Chapter 6 Practice Questions - Flashcards

question

1) The chemical formula clearly indicates the relationship between the mass of each element in the formula.

answer

false

question

2) Mass is used as a method of counting atoms

answer

true

question

3) One hundred nickels must have the same mass as one hundred pennies.

answer

false

question

4) The numerical value of the mole is defined as being equal to the number of atoms in exactly 12 grams of pure carbon-12.

answer

false

question

5) The mole has a value of 6.023 × 1022

answer

false

question

6) Avogadro's Number is 6.022 × 1023.

answer

true

question

7) The number 6.022 × 1023 is six times larger than the number 6.022 × 1022.

answer

false

question

8) The lighter the atom, the less mass in one mole of that atom.

answer

true

question

9) One mole of argon has more atoms in it than one mole of neon.

answer

false

question

10) One mole of nitrogen gas contains (2) × (6.022 × 1023) nitrogen atoms.

answer

true

question

11) One mole of zinc contains 65.39 zinc atoms.

answer

false

question

12) One mole of copper atoms is 6.022 × 1023 copper atoms

answer

true

question

13) The mass of 2.0 moles of H2O is greater than the mass of 1.0 mole of CO2.

answer

false

question

15) Two moles of cobalt atoms have a mass of 117.87 grams

answer

true

question

16) Six grams of carbon contains 3.008 × 1023 atoms.

answer

true

question

17) One mole of I2 has more atoms in it than one mole of Na.

answer

true

question

18) One mole of CO2 gas contains 1 mole of carbon atoms and 2 moles of oxygen atoms.

answer

true

question

19) The molar mass of a compound in grams per mole is numerically equal to the formula mass of the compound in atomic mass units.

answer

true

question

20) One mole of water contains 16 grams of oxygen atoms.

answer

true

question

21) One mole of water contains 6.022 × 1023 hydrogen atoms

answer

false

question

22) There are 6 grams of carbon in 22 grams of carbon dioxide.

answer

true

question

23) The molar mass of a compound serves as a conversion factor between grams and moles.

answer

true

question

24) One mole of lead(II) nitrate contains six moles of oxygen atoms.

answer

true

question

25) The chemical formula CuBr2 indicates that this compound is composed of 1 gram of copper and 2 grams of bromine.

answer

false

question

26) The correct formula for calculating mass percent of X in compound XY is: MASS OF X/MASS OF Y = Mass % X

answer

false

question

27) Water is 11.2% hydrogen by mass.

answer

true

question

28) C2H3O2 could be an empirical formula.

answer

true

question

29) c2h6o3 could be an empirical formula.

answer

true

question

30) C2H6O4 could be an empirical formula.

answer

false

question

31) An empirical formula gives the specific number of each type of atom in a molecule.

answer

false

question

32) An empirical formula gives the smallest whole number ratio of each type of atom in a molecule.

answer

true

question

33) The empirical formula for C6H6 is c3h3.

answer

false

question

34) The molecular formula is equal to the empirical formula multiplied by a whole number integer

answer

true

question

35) A molecule that has an empirical formula of HO and a molar mass of 34.02 gram must have a molecular formula of H2O2.

answer

true

question

36) The empirical formula mass is 18.0 and the molecular formula mass is 90, therefore n = 5.

answer

true

question

37) The empirical formula mass must be 25.0 if the molecular formula mass is 250 and n = 5.

answer

false

question

1) What is the correct value for Avogadro's number? A) 6.022 × 1023 B) 6.022 × 1033 C) 6.023 × 1022 D) 6.022 × 102.3 E) none of the above

answer

A) 6.022 × 1023

question

2) One half of a mole of atoms would contain how many atoms? A) 0.5 B) 3.011 × 1023 C) 6.022 × 1023 D) 6.022 × 1011.5 E) none of the above

answer

B) 3.011 × 1023

question

3) Which of the following statements about the mole is FALSE? A) One mole of atoms makes up an amount of atoms that can be seen with the naked eye. B) A mole of a monatomic element corresponds to one Avogadro's number of atoms. C) One mole of a monatomic element has a mass equal to its atomic mass expressed in grams. D) One mole of water contains 1/2 mole of oxygen atoms. E) none of the above

answer

D) One mole of water contains 1/2 mole of oxygen atoms.

