For the reaction- Ag-2Bg- 2Cg- the rate constants for the forward and the reverse reactions are 1- 10-4 and 2-5- 10-2 respectively- The value of equilibrium constant- K for the reaction would be-

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Effective Equilibrium Constant

For the react...

Question

For the reaction, $A_{(g)} + 2 B_{(g)} ⇌ 2 C_{(g)}$ , the rate constants for the forward and the reverse reactions are $1 \times 10^{- 4}$ and $2.5 \times 10^{- 2}$ respectively. The value of equilibrium constant, K for the reaction would be-

1 \times 10^{- 4}

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2.5 \times 10^{- 2}

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4 \times 10^{- 3}

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2.5 \times 10^{2}

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Solution

The correct option is C $4 \times 10^{- 3}$
The equilibrium reaction is $A_{(g)} + 2 B_{(g)} ⇌ 2 C_{(g)} .$
The expression for the equilibrium constant is $K = \frac{k_{f}}{k_{b}} .$
Substitute values in the above expression.
$K = \frac{1 \times 10^{- 4}}{2.5 \times 10^{- 2}} = 4 \times 10^{- 3} .$

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For the reaction, A(g)+2B(g)⇌2C(g), the rate constants for the forward and the reverse reactions are 1×10−4 and 2.5×10−2 respectively. The value of equilibrium constant, K for the reaction would be-

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For the reaction, $A_{(g)} + 2 B_{(g)} ⇌ 2 C_{(g)}$ , the rate constants for the forward and the reverse reactions are $1 \times 10^{- 4}$ and $2.5 \times 10^{- 2}$ respectively. The value of equilibrium constant, K for the reaction would be-