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Standard X

Chemistry

Factors Affecting the Rate of a Chemical Reaction

In the reacti...

Question

In the reaction, A + 2B $\to$ products, doubling the concentration of B (keeping the concentration of A unchanged) increases the rate of reaction by:

four times

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two times

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half times

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eight times

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Solution

The correct option is A four times
For the given reaction; $A + 2 B \to$ Products
Rate, $r =$ $k [A] [B]^{2}$
Now if [B] is doubled & [A] is constant;
New rate $r^{^{'}} = k [A] [2 B]^{2} = 4 k [A] [B]^{2} = 4 r$
Thus, the rate increases by four times.

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In the reaction, A + 2B → products, doubling the concentration of B (keeping the concentration of A unchanged) increases the rate of reaction by:

The correct option is A four timesFor the given reaction; A+2B→ ProductsRate, r=k[A][B]2Now if [B] is doubled & [A] is constant; New rate r′=k[A][2B]2=4k[A][B]2=4rThus, the rate increases by four times.

In the reaction, A + 2B $\to$ products, doubling the concentration of B (keeping the concentration of A unchanged) increases the rate of reaction by:

The correct option is A four times
For the given reaction; $A + 2 B \to$ Products
Rate, $r =$ $k [A] [B]^{2}$
Now if [B] is doubled & [A] is constant;
New rate $r^{^{'}} = k [A] [2 B]^{2} = 4 k [A] [B]^{2} = 4 r$
Thus, the rate increases by four times.