
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C8H8O2
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What is the percent composition of C2H6SO
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30.7% Carbon 7.7% Hydrogen 41.1 % Sulfur 20.5% Oxygen
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What is the percent composition of Calcium Chloride
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36.1% Calcium 63.9% Chlorine
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Stoichiometry is the study of ____ relationships that exist in chemical forums las and chemical reactions A. Qualitative B. subjective C. Descriptive D. Quantitative
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D. Quantitative
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The number of moles of each substance taking part in a chemical reaction is indicated by A. The molar mass of each substance B. the coefficients in the balanced equation C. The subscripts in the chemical formulas D. The type of reaction
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B. the coefficients in the balanced equation
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In the balanced equation 2H2 + O2 --> 2H2O A. 2 moles of hydrogen react with 1 mole of oxygen B. 4 moles of hydrogen act with 1 mole of oxygen C. 2 moles of hydrogen react with 2 moles of oxygen D. 4 moles of water are produced
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A. 2 moles of hydrogen react with 1 mole of oxygen
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What is the correct mole ratio of K3PO4 to KNO3 in the chemical reaction 3Mg(NO3)2 + 2K3PO4 ---> Mg3(PO4)2 + 6KNO3 A. 1:1 B. 2:3 C. 1:3 D. 1:2
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C. 1:3
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The coefficients in a balanced equation represent ratios of all of the following except A. Mass B. moles C. Volumes D. Molecules
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A. Mass
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A balanced equation verifies the law of conversation of matter because A. The molar masses of all substances are the same B. the coefficients on both sides of the equation are the same C. The mass of the reactants equals the mass of the products D. The mass of the products always equals 100 grams
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C. The mass of the reactants equals the mass of the products
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Given the equation N2 + 3H2 ---> 2NH3 what is the mole ratio of hydrogen to ammonia? a. 1:1 b. 1:2 c. 3:2 d. 2:3
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c. 3:2
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How many moles of KBr will be produced from 7 moles of BaBr2 BaBr2 + K2SO4 --> 2KBr + BaSO4
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10 mol KBr
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How many grams of chlorine gas can be produced from the decomposition of 37.41 moles of AuCl3 by this reaction: 2AuCl3 ---> 2Au + 3Cl2
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3984 grams Cl2
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How many moles of NO are produced from 13.2 moles of oxygen gas in the presence of excess ammonia? 4NH3 + 5O2 --> 4NO + 6H20
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10.6 moles NO
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How many grams of CH4 are required to produce 43 g of Cu according to the following equation 4CuO + CH4 --> CO2 + 2H2O + 4Cu
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2.7 g CH4
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How many grams of Fe3O4 are required to react completely with 300.0 grams of H2
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8689 g Fe3O4
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Verify the law of conversation of matter for the following reaction Al4C3 + 12HCl --> 4AlCl3 + 3CH4
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Reactants total mass= 582.0g Products total mass = 582.0g verified
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How many grams of Al will be produced for 21.3 moles of Al2O3? 2Al2O3 ---> 4Al 3O2
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1150 g Al
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Verify the law of conversation of matter for the following reaction 2H2S + 3O2 ----> 2SO2 + 2H2O
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reactants total mass= 164.2g produced total mass= 164.2g verified
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which type of reaction takes place in the presence of oxygen and produces carbon dioxide and water A. decomposition B. doubles replacement C. synthesis D. Combustion
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d. Combustion
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in balancing a chemical equation, which of the following are you allowed to do a. change subscripts b. write coefficients c. change superscripts d. add new substances
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b. write coefficients
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what is the probable product of a double replacement reaction? a. a new compound and the replace metal b. a new compound and the replaced nonmetal c. two different compounds d. a single compound
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c. two different compounds
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during a chemical reaction_______ A. new elements are produced b. atoms are destroyed c. atoms are rearranged d. elements are destroyed
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c. atoms are rearranged
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what is the sum of the coefficients in the following reaction: C3H8 + 5O2 ---> 3CO2 + 4H2O A. 10 B. 13 C. 17 D. 29
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B. 13
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in a combustion reaction a hydrocarbon combines with oxygen releasing what? A. carbon B. energy C. Hydrogen D. plasma
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B. energy
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which types of reactions are essentially opposites of one another A. combustion and synthesis B. single replacement and double replacement C. synthesis and single replacement D. synthesis and decomposition
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D. synthesis and decomposition
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Identify specific reaction 2H2 + O2 ---> 2H2O
