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Arrhenius Equation

The rate cons...

Question

The rate constants of a reaction at 300K & 280K respectively are $K_{1}$ & $K_{2}$ . Then:

K_{1} = 20 K_{2}

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K_{2} = 4 K_{1}

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K_{1} = 4 K_{2}

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K_{1} = 0.5 K_{2}

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Solution

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

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K_{1}

K_{2}

300 K

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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

E_{a_{1}}

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k_{1} > k_{2}

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