The reform reaction between steam and gaseous methane $(C{H}_4)$ 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 $427.$ liters per second of methane are consumed when the reaction is run at $153.C$ and the methane is supplied at $0\mathrm{.}62$atm. Calculate the rate at which dihydrogen is being produced. Give your answer in kilograms per second. Round your answer to $2$ significant digits.