Question

Hydrogen produced from a hydrolysis reaction was collected over water. The data is compiled in the table. Total volume of H2(g) collected 94.91 mL 28.0 °C Temperature Barometric pressure 744 mmHg Vapor pressure of water at 28.0 °C 28.5 mmHg Calculate the moles of hydrogen gas produced by the reaction moles: 327.897 mol H2

Answer 1

Given ,

Barometric pressure = 744 mmHg

Vapor pressure of water vapor = 28.5 mmHg

So vapor pressure of H2(P) = 744 mmHg- 28.5 mmHg

= 715.5 mmHg = 0.94 atm (as 1 atm = 760mmHg)

Volume(V) = 94.91ml = 0.09491L

T= 28C = 301K

Using gas equation, PV = nRT

R is universal gas constant = 0.0821 atmL/mol.K

n= PV/RT

On solving se get,

n = 0.0036 moles H2 (Answer)