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Question

For the reaction: 2A+BA2B the rate=k[A][B]2 with k=2.0×106 mol2L2S1. If the initial concentration of A and B are 0.1 mol L1 and 0.2 mol L1 respectively then which of the following is /are correct:

A
When A is reduced to 0.06 mol L1 then rate becomes 3.89×109 mol L1Sec1
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B
When A is reduced to 0.06 mol L1 then B will be 0.16 mol L1
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C
All are correct
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D
Initial rate of reaction is 8×109 mol L1S1
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Solution

The correct option is D Initial rate of reaction is 8×109 mol L1S1
Rate=k[A][B]2
Initial rate=2×106[0.1][0.2]2
=8×109 mol L1 sec1
Now as [A] is reduced to 0.06 mol L1 i.e. 0.04 mol L1 of [A] is reacted
2 moles A react with 1 mole B.
0.04 moles of A reacts with 0.02 moles of B
[B]left=0.20.02=0.18
rate=2×106[0.06][0.18]2=3.89×109mol2L1sec1

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