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

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 924 liters per second of methane are consumed when the reaction is run at 261°C and 0.96atm. Calculate the rate at which dihydrogen is being produced. Give your answer in kilograms per second. Round your answer to 2 significant digits.

The rate at which dihydrogen is being produced is 0.12 kg/sec

Explanation:

The balanced chemical equation is ;

According to ideal gas equation:

P = pressure of gas = 0.96 atm

V = Volume of gas = 924 L

n = number of moles

R = gas constant =

T =temperature =

According to stoichiometry:

1 mole of methane produces = 3 moles of hydrogen

Thus 20.2 moles of methane produces = moles of hydrogen

Mass of hydrogen =

Thus the rate at which dihydrogen is being produced is 0.12 kg/sec

first one is the correct answer