Question

Zinc reacts with aqueous sulfuric acid to form hydrogen gas: Zn (s) + H2SO4 (aq) → ZnSO4 (aq) + H2 (g) In an experiment, 201 mL of wet H2 is collected over water at 27 °C with a total pressure of the water-hydrogen mixture of 748 torr. The vapor pressure of water at 27 °C is 26.74 torr. How many grams of Zn have been consumed?

385

3.85 × 105

0.507

4.28 × 106

507

Answer 1

= total pressure - Vapor Pressure of water Vapor pressure of H2 - 748 - 26174 = 721.2 1 = 721.26 atm = o.gug cetm Vapor pressure of H₂ (Pry) = o.gug atm Volume of H₂ = 201, mL = 0.201, L gas constant (R) = 0.082 cetm. L Molok Temp (T) = 27°C = (2 7 + 273 )k - 300k Ideal gas Law PV = nRT = PV - 2 - Prz Vez - Digug x 0,201 RT 0082 X 300 = 0.007754 mole Chemical reaction zu & Hy sou - Zn soy & M₂ 1 male H₂ Produced when I mole 2n conAumed than 0.007754 mole zinc consumed 0.007754 mole H₂ Produade Moker muss & zinc (zn) = 65.38 g/mole than mass of consumed Zinc (zu) = 65.38 x 0 1007754 (9) =0.5069 (9) = 0.507 gram