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.

Question

Chemistry

Lizzy

6 December, 02:01

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.

+4

Answers (1)

Know the Answer?

Abbie Gamble · 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.