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synthesis
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Identify specific reaction C3H8 + 5O2---> 3CO2 + 4H2O
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combustion
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Identify specific reaction Zn + CuSO4 ---> ZnSO4 + Cu
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single replacement
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Identify specific reaction H2CO3 ---> CO2 + H2O
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Decomposition
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Identify specific reaction AgNO3 + NaCl ----> AgCl + NaNO3
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double replacement
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Balance hno3 + CaCO3 ---> Ca(NO3)2 + CO2 + H2O
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coefficients 2+ 1 ---> 1 + 1 + 1
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balance Al2O3 + C + Cl2 ---> AlCl3 + CO
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coefficients 1 + 3 + 3 --> 2 + 3
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balance Al(NO3)3 + Na2S ---> Al2S3 + NaNO3
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coefficients 2 + 3 ---> 1 + 6
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Balance H2S + Fe(OH)3 ---> Fe2S3 + H2O
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coefficients 3 + 2 ---> 1 + 6
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write and balance aluminum hydroxide reacts with nitric acid ( HNO3) to yield aluminum nitrate and water
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Al(OH)3 + 3HNO3 --> Al(NO3)3 + 3H2O
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Write and balance Iron metal reacts with oxygen to produce iron III oxide
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4Fe + 3O2 ---> 2Fe2O3
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write and balance Sodium hydroxide reacts with phosphoric acid( H3PO4) to yield sodium phosphate and water
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3NaOH + H3PO4 ---> Na3PO4 + 3H2O
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finish balance CuCO3 --->
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CuCo3 ---> CuO + CO2
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finish and balance Mg + O2 ---->
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2Mg + O2 ---> 2MgO
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finish and balance C3H6 + O2---->
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2C3H6 + 9O2 ----> 6CO2 + 6H2O
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finish and balance H2O ---->
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2H2O ---> 2H2 + O2
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finish and balance Al + NiSO4 --->
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2Al + 3NiSO4 ---> Al2(SO4)3 + 3Ni
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finish and balance AgNO3 + NaCl--->
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AgNO3 + NaCl ----> AgCl + NaNO3
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finish and balance (NH4)2S + ZnCl2 --->
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(NH4)2S + ZnCl2 ---> 2NH4Cl + ZnS
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finish and balance Zn + CuSO4 --->
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Zn + CuSO4 ---> Zn(SO4) + Cu
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infer three peices of evidence that a chemical reaction has taken place
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- temperature change - color change - odor - release of gases - formation of a solid
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The basis of an ionic bond is the A. Sharing of an electron pair B. electrical attraction between oppositely charged ions C. Absorption of energy D. Absorption of water into their solid structures
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B. Electrical attraction between oppositely charged ions
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According to the octet rule, atoms tend to lose, gain or share electrons in order to have how many electrons in its outer she'll A. 2 B. 4 C. 6 D. 8
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D. 8
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Which is the correct order of bond strength, from greatest to least, for compounds MgCl2, MgO, Mg3N2 A. MgO, MgCl2, Mg3N2, B. Mg3N2, MgCl2, MgO C. MgCl2, MgO, Mg3N2 D. Mg3n2, MgO, MgCl2
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D. Mg3n2, MgO, MgCl2
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Which is a correct statement of bond strength A. Compounds with smaller atoms have weaker bond strength B. compounds with higher total numbers of atoms in the compound have greater bond strength C. Compounds containing atoms with greater charges have higher bond strength D. Compounds with a more negative lattice energy have lower bond strength
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C. Compounds containing atoms with greater charges have higher bond strength
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A cation is an ion with A. A positive charge B. a negative charge C. No charge D. More than 8 electrons
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A. A positive charge
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The basis of an ionic bond is the A. Sharing of a electron pair B. electrical attraction between oppositely charged ions C. Absorption of energy D. Absorption of water into their solid structure
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B. electrical attraction between oppositely charged ions
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Which is described as the force holding two atoms together A. Cation B. chemical bond C. Formula unit D. Lattice
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B. chemical bond
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A monatomic ion consist of A. More than one atom B. one atom C. No atoms
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B. one atom
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Whcih is true of binary ionic compounds A. They consist of only two atoms B. they consist of atoms of only two elements C. They contain different anions D. They have bonds that share two valence electrons
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B. they consist of atoms of only two elements
