Question

OKINETICS AND EQUILIBRIUM Calculating the reaction rate of one reactant from that of another CA The reform reaction between steam and gaseous methane (CH) 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 422. liters per second of methane are consumed when the reaction is run at 156. "C and 0.55 atm. 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. Y

Answer 1

Chulg) + H₂O(g) Colg) + 3 Hy (9) - - d [Chu ] I d[Ho] - dtJE a. [hq] - 3x422 = 12 66 15 puh RT h = 0.558 1266 = 19.77 moles - 0.082*429 et Mass - 19.77 x 9 = 39.54 g d [Ha] = 39.54 kg 5' = 3.95 x 10 = 2 kg s- 1000