The reaction `2H_2O_2 to 2H_2O + O_2` is a

Options

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

Answer

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

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

we need to follow these steps:

### Step 1: Identify the reactants and products
The reactant in this reaction is hydrogen peroxide (H₂O₂), and the products are water (H₂O) and oxygen (O₂).

### Step 2: Write the rate law expression
The rate law for a reaction can be expressed as:

\[ \text{Rate} = k [\text{Reactant}]^n \]

where \( k \) is the rate constant, \( [\text{Reactant}] \) is the concentration of the reactant, and \( n \) is the order of the reaction with respect to that reactant.

### Step 3: Determine the order of the reaction
In this case, the reaction involves the decomposition of hydrogen peroxide. The stoichiometric coefficients in the balanced equation can give us an initial idea about the order of the reaction.

For the reaction:

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

The coefficient of H₂O₂ is 2. This suggests that the reaction is second order with respect to H₂O₂.

### Step 4: Calculate the overall order of the reaction
The overall order of the reaction is the sum of the powers of the concentration terms in the rate law. Since we have:

- H₂O₂ with a coefficient of 2, we consider it as \( [H_2O_2]^2 \).

Thus, the overall order of the reaction is:

\[ \text{Order} = 2 \]

### Conclusion
The order of the reaction \( 2H_2O_2 \rightarrow 2H_2O + O_2 \) is **2**, indicating that it is a second-order reaction.

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