question

4) How many atoms are in 5.80 moles of He? A) 6.02 × 1023 B) 1.03 × 1023 C) 4.00 D) 3.49 × 1024 E) none of the above

answer

D) 3.49 × 1024

question

5) How many atoms are in 1.50 moles of fluorine gas? A) 6.022 × 1023 B) 9.03 × 1023 C) 18.98 D) 1.81 × 1024 E) none of the above

answer

D) 1.81 × 1024

question

6) How many moles of Cu are in 1.48 × 1025 Cu atoms? A) 0.0408 B) 24.6 C) 1.54 × 1025 D) 6.022 × 1023 E) none of the above

answer

B) 24.6

question

7) One mole of boron has a mass of ________ g. A) 9.012 B) 6.022 × 1023 C) 5 D) 10.811 E) none of the above

answer

D) 10.811

question

8) One mole of oxygen gas has a mass of ________ g. A) 16.0 B) 32.0 C) 6.022 × 1023 D) 8 E) none of the above

answer

B) 32.0

question

9) What is the mass in grams of 5.40 moles of lithium? A) 6.94 B) 37.5 C) 1.29 D) 3.25 × 1024 E) none of the above

answer

B) 37.5

question

10) What is the mass of 0.560 moles of chlorine gas? A) 19.9 B) 63.3 C) 127 D) 39.7 E) none of the above

answer

D) 39.7

question

11) You have 10.0 g each of Na, C, Pb, Cu and Ne. Which contains the largest number of moles? A) Na B) C C) Pb D) Cu E) Ne

answer

B) C

question

12) You have 10.0 g each of Na, C, Pb, Cu and Ne. Which contains the smallest number of moles? A) Na B) C C) Pb D) Cu E) Ne

answer

B) C

question

13) How many moles of iron are contained in 1.75 kg of iron? A) 3.13 × 10-2 B) 3.13 × 10-4 C) 31.3 D) 3.13 × 104 E) none of the above

answer

C) 31.3

question

14) How many moles are there in 17.5 grams of sodium? A) 22.99 B) 1.05 × 1025 C) 0.761 D) 1.31 E) none of the above

answer

C) 0.761

question

15) How many moles are there in 82.5 grams of iron? A) 4.97 × 1025 B) 55.85 C) 0.677 D) 1.48 E) none of the above

answer

D) 1.48

question

16) How many moles of bromine gas are in 37.7 grams? A) 0.236 B) 0.472 C) 3.01 × 103 D) 79.9 E) none of the above

answer

A) 0.236

question

17) How many atoms are in 15.6 grams of silicon? A) 2.64 × 1026 B) 3.34 × 1023 C) 0.555 D) 438 E) none of the above

answer

B) 3.34 × 1023

question

18) How many hydrogen atoms are in 35.0 grams of hydrogen gas? A) 4.25 × 1025 B) 2.09 × 1025 C) 2.12 × 1025 D) 1.05 × 1025 E) none of the above

answer

D) 1.05 × 1025

question

19) What is the mass of 3.09 × 1024 atoms of sulfur in grams? A) 9.64 × 1022 B) 9.91 × 1025 C) 165 D) 0.160 E) none of the above

answer

C) 165

question

20) How many moles of Pb are in 4.71 × 1021 Pb atoms? A) 0.00782 B) 2.84 × 1045 C) 207.2 D) 6.022 × 1023 E) none of the above

answer

A) 0.00782

question

21) What is the mass of 1.56 × 1021 atoms of magnesium in grams? A) 4.72 × 10-5 B) 0.0630 C) 0.142 D) 1.07 × 10-4 E) none of the above

answer

B) 0.0630

question

22) In comparing a balloon containing 25 grams of helium to a balloon containing 25 grams of neon, which one of the following statements is TRUE? A) Each balloon has an equal number of atoms. B) The helium balloon has more atoms. C) The neon balloon has more atoms. D) This scenario cannot happen because gases have no mass. E) none of the above

answer

B) The helium balloon has more atoms.

question

23) In comparing 1 mole of carbon atoms to one mole of magnesium atoms, which statement is TRUE? A) The mass of 1 mole of carbon is greater than the mass of 1 mole of magnesium. B) The mass of 1 mole of magnesium is greater than the mass of 1 mole of carbon. C) The mass of 1 mole of carbon is the same as the mass of 1 mole of magnesium. D) There are more atoms in 1 mole of magnesium than in 1 mole of carbon. E) none of the above

answer

B) The mass of 1 mole of magnesium is greater than the mass of 1 mole of carbon.

