For a zero-order reaction, the plot of concentration of reactant versus time is:

The rate of a certain reaction follows the expression $r = k[X]^2[Y]$. If the concentration of X is doubled and the concentration of Y is halved, how will the initial rate change?

The addition of a catalyst during a chemical reaction alters which of the following quantities

The enzyme catalysed reaction is faster than metal catalysed reaction because its activation energy is:

The rate of a chemical reaction depends upon:

For a chemical reaction $2X + Y o Z$, the rate of appearance of $Z\;is\;0.05\;{\rm{mol}}\;{{\rm{L}}^{ - 1}}{\rm{.}}$ The rate of disappearance of $X$ will be

The rate of a reaction is described by $r = k[C]^3[D]$. What will be the effect on the rate if the concentration of C is halved while the concentration of D is kept constant?

In the reaction

${\rm{BrO}}_3^ - \left( {aq} \right) + 5{\rm{B}}{{\rm{r}}^ - }\left( {aq} \right) + 6{{\rm{H}}^ + } o 3{\rm{B}}{{\rm{r}}_2}\left( l \right) + 3{{\rm{H}}_2}{\rm{O}}\left( l \right)$

The rate of appearance of bromine $({\rm{B}}{{\rm{r}}_2})$ is related to rate of disappearance of bromide ions as following:

For the non-equilibrium process, $A + B o products$, the rate is first order with respect to $A$ and second order respect to $B$. If $1.0\;mole$ each of $A$ and $B$ are introduced into a 1 litre vessel and the initial rate was $1.0 imes {10^{ - 2}}\;{\rm{mol}}/{\rm{litre}}\;\;{\rm{sec}}{\rm{.}}$ The rate (in ${\rm{mol}}\;{\rm{litr}}{{\rm{e}}^{ - 1}}{\sec ^{ - 1}}$ ) when half of the reactants have been used:

A radioactive isotope decays by first-order kinetics. If its initial activity is $1000 \, cpm$ and its rate constant is $0.05 \, day^{-1}$, what will be its activity after 10 days?

The reason for almost doubling the rate of reaction on increasing the temperature of the reaction system by $10^\circ C$ is