Explain nitrogen monoxide reacts with hydrogen gas

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Reference no: EM13521798

Nitrogen monoxide reacts with hydrogen gas to form nitrogen gas and water (vapor). Write a balanced equation for this reaction. The reaction is experimentally found to be first order in H2 and second-order in NO. Write down the form of the experimentally-determined rate law and the units of the rate constant if the concentrations are in mol/L. Now the reaction is believed to take place in three steps, the first of which is the fast reversible dimerization of NO to form N2O2, and the last of which (again fast) is the reaction N20 + H2 --> N2 + H2O. So, what is the slow (second) step? Then show, using the steady-state approximation, that the mechanism is consistent with the observed rate law. Why is it only approximately true that the reaction is first-order in H2?

Reference no: EM13521798

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