# Physical and inorganic chemistry chapter 2 stoichiometry Martha Hill
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6.022 x 10^23. example: 1 mol of C =6.022 x 10^23, 1 mol of HCl= 6.022 x 10^23, 2 mol of NaCl= 2 x 6.022 x 10^23 Number of Cl- ions in 2 moles of MgCl2 = 2 x 2 x 6.022 x 10^23 Number of Mg2+ ions in 1 mol of MgCl2 = 6.022 x 10^23
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Molar mass

Atomic mass(neutron + proton) = Molar mass ( g/mol)
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Mass

Number of moles= Mass of substance(Gram) / Molar mass of substance( g/mol)
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Yield of a chemistry reaction

Percent yield =(Actual product yield/ theoretical product yield )x 100%
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Concentration

%(w/v)= g/ml , %(v/v)= ml/ml , Molarity= mol/litre
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Dilution Process

Mi x Vi = Mf x Vi . Initial molarity x initial volume = final molarity x final volume.
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Ideal gas law

pV = nRT . P= pressure, V= Volume of gas, n= number of mols of gas, R= gas constant, T= temperature of the gas (K). 1 atm=101325Pa =760mmHg .(1atm x 22.4L)/(1mol x 273K)=0.08206 (101325Pa x 0.0224m^3)/(1mol x 273K)= 8.314
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Percent composition

mass percent of each element in a compound. Mass of copper in Cu2(OH)2CO3. [2×63.55/ (63.55 x 2 + (16×1.01) + 12.01 + 16×3)]x 100% = 57.5%
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Empirical Formula