A proposed mechanism for the oxidation of nitric oxide to
nitrog...

Question

A proposed mechanism for the oxidation of nitric oxide to 
nitrogen dioxide was described in Problem 14.29. Another 
possible mechanism for this reaction is 
2 NO1g2  k1 
k-1 
N2O21g2 Faster, reversible 
N2O21g2 + O21g2 ¡ k2 2NO21g2 Slower, rate-determining 
(a) Write a balanced equation for the overall reaction.

Accepted Answer

Hello. In this problem, we are asked to provide the balanced chemical equation for the overall reaction of the following mechanism. So to come up with the balanced equation we need to cancel things that appear on opposite sides. So we see that we have sulfur trioxide on the product side and then on the reactant side on the product side it has two moles of sulfur trioxide, and on the reactant side it only has one. So in order to get them to balance, we need to have a coefficient of two in front of both of them. So we are going to multiply this second reaction, everything by two. So let's write our reactions out then. So we'll have to sulfur dioxide because oxygen Goes to two moles of sulfur trioxide and the multiplying the next equation, everything by two, we get two moles of sulfur trioxide Plus two moles of water, supposed to form two moles of sulfuric acid. And so now our two moles of sulfur trioxide will cancel. And now we combine everything that appears on the reactive side together and then everything that appears on the product side together. So we get two moles of S. 02 dioxide gas plus oxygen Plus two moles of water Goes to form two moles of sulfuric acid. And so at this point in time it's also a good idea to go back through and double check this equation to ensure that everything is indeed balanced. Thanks for watching. Hope this helps

Watch next