In which of the following case, does the reaction go fartiest to completion ifKc=102Kc=10Kc=10−2Kc=1

1. Break Down the Problem

To determine in which case the reaction goes farthest to completion, we need to analyze the given equilibrium constants (Kc) for their implications on the direction of the reaction.

1. The values of Kc provided are:
   • Kc = 10^2
   • Kc = 10
   • Kc = 10^(-2)
   • Kc = 1

2. Relevant Concepts

The value of the equilibrium constant (Kc) indicates the extent to which a reaction proceeds before reaching equilibrium. A larger Kc value suggests a greater degree of product formation:

• If Kc >> 1, the products are favored at equilibrium.
• If Kc ≈ 1, the reaction is more balanced between reactants and products.
• If Kc << 1, the reactants are favored.

3. Analysis and Detail

Let's analyze each case:

1. Kc = 10^2 (Kc = 100): A very large value indicating that the reaction will favor products significantly. The reaction will go farthest to completion.
2. Kc = 10: Indicates moderate product formation. The reaction favors products, but to a lesser extent than Kc = 100.
3. Kc = 10^(-2) (Kc = 0.01): A very small value indicating that the reaction will favor reactants, and thus, it won’t proceed far toward completion.
4. Kc = 1: Indicates that there is a balanced formation of products and reactants, thus, it does not favor completion either way.

4. Verify and Summarize

From our analysis, Kc = 100 indicates the greatest tendency toward product formation. On the contrary, Kc values of less than 1 (specifically Kc = 0.01) indicate a strong preference for reactants and do not support completion.

Final Answer

Among the given cases, the reaction goes farthest to completion in the case where Kc = 100.