Which of the following relations is correct for the given reaction orders?

An endothermic reaction with a high activation energy for the forward reaction is represented by the diagram:

For a chemical reaction,the temperature is increased from $25\,^{\circ}C$ to $55\,^{\circ}C$. The rate of reaction will change by a factor of (Assume $\mu = 3$).

Determine whether the following statements are True or False:
$(a)$ The rate of reaction can be decreased by decreasing the concentration of reactant.
$(b)$ Graphite quickly changes to Diamond.
$(c)$ The rate of corrosion of iron is fast.
$(d)$ The meaning of kinesis in Greek is movement.

The reaction $A \xrightarrow{K} \text{Product}$ is zero order while the reaction $B \xrightarrow{K} \text{Product}$ is first order. For what initial concentration of $A$,the half-lives of the two reactions will be equal?

Given below are two statements:
Statement $I$: The rate law for the reaction $A + B \rightarrow C$ is rate $(r) = k[A]^2[B]$. When the concentration of both $A$ and $B$ is doubled,the reaction rate is increased "$x$" times.
Statement $II$: The figure shows the variation in concentration against time plot for a "$y$" order reaction.
Concentration of $R$ vs Time plot: $A$ straight line with a negative slope equal to $-K$.
The value of $x + y$ is . . . . . .