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 159. liters per second of methane are consumed when the reaction is run at 294.°c and 0.86atm . 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.

The rate of the dihydrogen production is 0.0175 kg/sec for the given reaction.

The given reaction

One mole of Methane is react with one mole of water to form 1 mole of CO and 3 moles of Hydrogen.

The rate of hydrogen production can be calculated from ideal gas law

Where,

p- pressure = 0,86 atm · 101,325 kPa/atm = 87,14 kPa.

V- volume of methane =  159 L

T -  temperature= 294°C = 567 K.

R - gas constant = 8,314 J/K·mol.

n - number of moles = ?

Put the values in the formula, sole it for n,

Since, the molar ratio of methane to hydrogen is 3:1.

SO,

Hence, the mass of the dihydrogen produced,

Therefore, the rate of the dihydrogen production is 0.0175 kg/sec for the given reaction.

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i believe the answer is true.

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