Statement 1 : KP=KC for all reversible reaction.Statement 2 : At constant temperature, the pressure of the gas is proportional to its concentration.

# Statement 1 : ${\mathrm{K}}_{\mathrm{P}}={\mathrm{K}}_{\mathrm{C}}$ for all reversible reaction.Statement 2 : At constant temperature, the pressure of the gas is proportional to its concentration.

1. A

If both Statement 1 and Statement 2 are true but statement 2 is the correct explanation of the statement 1.

2. B

If both Statement 1 and Statement 2 are true but statement 2 is not the correct explanation of the statement 1.

3. C

If Statement 1 is true but Statement 2 is false.

4. D

If Statement 1 is false but Statement 2 is true.

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### Solution:

Statement 1 is false but statement 2 is true.

${\mathrm{K}}_{\mathrm{P}}\ne {\mathrm{K}}_{\mathrm{C}}$ for all reaction

${\mathrm{K}}_{\mathrm{P}}={\mathrm{K}}_{\mathrm{C}}{\left(\mathrm{RT}\right)}^{∆\mathrm{n}}$

$∆\mathrm{n}=$number of moles of products - number of moles of reactants in the balanced chemical equation.

So, if for a reaction $∆\mathrm{n}=$0. Then ${\mathrm{K}}_{\mathrm{P}}={\mathrm{K}}_{\mathrm{C}}$

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