Question

Hydrogen produced from a hydrolysis reaction was collected over water. The data is compiled in the table. Total volume of H2(g) collected 93.33 mL Temperature 26.0 °C Barometric pressure 735 mmHg Vapor pressure of water at 26.0 °C 25.5 mmHg Calculate the moles of hydrogen gas produced by the reaction. moles: mol H 2

Answer 1

Answer

0.0035496mol

Explanation

Pressure of H2 = Barometric reading - vapor pressure of water at 26.0℃  

= 735mmHg - 25.5mmHg

= 709.5mmHg

760mmHg = 1atm

709.5 mmHg =0.9336atm

Ideal gas equation is

PV = nRT

P = Pressure, 0.9336atm

V = Volume , 0.09333L

n = number of moles

R = gas constant , 0.082057(L atm/ mol K)

T = Temperature, 26℃ = 299.15K

n = PV/RT

= 0.9336atm × 0.09333L / (0.082057 L atm / mol K × 299.15K)

= 0.0035496mol