Consider the following reaction: 2 no(g) + 2h2(g) → n2(g) + 2 h2o(g) the rate law for this reaction is first order in h2 and second order in no. what would happen to the rate if the initial concentration of no tripled while all other factors stayed the same? the rate will increase by a factor of 9. the rate will decrease by a factor of 3. the rate will double. the rate will triple. the rate will remain constant.
Answers: 3
= 2
= 1![Rate=k[NO]^2[H_2]^1](/tpl/images/0229/1480/39530.png)
![Rate'=k[3\times NO]^2[H_2]^1](/tpl/images/0229/1480/e80a2.png)
![Rate'=k[3]^2[NO]^2[H_2]^1](/tpl/images/0229/1480/b88df.png)
![Rate'=k\times 9[NO]^2[H_2]^1](/tpl/images/0229/1480/d2dcb.png)
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Consider the following reaction: 2 no(g) + 2h2(g) → n2(g) + 2 h2o(g) the rate law for this reaction...
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