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An empirical formula always indicates A. Which atoms are attached to which in a molecule B. how many of each atom are in a molecule C. The simplest whole number ratio of different atoms in a compound D. The isotope of each element in a compound
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C. The simplest whole number ratio of different atoms in a compound
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A compound has the formula X3Y. For every 15 X atoms present in this compound, how many Y atoms are there A. 3 B. 5 C. 45 D. 15
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B. 5
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Which is a physical property of ionic compounds in their solid state A. Good conductor of electricity B. weak attractive forces between ions C. Low boiling point D. High meting point
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D. High melting point
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Which is a property of substances that exhibit metallic bonding A. High boiling points B. rigid and brittle C. Low melting points D. Poor conductor of electrcity
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A. High boiling points
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An ionic compound must have an overall charge of A. +2 B. -2 C. +1 D. -1 E. 0
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E. 0
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Write empirical formula Zn^2 + PO4^3 --->
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Zn3(PO4)2
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Write empirical formula Pb^2 + NO3^-1 --->
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Pb(NO3)2
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Write empirical formula NH4^1 + CO3^2 --->
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(NH4)2CO3
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Write Empirical Formula Na^1 + S^-2 --->
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Na2S
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Write Emprical Formula Na^1 + OH^-1 --->
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NaOH
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Write empirical formula Chromium (IV) Phosphate
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Cr3(PO4)4
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Write empirical formula Iron(II) Sulfide
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FeS
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Write empirical formula Ammonium hydroxide
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NH4OH
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Write empirical formula Magnesium oxide
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MgO
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Write empirical formula Lead (II) Nitrate
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Pb(NO3)2
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Write empirical formula Sodium Chloride
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NaCl
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Write empirical formula Aluminum Niteide
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AlN
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Nam Ba(OH)2
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Barium hydroxide
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Name Na2S
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Sodium sulfide
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Name NaC2H3O2
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Sodium acetate
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Name CrCl3
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Chromium ( III) Clhoride
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Name Ag2SO4
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Silver sulfate
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Name KBr
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Potassium bromide
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Name Cu(NO3)2
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Copper (II) Nitrate
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A bond is classified as non polar covalent if the difference in the electro negativity between the two atoms is A. 2.0 or more B. between 0.5 and 1.9 C. 0.4 or less D. Less than zero
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C. 0.4 or less
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How many single covalent bonds can halogens form A. 1 B. 2 C. 3 D. 4
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A. 1
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Which one of the following molecular formulas is also an empirical formula A. C6H6O2 B. C2H6SO C. H2O2 D. H2P4O6
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B. C2H6SO
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When one atom is significantly more electronegative than another one, a covalent bond between them is A. Non polar B. hydrate C. Polar D. Very unstable
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C. Polar
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What is the maximum number of double bonds that a hydrogen atom can form A. 0 B. 1 C. 2 D. 3
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A. 0
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The type of compound that is mostly likely to contain a covalent bond is A. One that is composed of a metal from the far left of the periodic table and a nonmetal from the far right of the periodic table B. a solid metal C. One that is composed of only nonmetals D. Held togther by the electrostatic forces between oppositely charged ions
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C. One that is composed of only nonmetals
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A bond is classified as polar covalent if the difference in the electro negativity is between the two atoms is A. 2.0 or more B. between 1.9 and 0.5 C. 0.4 or less D. Less than zero
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B. between 1.9 and 1.5
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How many single covalent bonds must a silicon atom form to have a complete octet in its glance she'll A. 3 B. 4 C. 1 D. 2
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B. 4
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The basis of a covalent bond is the A. Sharing of an electron pair B. electrical attraction between oppositely charged ions C. Absorption D. Absorption of water into their solid structures
