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 the suitable condition for the forward reaction in a chemical equilibrium, we need to analyze the relationship between the reaction quotient (Q) and the equilibrium constant (Kc). Here’s a step-by-step solution:

### Step 1: Understand the Reaction Quotient (Q)
The reaction quotient (Q) is a measure of the relative concentrations of products and reactants at any point in time during a reaction. It is calculated using the formula:
\[ Q = \frac{[C]^c [D]^d}{[A]^a [B]^b} \]
where \([C]\) and \([D]\) are the concentrations of the products, and \([A]\) and \([B]\) are the concentrations of the reactants.

### Step 2: Analyze the Equilibrium Constant (Kc)
The equilibrium constant (Kc) is a specific value that represents the ratio of the concentrations of products to reactants at equilibrium. It is also calculated using the same formula as Q but specifically at equilibrium conditions.

### Step 3: Compare Q and Kc
- If \( Q < Kc \): This indicates that the concentration of reactants is higher compared to products, and the reaction will proceed in the forward direction to produce more products.
- If \( Q = Kc \): The system is at equilibrium, and there is no net change in the concentrations of reactants and products.
- If \( Q > Kc \): This indicates that the concentration of products is higher compared to reactants, and the reaction will favor the reverse direction to produce more reactants.

### Step 4: Identify the Suitable Condition for Forward Reaction
For the forward reaction to be favored, we need the condition where:
\[ Q < Kc \]
This means that the concentration of reactants is greater than that of products, prompting the reaction to shift towards the formation of more products.

### Conclusion
The suitable condition for the forward reaction is when:
\[ Q < Kc \]