question

24) Which of the following contains 9.02 × 1023 atoms? A) 4.00 g H2 B) 9.00 g H2O C) 28.0 g N2 D) 32.0 g O2 E) none of the above

answer

B) 9.00 g H2O

question

25) The mass of one mole of carbon dioxide is ________ g. A) 28.01 B) 384.4 C) 32.00 D) 44.01 E) none of the above

answer

D) 44.01

question

26) What is the molar mass of aluminum sulfate? A) 123.0 g/mol B) 278.0 g/mol C) 306.2 g/mol D) 315.2 g/mol E) 342.2 g/mol

answer

E) 342.2 g/mol

question

27) Calculate the molar mass of ammonium carbonate. A) 78.05 g/mol B) 88.05 g/mol C) 96.09 g/mol D) 112.09 g/mol E) none of the above

answer

C) 96.09 g/mol

question

28) Calculate the molar mass of calcium nitrate. A) 136.03 g/mol B) 102.09 g/mol C) 132.10 g/mol D) 164.10 g/mol E) none of the above

answer

D) 164.10 g/mol

question

29) How many molecules of sulfur trioxide are in 78.0 grams? A) 5.87 × 1023 B) 7.33 × 1023 C) 3.76 × 1027 D) 0.974 E) none of the above

answer

A) 5.87 × 1023

question

30) How many molecules of nitrogen monoxide are in a 22.5 gram sample? A) 5.86 × 1023 B) 7.33 × 1023 C) 4.51 × 1023 D) 4.06 × 1023 E) none of the above

answer

C) 4.51 × 1023

question

31) If 3.011 × 1023molecules have a mass of 20.04 grams, what is the molar mass of this substance? A) 40.08 g/mol B) 10.02 g/mol C) 20.04 g/mol D) 6.658 × 10-23g/mol E) none of the above

answer

A) 40.08 g/mol

question

32) If 2.01 × 1023 atoms of an element from Group IA of the periodic table has a mass of 7.675 grams, this element is most likely: A) Li. B) Na. C) K. D) Rb. E) Cs.

answer

B) Na.

question

33) One mole of (NH4)2HPO4 contains how many moles of hydrogen atoms? A) 4 B) 2 C) 8 D) 9 E) none of the above

answer

D) 9

question

34) One mole of ammonium nitrate contains: A) 3 moles of hydrogen. B) 2 moles of oxygen. C) 2 moles of nitrogen. D) 1 mole of nitrogen. E) none of the above

answer

C) 2 moles of nitrogen.

question

35) One mole of ammonium nitrite contains: A) 2 moles of nitrogen atoms. B) 4 moles of hydrogen atoms. C) 2 moles of oxygen atoms. D) All of A, B, and C. E) None of A, B, and C.

answer

D) All of A, B, and C.

question

36) One mole of potassium sulfate contains: A) 4 moles of oxygen. B) 2 moles of sulfur. C) 1 mole of potassium. D) 3 moles of potassium. E) none of the above

answer

A) 4 moles of oxygen.

question

37) How many moles of carbon are in 3.5 moles of calcium carbonate? A) 10.5 B) 3.5 C) 7 D) 100.09 E) none of the above

answer

B) 3.5

question

38) How many moles of fluorine are in 3.2 moles of xenon hexafluoride? A) 22.4 B) 12.8 C) 19.2 D) 16 E) none of the above

answer

C) 19.2

question

39) If a sample of carbon dioxide contains 3.8 moles of oxygen atoms, how many moles of carbon dioxide are in the sample? A) 1.9 B) 3.8 C) 7.6 D) 11.4 E) none of the above

answer

A) 1.9

question

40) A 15.5 gram sample of diphosphorous pentoxide contains how many grams of phosphorous? A) 3.38 B) 1.69 C) 6.76 D) 13.5 E) none of the above

answer

C) 6.76

question

41) A 42.7 gram sample of potassium nitrate contains how many grams of potassium? A) 39.1 B) 16.5 C) 21.4 D) 8.54 E) none of the above

answer

B) 16.5

question

42) An iron ore sample is found to be 35.00% Fe by mass. How many grams of ore are needed to obtain 454.0 grams of Fe? A) 1297 B) 158.9 C) 295.1 D) 350.0 E) none of the above

answer

A) 1297

question

43) A 500. gram iron ore sample was determined to contain 242 grams of iron. What is the mass percent of iron in the ore? A) 93.7 B) 48.4 C) 51.6 D) 32.6 E) none of the above