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A. Sharing of an electron pair
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Which one of the following does not occur as a diatomic molecule in elemental form? A. Oxygen B. nitrogen C. Sulfur D. Hydrogen
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C. Sulfur
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In a triple bond between two atoms, the number of shared pairs of electron is A. 1 B. 2 C. 3 D. 4
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C. 3
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The name of an oxyacid has the suffic -ic acid. What is the suffix of the oxyanion A. Ic B. it's C. Ate D. Ous
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C. Ate
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Which central atom violates the octet rule A. NH3 B. SeF2 C. BF3 D. AsF3
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C. BF3
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In which of the molecules below is the carbon-carbon distance the shortest A. H2C= CH2 B. H-C( three lines) C-H C. H3C-CH3 D. H2C=C=CH2
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B. H-C(three lines) C-H
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Which two bonds are most similar in polarity A. O-F and Cl-F B. B-F and Cl-F C. Al- Cl and I-Br D. I-Br and SI-Cl
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A. O-F and Cl-F
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A bond is classified as ionic if the difference in the electro negativity between the two atoms is A. 2.0 or more B. between 1.9 and 0.5 C. 0.4 or less D. Less than zero
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A. 2.0 or more
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Name SF6
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Sulfur hexafluoride
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Name As2S3
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Diarsenic trisulfide
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Name P2O5
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Diphosphorus pentoxide
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Name H2O
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Water
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Write chemical formula Iodine pentaflouride
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IF5
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Write chemical formula Chlorine
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Cl2
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Write chemical formula Carbon tetra chloride
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CCl4
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Write chemical formula Digit roger monoxide
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N2O
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Name Perchloric acid
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HClO4
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Name Phosphoric acid
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H3PO4
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Name Nitric acid
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HNO3
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Name Hydrobromic acid
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HBr
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Name HCl
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Hydrochloric acid
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Name H2CO3
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Carbonic acid
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Name HI
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Hydroiodic acid
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Name H2SO4
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Suffic acid
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Name MgSO4 - 7H2O
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Magnesium Sulfate- heptahydrate
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Find electro negativity and name bond type Sulfur and oxygen
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1.0/ polar
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Find electro negativity and name bond type Phosphorous and oxygen
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1.4/ polar
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Find electro negativity and name bond type Potassium and fluoride
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3.2/ ionic
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Find electro negativity and name bond type Sulfur and iodine
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0/ non polar
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Find the complete ionic equation, identity the spectator ions, and write the net equation NiBr2(aq) + 2AgNO3(aq) ---> Ni(NO3)2(aq) + 2AgBr(s)
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COmplete equation= Ni^2(aq) +2Br^-1(aq) + 2Ag^1(aq) + 2NO3^-1(aq) ---> Ni^2(aq) + 2NO3^-1(aq) + 2AgBr(s) Spectator ions= Ni^2(aq) and NO3^-1(aq) Ionice equation= Br^-1(aq) + Ag^1(aq) ---> AgBr(s)
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Find the complete ionic equation, identity the spectator ions, and write the net equation CuCl2(aq) + 2NaOH(aq) ---> Cu(OH)2(s) + 2NaCl(aq)
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Complete equation= Cu^2(aq) + 2Cl^-1(aq) + 2Na^1(aq) + 2OH^-1(aq) ---> CU(OH)2(s) + 2Na^1(aq) + 2Cl^-1(aq) Spectator ions= Cl^-1(aq) and Na^1(aq) Net equation= Cu^2(aq) + 2OH^-1(aq) ---> Cu(OH)2^-1
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Find the complete ionic equation, identity the spectator ions, and write the net equation Aqueous silver nitrate reacts with ammonium carbonate to produce a silver carbonate precipitate
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Complete equation= 2AgNO3(aq) + (NH3)2CO3(aq) ---> Ag2CO3(s) + 2NH4NO3(aq) Ionic equation= 2Ag^1(aq) + 2NO3^-1(aq) + 2NH4^1(aq) + CO3^-2 ---> Ag2Co3(s) 2NH4^1(aq) + 2NO3^-1(aq) Spectator ions= NO3^-1(aq) and NH4^1(aq) Net equation= 2Ag^1(aq) + CO3^-2(aq) ---> Ag2CO3(s)
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Find the complete ionic equation, identity the spectator ions, and write the net equation Aqueous barium iodide and sodium sulfate combine to form a barium sulfate precipitate
