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For a homogeneous decomposition of N(2)O...

For a homogeneous decomposition of `N_(2)O_(5)` into `NO_(2)" and "O_(2)`,
`2N_(2)O_(5)(g)to4NO_(2)(g)+O_(2)(g)," rate "=(-(1)/(2)Delta[N_(2)O_(5)])/(Deltat)=k[N_(2)O_(5)]`
Find out the order with respect to `N_(2)O_(5)`.

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AI Generated Solution

To determine the order of the reaction with respect to \( N_2O_5 \) for the given decomposition reaction, we can follow these steps: ### Step 1: Write the balanced chemical equation The decomposition of \( N_2O_5 \) is given by the equation: \[ 2 N_2O_5(g) \rightarrow 4 NO_2(g) + O_2(g) \] ...
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For a reaction, 2N_(2)O_(5)(g) to 4NO_(2)(g) + O_(2)(g) rate of reaction is:

For the first order reaction 2N_(2)O_(5)(g) rarr 4NO_(2)(g) + O_(2)(g)

The rate law for the decompoistion of gaseous N_(2)O_(5) , N_(2)O_(5)(g) rarr 2NO_(2)(g) + (1)/(2)O_(2)(g) is observed to be: r = (-d[N_(2)O_(5)])/(dt) = k[N_(2)O_(5)] A reaction machanism which has been suggested to be conisstent with this rate law is N_(2)O_(5)(g) overset(k_(eq))hArr NO_(2)(g)+NO_(3)(g) ("fast equilibrium") NO_(2) (g) + NO_(3)(g) overset(k_(1))rarr NO_(2)(g) + NO(g) + O_(2)(g) (slow) NO(g) + NO_(3)(g) overset(k_(2))rarr 2NO_(2)(g) (fast)

2N_(2)O_(5) rarr 4NO_(2) + O_(2) If (-d[N_(2)O_(5)])/(dt) = k_(1)[N_(2)O_(5)] (d[NO_(2)])/(dt) = k_(2)[N_(2)O_(5)] (d[O_(2)])/(dt) = k_(3)[N_(2)O_(5)] What is the relation between k_(1), k_(2) , and k_(3) ?

In the decompoistion of N_(2)O_(5)(g) , 2N_(2)O_(5)(g)overset(k_(obs))rarr4NO_(2)(g) + O_(2)(g) , the observed rate law is given by (d[O_(2)])/(dt) = k_(obs)[N_(2)O_(5)] . Which of the following proposed mechanics is conisstent with the rate law?