Two substances, A and B, react with each other in such a way that A is 50% consumed in 33 minutes and 75% consumed in 66 minutes. Changing the concentration of B has no effect on the result. The reaction is:
A) first order in both A and B
B) first order in A and zero order in B
C) zero in both A and B
D) zero order in A and first order in B
E) second order in A an zero order in B
Let the rate of the reaction be
Rate = K * [A]^x * [B]^y
Since the rate of the reaction is not altered by changing the concentration of B implies that the value of y must be zero, in that case [B] doesn't alter the rate of the reaction
Hence the reaction must be zero order in B
Similarly, Let the reaction be zero order in A, it can't be otherwise the reaction wouldn't have taken independent of concentration
Let the reaction wrt A be first order
ln(Ao/At) = kt
at t==33 minutes
ln2 = k * 33
k = ln2/33
at t==66 minutes
ln4 = k * 66
k = ln2/33
Hence the value of K is same therefore the reaction must be first order wrt A
Hence the correct answer is First order in A and zero order in B
Therefore, the correct answer is Option B
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