From the expression of the following reactions, determine order of reaction and the dimensions of the rate constant.
(i) `3NO(g)rarrN_2O(g)+NO_2(g) " Rate"=k[NO]^2`
(ii) `H_2O_2(aq)+3l^(-)(aq)+2H^+rarr2H_2O(l)+l_3^(-)" Rate"= k[H_2O_2][l]`
(iii) `CH_3CHO(g) rarrCH_4(g)+CO(g)+CO(g)" Rate" =k[CH_3CHO]^(3//2)`
(iv) `C_2H_5Cl(g)rarrC_2H_4(g)+HCl(g)" Rate"=k[C_2H_5Cl]`

Explanation

To determine the order of the reaction and the dimensions of the rate constant for each of the provided reactions, we will analyze the given rate equations step by step.

### (i) Reaction: `3NO(g) → N2O(g) + NO2(g)`
**Rate Equation:** Rate = k[NO]^2

1. **Determine the order of the reaction:**
The order of the reaction is the sum of the powers of the concentration terms in the rate equation. Here, the power of [NO] is 2.
**Order = 2**
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