The reform reaction between steam and gaseous methane ( CH4 ) produces \"synthes

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 246. liters per second of methane are consumed when the reaction is run at 230.°C and 0.35atm . 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 --> CO + 3H2

we use PV = nRT to find moles of CH4   per 1second ,   T = 230C = 230 + 273 = 503 K

0.35 atm x 246 L = n x 0.08206 liter atm/molK x 503 K

n = 2.086

H2 moles produced = 3 x CH4 moles = 3 x 2.086 = 6.258

H2 mass produced = moles x molar mass of H2 = 6.258 mol x 2 g/mol = 12.52 g = 0.0125 kg

Thus H2 produced = 0.013 kg/s               ( rounded to two digits )

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