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The mechanism of the reaction 2NO(g)+...

The mechanism of the reaction
`2NO(g)+H_(2)(g)rarrN_(2)(g)+2H_(2)O(g)`, is:
Step1: `2NO(g)+H_(2)(g)overset(("slow"))rarrN_(2)+H_(2)O_(2)`
Step2: `H_(2)O_(2)+H_(2)overset("fast")rarr2H_(2)O`

A

rate `=k[NO]^2[H_2]^2`

B

rate = `k[H_2O_2][H_2]`

C

on doubling the concentration of `H_2` , keeping the concentration of NO constant , the rate will become double

D

If the initial concentration of `H_2` and NO is `C_2` and after time 't' the concentration of `N_2` is x , then rate `=(C_0-2x)^x`

Text Solution

Verified by Experts

The correct Answer is:
C
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For the reaction mechanism of the reaction {:(2NO(g),+,2H_(2)(g)),(to N_(2)(g),+,2H_(2)O(g)):} {:("Step I",2NO,overset(k_(1))hArr,N_(2)O_(2),,,K_(eq)"(fast)"),("Step II",N_(2)O_(2)+H_(2),overset(k_(2))rarr,N_(2)O+H_(2)O,,"(slow)"),("Step III",N_(2)O+H_(2),overset(k_(3))rarrr,N_(2)+H_(2)O,,"(fast)"):} Expression of rate of reaction is (Take K_(eq) xx k_(2) = k')

In the reaction 2H_(2)(g) + O_(2)(g) rarr 2H_(2)O (l), " "Delta H = - xkJ

Determining the rate law from a mechanism with an initial slow step: Ozone reacts with nitrogen dioxide to produce oxygen and dinitrogen pentoxide O_(3)(g)+2NO_(2)(g)rarrO_(2)(g)+N_(2)O_(5)(g) The proposed mechanism is O_(3)(g)+NO_(2)(g)overset(slow)rarr NO_(3)(g)+O_(2)(g) NO_(3)(g)+NO_(2)(g)overset("fast")rarrN_(2)O_(5)(g) What is the rate law predicted by this mechanism ? Strategy : The designations "slow" and "fast" indicate the relative rates of the steps. The rate is determined completely by the slow step, or rate-determining sterp.

The reaction 2H_2O(l)rarr2H_2(g)+O_2(g) is an example of

2H_(2)+O_(2)to2H_(2)O 2 g H_(2) and 1 g O_(2) react to form H_(2)O

For the reaction 2H_(2) + 2NO rarr N_(2) + 2H_(2)O , the following mechanism has been suggested : 2NO ? N_(2)O_(2) equilibrium constant K_(1) (fast) N_(2)O_(2) +H_(2) overset(k_(2)) rarr N_(2)O +H_(2)O (slow) N_(2) O +H_(2) overset(k_(3)) rarr N_(2)+H_(2)O (fast) Establish the rate law for given reaction.

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