answer

B) 48.4

question

44) Bauxite is an ore that contains the element aluminum. If you obtained 108 grams of aluminum from an ore sample that initially weighed 204 grams, what is the mass percent of aluminum in this bauxite ore? A) 52.9 B) 15.6 C) 0.53 D) 47.1 E) none of the above

answer

A) 52.9

question

45) What is the mass percent of hydrogen in water? A) 33.3 B) 88.8 C) 5.60 D) 11.2 E) none of the above

answer

D) 11.2

question

46) What is the mass percent of chlorine in hydrochloric acid? A) 2.8 B) 35.5 C) 97.2 D) 70.1 E) none of the above

answer

C) 97.2

question

47) What is the mass percent of carbon in oxalic acid, H2C2O4? A) 2.24 B) 13.3 C) 26.7 D) 34.5 E) none of the above

answer

C) 26.7

question

48) Which of the following compounds has the highest mass percent of "O"? A) MnO B) MnO2 C) Mn2O3 D) Mn3O2 E) none of the above

answer

B) MnO2

question

49) Which of the following statements about empirical formulas is incorrect? A) An empirical formula represents a molecule. B) An empirical formula gives the smallest whole number ratio of each type of atom in a molecule. C) An empirical formula must be multiplied by an integer to obtain the molecular formula. D) The molecular formula can be the same as the empirical formula in some situations. E) All statements are correct.

answer

A) An empirical formula represents a molecule.

question

50) The empirical formula of a compound: A) describes the mass relationships in a molecule. B) is the same as the molecular formula. C) indicates the structure of the molecule. D) indicates the simplest ratio of atoms in the compound. E) none of the above

answer

D) indicates the simplest ratio of atoms in the compound.

question

51) The simplest formula for hydrogen peroxide is HO. To determine its molecular formula, it is necessary to know: A) the properties of hydrogen peroxide. B) the density of hydrogen peroxide. C) the molar mass of hydrogen peroxide. D) the number of moles of hydrogen peroxide in 1.00 g of the substance. E) none of the above

answer

C) the molar mass of hydrogen peroxide.

question

52) Which of the following is already in its empirical formula? A) C22H34O10 B) C6H6 C) c6h12o3-structure/">c6h12o3 D) C5H12O2 E) none of the above

answer

D) C5H12O2

question

53) The chemical formula CH2O can be classified as: A) molecular only. B) empirical only. C) empirical, possibly molecular. D) not enough information E) none of the above

answer

C) empirical, possibly molecular.

question

54) A chromium oxide compound contains 104.0 grams of chromium and 48.0 grams of oxygen. What is the most likely empirical formula of this compound? A) CrO B) CrO2 C) CrO3 D) Cr2O3 E) Cr3O2

answer

D) Cr2O3

question

55) An iron chloride compound contains 55.85 grams of iron and 106.5 grams of chlorine. What is the most likely empirical formula for this compound? A) FeCl B) FeCl2 C) Fe2Cl D) FeCl3 E) Fe3Cl

answer

D) FeCl3

question

56) A 7.96 gram sample of silver reacts with oxygen to form 8.55 gram of the metal oxide. What is the formula of the oxide? A) AgO B) AgO2 C) Ag2O D) Ag3O E) none of the above

answer

C) Ag2O

question

57) Determine the empirical formula of a compound containing 60.3% magnesium and 39.7% oxygen. A) MgO B) MgO2 C) Mg2O3 D) Mg2O E) none of the above

answer

A) MgO

question

58) Determine the empirical formula of a compound containing 83% potassium and 17.0% oxygen. A) KO B) KO2 C) K2O3 D) K2O E) none of the above

answer

D) K2O

question

59) Vitamin C is known chemically by the name ascorbic acid. Determine the empirical formula of ascorbic acid if it is composed of 40.92% carbon, 4.58% hydrogen, and 54.50% oxygen. A) CHO B) CH2O C) C2H3O2 D) c3h4o3 E) none of the above

answer

D) C3H4O3

question

60) Determine the correct empirical formula of a compound containing 26.68% carbon, 2.24% hydrogen, and 71.08% oxygen. A) CHO B) CHO2 C) C0.5H0.5O1 D) c2h2o4 E) none of the above

answer

B) CHO2

question

61) A compound composed of only carbon and hydrogen is 25.2% hydrogen by mass. The empirical formula for this compound is: A) CH 0.25 B) C3H C) CH4 D) C2H8 E) none of the above

