K for the reaction `2A+B⇌2C` is `1.5×10^12` .This indicates that at equilibrium the concentration of ______ would be maximum.

Options

A. A
B. B
C. C
D. None

Answer

To solve the question regarding the equilibrium constant \( K \) for the reaction \( 2A + B \rightleftharpoons 2C \), we need to analyze the implications of the given value of \( K \).

### Step-by-Step Solution:

1. **Understanding the Reaction**: The reaction is given as \( 2A + B \rightleftharpoons 2C \). This indicates that two moles of reactant \( A \) and one mole of reactant \( B \) produce two moles of product \( C \).

2. **Equilibrium Constant Expression**: The equilibrium constant \( K \) for this reaction can be expressed as:
\[ K = \frac{[C]^2}{[A]^2[B]} \]
where \([C]\), \([A]\), and \([B]\) are the molar concentrations of the respective species at equilibrium.

3. **Given Value of K**: The problem states that \( K = 1.5 \times 10^{12} \). This is a very large value.

4. **Interpreting the Value of K**: A large value of \( K \) indicates that at equilibrium, the concentration of products is much greater than that of the reactants. Specifically, since \( K \) is significantly greater than 1, it suggests that the formation of products \( C \) is favored.

5. **Conclusion**: Since the equilibrium constant \( K \) is very high, it implies that at equilibrium, the concentration of product \( C \) will be maximum compared to the concentrations of reactants \( A \) and \( B \).

### Final Answer:
At equilibrium, the concentration of **C** would be maximum.