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Complete equation = BaI2(aq) + Na2SO4(aq) ---> BaSO4(s) + 2NaI(aq) Ionic equation= Ba^2(aq) + 2I^-1(aq) + 2Na^1(aq) + SO4^-2(aq) ---> BaSO4(s) + 2Na^1(aq) + 2I^-1(aq) Spectator ions= I^-1(aq) and Na^1(aq) Net equation= Ba^2(aq) + SO4^-2 ---> BaSO4(s)
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Find the complete ionic equation, identity the spectator ions, and write the net equation Aqueous sulfuric acid reacts with aqueous sodium hydroxide to produce aqueous sodium sulfate and water
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Complete equation= H2SO4(aq) + 2NaOH(aq) ---> Na2SO4(aq) + 2H2O(l) Ionic equation= 2H^1(aq) + SO4^-2(aq) + 2Na^1(aq) + 2OH^-1(aq) ---> 2Na^1(aq) + SO4^-2(aq) + 2H2O(l) Spectator ions= SO4^-2(aq) and Na^1(aq) Net equation= H^1(aq) + OH^-1(aq) ---> H2O(l)
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Write products with states and balance 2HNO3(aq) + Ba(OH)2(aq) --->
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Ba(NO3)2(aq) + 2H2O(l)
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Write products with states and balance K2S(aq) + Ni(NO3)2(aq) --->
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2KNO3(aq) + NiS(s)
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Write products with states and balance H2SO4(aq) + K2CO3(aq) --->
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H2O(l) + CO2(g) + K2SO4(aq)
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Write products with states and balance Pb(NO3)2(aq) + 2 Nacl(aq) --->
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PbCl2(s) + 2NaNO3(aq)
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Which of the following is a reason why the actual yield differs from the expected yield A. Some portion of the reactants may not react B. some of the reactants may take part in side reactions C. Some of the product may be lost during the process of recovering it or transferring it D. All of the above
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D. All of the above
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A reaction was predicted through calculations to produce 32.4 g of a compound. When the product was measures from the expirement, there were only 26.1 g made. What is the percent yield of this reaction A. 80.6% B. 6.3% C. 24.1% D. 58.5%
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A. 80.6%
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A certain reaction has a 73.6% yield. If 53.8 grams of the product were predicted by stoichiometry to be made, what would the actual yield be A. 73.1 g B. 19.8 g C. 26.9 g D. 39.6 g
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D. 39.6 g
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The limiting reactant is a chemical reaction A. Is completely used in the reaction B. will have some amount unchanged, or leftover, after the reaction C. Cannot be calculated without performing the reaction D. Has no effect on the amount of product formed
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A. Is completely used in the reaction
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The calculated amount of product that should be produced in a chemical reaction is called A. True yield B. expected yield C. Actual yield D. Percent yield b
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B. expected yield
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The excess reactant in a chemical reaction A. Is completely used in the reaction B. will have some amount unchanged, or leftover, after the reaction C. Cannot be calculated without performing the reaction D. Has no effect on the amount of product formed
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B. will have some amount unchanged, or leftover, after the reaction
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A chemical reaction can theoretically produce 137.5 grams of product, but in actuality 112.9 grams are produced. WHich is the percent yield for this reaction? A. 82.1% B. 62.0% C. 24.6% D. 17.9%
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A. 82.1%
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The ration of the actual amount of product to the amount of product in a calculated chemical reaction is called the A. True yield B. expected yield C. Actual yield D. percent yield
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D. percent yield
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When 22.5 g of Cu reacts with 53.4g AgNO3, what is the limiting reactant? Cu + 2AgNO3 ---> Cu(NO3)2 + 2Ag
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AgNO3
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Identify the limiting reactant and how much chlorine should be produced if 84.2 grams of aluminum chloride and 68.4 grams bromine are combined 2AlCl3 + 3Br2 ---> 2AlBr3 + 3Cl2
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Bromine / 30.4 g Cl2
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When 4.22g of AgNO3 reacts with 7.73 g of AlCl3 according to the following reaction 3AgNO3 + AlCl3 ---> Al(NO3)3 + 3AgCl A- what is the limiting a taint B- what mass of AgCl is produced C- which reactant is in excess D- how much excess is left
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A- AgNO3 B- 3.56 g AgCl C- AlCl3 D- 6.62 g AlCl3
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A piece of 6.32 g of Zn is placed Ina copper sulfate solution in excess. 4.36 g of copper was recovers . What is the percent yield Zn + CuSO4---> Cu + ZnSO4
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70.9%
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If the action of 3.82 g of magnesium Niteide with 7.73 g of water produces 3.60 g of magnesium oxide. What is the theoretical yield and percent yield Mg3N2 + 3H2O ---> 2NH3 + 3MgO
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Theoretical yield= 4.58 g MgO Percent yield= 78.6 %
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The percent yield of sulfure hexafluoride in the action is 79.0%. Caculate the theoretical yield of sulfur hexafluoride when 7.90 g of fluorine reacts with excess sulfure. What is the actual yield of this experiment. S + 3F2 ----> SF6
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Theoretical yield = 10.1 g SF6 Actual yield = 7.98 g SF6
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Determine the percent yield of gold III chloride and theoretical yield 2Au + 3Cl2 ----> 2AuCl3 Given: Au- 39.4 g Cl2- 21.3 g Actual yield- 35.2 g
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Theoretical yield- 60.7 Percent yield- 58.0 %
