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  • For the reaction,  <img alt="2 \mathrm{NO}(\mathrm{g})+\mathrm{H}_{2}(\mathrm{g}) \longrightarrow \mathrm{N}_{2} \mathrm{O}(\mathrm{g})+\mathrm{H}_{2} \mathrm{O}(\mathrm{g})" src="http:

For the reaction, 
2 \mathrm{NO}(\mathrm{g})+\mathrm{H}_{2}(\mathrm{g}) \longrightarrow \mathrm{N}_{2} \mathrm{O}(\mathrm{g})+\mathrm{H}_{2} \mathrm{O}(\mathrm{g}), at 900 K following data are observed.
Initial pressure of                Initial pressure of              Initial rate of pressure
     NO (atm)                                H2 (atm)                        decrease (atm min-1)
       0.150                                    0.40                                         0.020
       0.075                                    0.40                                         0.005
       0.150                                    0.20                                         0.010
Find out the order of reaction.

Option: 1

3


Option: 2

2


Option: 3

0


Option: 4

1


Answers (1)

best_answer

Initial Rate Method to Determine Correct Rate Law and Order of Reaction -

Consider the reaction:

\mathrm{2A\: +\: B\: \rightarrow P}

The rate law for this reaction is given as follows:

\mathrm{Rate\: =\: K[a]^{x}[B]^{y}}

Now, x and y are the coefficients that are determined experimentally.

K = Rate constant
x,y = Order of reaction with respect to A and B.

Now,

\begin{array}{l}{\text { From experiments I and II, }\left[\mathrm{H}_{2}\right] \text { is constant and }[\mathrm{NO}]} \\ {\text { is doubled. Then rate becomes } 4 \text { times. }} \\ {\text { So order of reaction w.r.t. }(\mathrm{NO})=2}\end{array}
\begin{array}{l}{\text { From experiments I and III, }[\mathrm{NO}] \text { is constant, and }\left[\mathrm{H}_{2}\right] \text { is }} \\ {\text { doubled then rate becomes } 2 \text { times. So order of reaction }} \\ {\text { w.r.t. }\left(\mathrm{H}_{2}\right)=1 .} \\ {\text { Total order }=3}\end{array}

 

Posted by

Rishabh

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