If the value of equilibrium constant for a particular reaction is`1.6xx10^(12)` , then art equilibrium the system will contain

Options

A. all reactants
B. mostly reactants
C. mostly products
D. similar amounts of reactants and products

Explanation

To solve the problem, we need to analyze the implications of the given equilibrium constant (K) value for a reaction.

### Step 1: Understanding the Equilibrium Constant
The equilibrium constant (K) for a reaction at equilibrium is defined as the ratio of the concentrations of the products to the concentrations of the reactants, each raised to the power of their coefficients in the balanced equation.

### Step 2: Setting Up the Reaction
Let's consider a hypothetical reaction:
\[ aA \rightleftharpoons bB \]
The equilibrium constant expression for this reaction can be written as:
\[ K_c = \frac{[B]^b}{[A]^a} \]

### Step 3: Substituting the Given Value
Given that \( K_c = 1.6 \times 10^{12} \), we can interpret this value. A very high value of K (much greater than 1) indicates that at equilibrium, the concentration of products (B) is much greater than the concentration of reactants (A).

### Step 4: Analyzing the Implications
Since \( K_c \) is significantly greater than 1, we can conclude that:
\[ [B] \gg [A] \]
This means that at equilibrium, the system will predominantly contain the products rather than the reactants.

### Step 5: Conclusion
Thus, based on the high value of the equilibrium constant, we can conclude that at equilibrium, the system will contain mostly products.

### Final Answer
At equilibrium, the system will contain mostly products.

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