Question

Hydrogen cyanide gas is commercially prepared by the reaction of methane [CH4(g)], ammonia [NH3(g)], and oxygen [O2(g)] at a high temperature. The other product is gaseous water.
a. Write a balanced chemical equation for the reaction.
b. Methane and ammonia gases flow into a reactor at a rate of 20.0 L/s. Oxygen gas is introduced at a flow rate of 40.0 L/s. All the reactant gases are at 1.00 atm and 150.oC. What mass of HCN is produced per second by this reaction assuming 100% yield?


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  • CreatedMay 04, 2015
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