The elementary reaction $2SO_{2(g)} + O_{2(g)} \to 2SO_{3(g)}$ is carried out in a $1 \ dm^3$ vessel and a $2 \ dm^3$ vessel separately. The ratio of the reaction velocities will be

Which of the following graphs is correct for a first order reaction $R \rightarrow P$?

Which of the following statements is correct?

For any chemical reaction,what factors do chemists aim to determine?

Half-lives of a first-order and a zero-order reaction are the same. Assume that the initial concentration of the reactant is the same for both reactions,then the ratio of the initial rates of the first-order reaction to that of the zero-order reaction is:

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 . . . . . .