Question

Rate is expressed in $mol{L}^{-1}mi{n}^{-1}$
In the above reaction, the order is:

	$A+B\to C$
	[A]	[B]	[C]
1	1.0	1.0	0.25
2	2.0	1.0	0.50
3	1.0	2.0	0.25

• A. Zero in A and one in B
• B. One in A and zero in B
• C. One in both A and B
• D. Zero in both A and B

Answer 1

The correct option is B One in A and zero in B

Now, If we see row 1 and row 2. We can see by doubling the concentration of A will double the product.so we can say A is following $r=K_1[A{]}^1$.
Hence A is 1st order
In row 2 and row 3, concentration of B is doubled but product concentration is still the same. So we can say that reaction follows $Rate=k[B{]}^0$. Here as the power of B is zero,product concentration is independent of B
B zeroth order