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 step by step, we will 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:
\[ \text{Rate} = k [\text{NO}]^x [\text{H}_2]^y \]
where \( x \) is the order with respect to NO and \( y \) is the order with respect to H₂.

### Step 2: Analyze the Given Data
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