For a reaction at `800^(@)C`
`2NO + 2H_(2) rarr N_(2) + 2H_(2)O`, the following data were obtained:
`|{:(,[NO] xx 10^(-4) (M),[H_(2)] xx 10^(-3)(M),-(1)/(2) (d[NO])/(dt) xx 10^(-4) (mol L^(-1) min^(-1))),(i.,1.5,4.0," " 4.4),(ii.,1.5,2.0," "2.2),(iii.,0.5,2.0," "0.24):}|`
What is the order of this reaction with respect to `NO` and `H_(2)` ? Also calculate the rate constant.

Explanation

To solve the problem, we need to determine the order of the reaction with respect to NO and H2, and then calculate the rate constant \( k \).

### Step 1: Write the rate law expression
The rate law for the reaction can be expressed as:
\[ \text{Rate} = k [NO]^x [H_2]^y \]
where \( x \) is the order with respect to NO and \( y \) is the order with respect to H2.
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