answer

C) CH4

question

62) What is the molecular formula of a compound given the molar mass of the compound is 186.5 gram and the empirical formula is C2H7? A) C4H14 B) C3H21 C) C2H7 D) C2H14 E) none of the above

answer

E) none of the above

question

63) An estrogen compound with the empirical formula C12H17O2 has a molecular mass of 386.6 g/mol. What is the value of n necessary to find the molecular formula? A) 0.2 B) 1 C) 2 D) 20 E) none of the above

answer

C) 2

question

64) What is the value of n when the empirical formula is C3H5 and the molecular mass is 205.4 g/mol? A) 0.02 B) 5 C) 10 D) 140 E) none of the above

answer

B) 5

question

65) What would the empirical formula be for the molecular compound c6h9O4? A) C2H3O2 B) CH3O2 C) C3H6O2 D) C3H9O4 E) none of the above

answer

E) none of the above

question

66) What is the molecular formula of a compound given the molar mass of the compound is 30.04 gram and the empirical formula is NH? A) NH B) N2H2 C) N2H6 D) N4H4 E) none of the above

answer

B) N2H2

question

67) A compound has a molar mass of 180.18 g/mol. Given the following percent composition, calculate the molecular formula: 39.99% C, 6.73% H, 53.28% O. A) CH3O2 B) CH2O C) C3H6O3 D) C6H12O6 E) none of the above

answer

D) C6H12O6

question

68) An unknown acid has a molar mass of 60.06 g/mol. Given the following percent composition, what is the molecular formula? 40% C, 6.7% H, 53.3% O . A) C3H4O3 B) CH2O C) C2H4O2 D) C6H12O6 E) none of the above

answer

C) C2H4O2

question

69) A compound composed of only hydrogen and oxygen is 5.94% hydrogen by mass. The molar mass of this compound is 34.02 g/mol. What is the compound's molecular formula? A) 34.02 B) H2O2 C) HO D) H6O E) none of the above

answer

B) H2O2

question

1) Bananas cost 33¢ per pound. If you spent $0.77, how many pounds of bananas did you purchase? A) 2.33 B) 1.73 C) 0.429 D) 2.01 E) none of the above

answer

A) 2.33

question

2) How many atoms are present in 4.5 moles? A) 3.7 x 1023 B) 3.7 x 10-25 C) 2.7 x 1024 D) 6.02 x 1023 E) none of the above

answer

C) 2.7 x 1024

question

3) If you have 2.41 x 1024 atoms of copper, how many moles of copper do you have? A) 0.250 B) 4.00 C) 0.600 D) 3.00 E) none of the above

answer

B) 4.00

question

4) How many moles of potassium are in 156.4 g? A) 39.10 B) 4.000 C) 0.2500 D) 5.050 E) none of the above

answer

B) 4.000

question

5) What is the mass of 3.91 x 1024 sulfur atoms? A) 208 B) 4.93 C) 155 D) 32.07 E) none of the above

answer

A) 208

question

6) How many atoms of lithium are in 18.7 g? A) 2.14 x 1024 B) 2.70 x 1024 C) 1.62 x 1024 D) 3.11 x 1024 E) none of the above

answer

C) 1.62 x 1024

question

7) What is the mass (in grams) of 1.95 moles of water ? A) 18.02 B) 9.24 C) 35.1 D) 6.022 × 10 23 E) none of the above

answer

C) 35.1

question

8) What is the mass (in grams) of 3.03 × 1024 molecules of carbon dioxide molecules? A) 221 B) 0.114 C) 1.33 D) 44.01 E) none of the above

answer

A) 221

question

9) How many moles of oxygen are in 3.30 moles of NaClO4 ? A) 3.30 B) 0.303 C) 19.0 D) 13.2 E) none of the above

answer

D) 13.2

question

10) Given that sodium chloride is 39.0% sodium by mass, how many grams of sodium chloride are needed to have 950 mg of Na present? A) 2.44 B) 0.371 C) 2,430 D) 37.1 E) none of the above

answer

A) 2.44

question

11) What is the mass percent of Na in sodium chloride? A) 58.4 B) 60.7 C) 39.3 D) 47.5 E) none of the above

answer

C) 39.3

question

12) What is the mass percent of oxygen in sodium oxide? A) 37.1 B) 25.8 C) 74.2 D) 62.0 E) none of the above

answer

B) 25.8

Chapter 6 Practice Questions – Flashcards

Unlock all answers in this set

Haven't found what you were looking for?

Search for samples, answers to your questions and flashcards