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Hydrogen produced from a hydrolysis reaction was collected over water and the following data was compiled....

Hydrogen produced from a hydrolysis reaction was collected over water and the following data was compiled.

Total volume of H2(g): 96.62 mL

Temp: 28.0C

Bariometric Pressure: 7.40x10^2 mmHg

Vapor pressure of water at 28C: 28.5 mmHg

Calculate the moles of hydrogen gas produced by the reaction.

Solutions

Expert Solution

According to dalton's law total pressure of gas is equal to sum of partial pressure exerted by each individual gas

Ptotal = P1 + P2 + P3

Total pressure = pressure of vapour + pressure of hydrogen

pressure of hydrogen = Total pressure - pressure of vapour = 7.40 102 - 28.5 = 711.5 mmHg

Use ideal gas equation to calculate mole of hydrogen

Ideal gas equation

PV = nRT             where, P = atm pressure= 711.5 = 0.93618 atm,

V = volume in Liter = 96.62 ml = 0.09662 L

n = number of mole = ?

R = 0.08205L atm mol-1 K-1 =Proportionality constant = gas constant,

T = Temperature in K = 280 = 273.15+ 28 = 301.15 K

We can write ideal gas equation

n = PV/RT

Substitute the value

n = (0.936180.09662)/(0.08205301.155) = 0.00366 mole

0.00366 mole of hydrogen gas produced.

queen_honey_blossom answered 2 years ago
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