The reform reaction between steam and gaseous methane (CH_4) produces \"synthesi

Question

The reform reaction between steam and gaseous methane (CH_4) 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 349. liters per second of methane are consumed when the reaction is run at 294. degree C and 0.89 atm. Calculate the rate at which dihydrogen is being produced. Give your answer in kilograms per second. Round your answer to 2 significant digits.

Explanation / Answer

CH4 + H2O --------------------> 3H2 + CO

volume = 349 L

temeprature = 294 + 273 = 567 K

Pressure = 0.89 atm

n = pV / RT

n = 0.89 x 349 / 0.0821 x 567

n = 6.67

moles of methane = 6.67

1 mole CH4 ------------------->3 mol H2

6.67 mole CH4 ---------------> 3 x 6.67 = 20 molH2

mass of H2 = 20 x 2 = 40 g

mass of H2 = 0.040 kg / sec

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