The rate of a chemical reaction increases by catalyst due

Options

A. Reacting with reactants
B. Increasing the activation energy
C. Decreasing the activation energy
D. Reacting with products

Answer

To solve the question regarding how a catalyst increases the rate of a chemical reaction, we can break it down into the following steps:

### Step 1: Understand the Role of a Catalyst
A catalyst is a substance that increases the rate of a chemical reaction without being consumed in the process. It achieves this by providing an alternative reaction pathway.

**Hint:** Remember that catalysts are not consumed in the reaction; they facilitate the reaction.

### Step 2: Activation Energy Concept
Every chemical reaction requires a certain amount of energy to proceed, known as the activation energy (Ea). The higher the activation energy, the slower the reaction rate.

**Hint:** Think of activation energy as the energy barrier that must be overcome for a reaction to occur.

### Step 3: Effect of a Catalyst on Activation Energy
A catalyst lowers the activation energy required for a reaction. By doing so, it allows more reactant molecules to have enough energy to undergo the reaction at a given temperature.

**Hint:** Lowering the activation energy increases the number of successful collisions between reactant molecules.

### Step 4: Conclusion
Since the catalyst provides an alternative pathway with a lower activation energy, the rate of the chemical reaction increases.

**Hint:** Focus on the relationship between activation energy and reaction rate when considering the effect of catalysts.

### Final Answer
The rate of a chemical reaction increases by a catalyst due to the decrease in activation energy.

**Correct Option:** C