Question

The reform reaction between steam and gaseous methane ( ch4 ) produces "synthesis gas," a mixture of carbon monoxide gas and dihydrogen gas. synthesis gas is one of the most widely used industrial chemicals, and is the major industrial source of hydrogen. suppose a chemical engineer studying a new catalyst for the reform reaction finds that 159. liters per second of methane are consumed when the reaction is run at 294.°c and 0.86atm . calculate the rate at which dihydrogen is being produced. give your answer in kilograms per second. be sure your answer has the correct number of significant digits.

Answer 1

Answer is: rate of production of hydrogen is 0,01758 kg/s.
Chemical reaction: CH₄ + H₂O → CO + 3H₂.
V(CH₄) = 159 L.
p = 0,86 atm · 101,325 kPa/atm = 87,14 kPa.
T = 294°C = 567 K.
R = 8,314 J/K·mol.
Ideal gas law: p·V = n·R·T.
n(CH₄) = p·V  ÷ R·T.
n(CH₄) = 87,14 kPa · 159 L ÷ 8,314 J/K·mol · 567 K.
n(CH₄) = 2,93 mol.
From chemical reaction: n(CH₄) : n(H₂) = 1 : 3.
n(H₂) = 2,93 mol · 3 = 8,79 mol.
m(H₂) = 8,79 mol · 2 g/mol.
m(H₂) = 17,58 g · 0,001 kg/g = 0,01758 kg.