Question

Hydrogen produced from a hydrolysis reaction was collected over water. The data is compiled in the table. Total volume of H2(g) collected 96.02 mL. Temperature 23.0°C Barometric pressure 735 mmHg Vapor pressure of water at 23.0 °C 21.0 mmHg Calculate the moles of hydrogen gas produced by the reaction. moles: mol

Answer 1

Answer

0.003712 mol

Explanation

Partial pressure of H2 = Barometric pressure - vapor pressure of water at 23.0℃

Partial pressure of H2 = 735mmHg - 21.0mmHg = 714mmHg = 0.9395atm

Number of moles of H2 is calculated by ideal gas equation

PV = nRT

P = Pressure , 0.9395atm

V= Volume , 96.02ml = 0.09602L

n = number of moles

R = gas constant, 0.82057(L atm/mol K)

T = Temperature , 23℃ = 296.15K

n = PV/RT

= 0.9395atm × 0.09602L / ( 0.082057(L atm/mol K) × 296.15K)

= 0.003712mol