Worksheet Questions Extraction

Calculate the molecular mass of glucose, where the molecular formula is C6H12O6. Express your answer in atomic mass units.

• 180.16 u

• 176.12 u

• 182.00 u

• 168.00 u

A compound contains 4.07% hydrogen, 24.27% carbon, and 71.65% chlorine by mass. Its molar mass is 98.96 g. Determine both the empirical formula and the molecular formula of the compound.

• Empirical formula CHCl; molecular formula C2H2Cl2

• Empirical formula CH2Cl; molecular formula C2H4Cl2

• Empirical formula C2HCl2; molecular formula C4H2Cl4

• Empirical formula CCl; molecular formula C2Cl2

Calculate the amount of water (g) produced by the combustion of 16 g of methane.

• 18 g

• 36 g

• 9 g

• 72 g

How many moles of methane are required to produce 22 g of CO2 after combustion?

• 0.25 mol

• 0.50 mol

• 1.00 mol

• 2.00 mol

50.0 kg of N2 (g) and 10.0 kg of H2 (g) are mixed to produce NH3 (g). Calculate the amount of NH3 (g) formed and identify the limiting reagent in the production of NH3 in this situation.

• 56.1 kg NH3 formed; H2 is the limiting reagent

• 29.7 kg NH3 formed; N2 is the limiting reagent

• 85.0 kg NH3 formed; H2 is the limiting reagent

• 56.1 kg NH3 formed; N2 is the limiting reagent

A solution is prepared by adding 2 g of a substance A to 18 g of water. Calculate the mass per cent of the solute.

• 5%

• 10%

• 18%

• 20%

Calculate the molarity of NaOH in the solution prepared by dissolving its 4 g in enough water to form 250 mL of the solution.

• 0.1 M

• 0.2 M

• 0.4 M

• 0.8 M

The density of 3 M solution of NaCl is 1.25 g mL^{-1}. Calculate the molality of the solution.

• 1.50 m

• 2.00 m

• 2.79 m

• 3.75 m

Calculate the molar mass of H2O. Use standard atomic masses: H = 1.008 g mol−1, O = 16.00 g mol−1.

• 16.00 g mol−1

• 18.02 g mol−1

• 20.02 g mol−1

• 34.02 g mol−1

Calculate the molar mass of CO2. Use standard atomic masses: C = 12.01 g mol−1, O = 16.00 g mol−1.

• 28.01 g mol−1

• 30.01 g mol−1

• 44.01 g mol−1

• 48.02 g mol−1