The r reaction between steam and gaseous methane (CH,) produces \"synthesis gas,

Question

The r reaction between steam and gaseous methane (CH,) produces "synthesis gas," a mixture of carbon 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 733. liters per second of methane are consumed when the reaction is run at 272. °C and 0.38 atm. Calculate the rate at which dihydrogen is being produced. Give your answer in kilograms per second. Round your answer to 2 significant digits ype bere to search

Explanation / Answer

The reaction:

CH4 + H2O = CO + H2

balance

CH4 + H2O = CO + 3H2

now..

PV = nRT

n = PV/(RT) = (0.38)(733)/(0.082*(272+273)) = 6.2327 mol of methane per second

ratio is

1 mol of CH4 = 3 mol of H2

6.2327 mol of CH4/s = 3*6.2327 = 18.6981 mol of H2/s

mass = mol*MW = 18.6981*2 = 37.3962 g of H2/s

to kg --> 37.3962*10^-3 = 0.0373 kg of H2/s

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