Please help! The reform reaction between steam and gaseous methane (CH_4) produc

Question

Please help!

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 989. liters per second of methane are consumed when the reaction is run at 204. Degree C and 0.14 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

The balanced reaction between CH4 and steam is given by

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

1 mole of CH4 produces 3 moles of hydrogen is prodced.

One has to find out the number of moles of CH4 to calculate the moles of hydrogen produced

from PV= nRT , P= 0.14 atm , V= 989 L/s T= 204 deg.c =204+273.15=477.15 K, R=0.08206 L.atm/mole.K

n=PV/RT= 0.14*989/(477.15*0.08206)=3.54 mol/s

So moles of hydrogen produced =3.54*3/1= 10.62 mol/s

Mole = mass/Molecular weight

Mass= moles* Molecular weight

mass of hydrogen =10.62*2 kg/S =21.24 kg/s

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