Which condition is suitable for the forward reaction?

Options

A. `Q=K_(c)`
B. `Q gt K_(c)`
C. `Q lt K_(c)`
D. `Q=0`

Answer

To determine which condition is suitable for the forward reaction, we need to understand the relationship between the reaction quotient (Q) and the equilibrium constant (Kc).

### Step-by-Step Solution:

1. **Understand the Terms**:
- **Reaction Quotient (Q)**: This is a measure of the relative amounts of products and reactants present in a reaction at any point in time. It is calculated using the same expression as the equilibrium constant but with the current concentrations of the reactants and products.
- **Equilibrium Constant (Kc)**: This is a constant that describes the ratio of the concentrations of products to reactants at equilibrium for a given reaction at a specific temperature.

2. **Identify the Reaction**:
- Consider a general reaction:
\[ A + B \rightleftharpoons C + D \]
- For this reaction, the expression for Q is:
\[ Q = \frac{[C][D]}{[A][B]} \]
- And the expression for Kc is the same but evaluated at equilibrium.

3. **Determine the Condition for Forward Reaction**:
- For the forward reaction to occur, the system must shift towards the products (C and D). This shift happens when there are more reactants (A and B) compared to products (C and D).
- Therefore, for the forward reaction to be favored, the value of Q must be less than Kc:
\[ Q < Kc \]

4. **Conclusion**:
- The suitable condition for the forward reaction is when \( Q < Kc \). This means that there are more reactants than products, prompting the reaction to proceed in the forward direction to reach equilibrium.

### Final Answer:
The suitable condition for the forward reaction is \( Q < Kc \).

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