Statement 1: A large value for the equilibrium constant indicates that products are favored at equilibrium.
Statement 2: The ratio of products to reactants at equilibrium is always greater than one.

Statement 1 and Statement 2 are correct and Statement 2 is the correct explanation of Statement 1

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Both the Statement 1 and Statement 2 are correct and Statement 2 is NOT the correct explanation of Statement 1.

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Statement 1 is correct but Statement 2 is not correct.

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Statement 1 is not correct but Statement 2 is correct.

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Both the Statement 1 and Statement 2 are not correct.

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Solution

The correct option is C Statement 1 is correct but Statement 2 is not correct.
We have, $K_{e q} = \frac{K_{f}}{K_{b}}$ , $K_{f} \to$ rate constant of forward reaction
$K_{b} \to$ rate constant of backward reaction
Now, if $K_{e q}$ is very large.
$\Rightarrow K_{f} >> K_{b}$
So, rate of forward reaction will be much more than rate of backward reaction. So, products will be more favoured.

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Statement 1: A large value for the equilibrium constant indicates that products are favored at equilibrium.Statement 2: The ratio of products to reactants at equilibrium is always greater than one.

Statement 1: A large value for the equilibrium constant indicates that products are favored at equilibrium.
Statement 2: The ratio of products to reactants at equilibrium is always greater than one.