What will be the rate equation for the reaction `2X + Y to Z`, if the order of the reaction is zero?

Options

A. Rate =k[X][Y]
B. Rate = k
C. Rate `= k[X]^(0)[Y]`
D. Rate = `k[X][Y]^(0)`

Explanation

To determine the rate equation for the reaction \(2X + Y \rightarrow Z\) when the order of the reaction is zero, we can follow these steps:

### Step 1: Understand the concept of zero-order reactions
In a zero-order reaction, the rate of reaction is independent of the concentration of the reactants. This means that changes in the concentration of reactants do not affect the rate of the reaction.

### Step 2: Write the general form of the rate equation
The general form of the rate equation for a reaction can be expressed as:
\[ \text{Rate} = k [X]^m [Y]^n \]
where \(k\) is the rate constant, and \(m\) and \(n\) are the orders of the reaction with respect to reactants \(X\) and \(Y\), respectively.

### Step 3: Set the orders \(m\) and \(n\) to zero
Since the reaction is zero-order, we set both \(m\) and \(n\) to zero:
\[ \text{Rate} = k [X]^0 [Y]^0 \]

### Step 4: Simplify the equation
Since any concentration raised to the power of zero is equal to 1, we can simplify the equation:
\[ \text{Rate} = k \cdot 1 \cdot 1 = k \]

### Conclusion
Thus, the rate equation for the reaction \(2X + Y \rightarrow Z\) when the order of the reaction is zero is:
\[ \text{Rate} = k \]