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Arrhenius Equation

A chemical re...

Question

A chemical reaction was carried at $300$ K and $280$ K. The rate constants were found to be $K_{1}$ and $K_{2}$ respectively, then?

K_{2} = 4 K_{1}

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K_{2} = 2 K_{1}

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K_{2} = 0.25 K_{1}

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K_{2} = 0.5 K_{1}

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Solution

The correct option is C $K_{2} = 0.25 K_{1}$
The value of rate constant gets doubled for each $10^{o} C$ rise in temperature. Thus, for $20^{o} C$ rise in temperature, the rate constant becomes 4 times.

This means $K_{1} = 4 K_{2}$

$K_{2} = \frac{K_{1}}{4} = 0.25 K_{1}$

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K_{1}

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A chemical reaction was carried out at 300K and 280K. The rate conatants were found to be K₁ and K₂ respectively. Then

1)K₂ = 4 K₁

2)K₂ =2 K₁

3)K₂ = 0.5 K₁

4)K₂ = 0.25 K₁

300 K

280 K

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