Answer: Option (d) is the correct answer.
Explanation:
Rate law is the rate which is in equilibrium with the concentration of reactants raised to the power of their coefficients.
For example, [tex]xA + yB \rightarrow zC[/tex]
Rate, r = k [tex][A]^{x} \times [B]^{y}[/tex] ........ (1)
So, when concentration of A is doubled then rate of reaction also doubles. Hence, then rate law will be as follows.
2r = k [tex][2A]^{x} \times [B]^{y}[/tex] ......... (2)
Dividing equation (1) by (2) we get the following.
[tex]\frac{r}{2r}[/tex] = [tex]\frac{k[A]^{x} \times [B]^{y}}{k[2A]^{x} \times [B]^{y}}[/tex]
Therefore, cancelling common factors we get the following.
[tex]\frac{1}{2} = \frac{1}{2x}[/tex]
[tex]2^{x}[/tex] = 2
x = 1
Thus, we can conclude that in the reaction A + B C, doubling the concentration of A doubles the reaction rate and doubling the concentration of B does not affect the reaction rate then rate of reaction will be as follows.
rate = k[A]
