The reaction `2H_(2)O_(2) rarr 2H_(2)O+O_(2)` is
`r=k[H_(2)O_(2)]`

Options

A. Zero order reaction
B. First order reaction
C. Second order reaction
D. Third order reaction

Explanation

To determine the order of the reaction given by the equation:

\[ 2H_2O_2 \rightarrow 2H_2O + O_2 \]

with the rate law expressed as:

\[ r = k[H_2O_2] \]

we can follow these steps:

### Step 1: Identify the Rate Law
The rate law for the reaction is given as:

\[ r = k[H_2O_2] \]

This indicates that the rate of the reaction depends on the concentration of hydrogen peroxide \([H_2O_2]\).

### Step 2: Determine the Order of the Reaction
The order of a reaction is determined by the sum of the powers of the concentration terms in the rate law. In this case, the rate law shows that the concentration of \([H_2O_2]\) is raised to the power of 1.

### Step 3: Calculate the Overall Order
Since the only reactant in the rate law is \([H_2O_2]\) with an exponent of 1, the overall order of the reaction is:

\[ \text{Order} = 1 \]

### Conclusion
Thus, the reaction \(2H_2O_2 \rightarrow 2H_2O + O_2\) is a first-order reaction.

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