Rates of Reaction

The factors which influence the rate of reaction are :

Concentration: Greater the concentrations of the reactants, faster is the rate of reaction.

Temperature: The rate of reaction increases with increase in temperature. For most of the reactions, the rate of reaction becomes almost double with 10o rise in temperature.

Presence of catalyst: A catalyst generally increases the speed of a reaction.

Answer the following question :

A small increase in temperature of the reacting system, the rate of reaction exceed to large extend. The most appropriate reason for this is-

Explain enzyme as a drug target.

How to define substrate.

The term $\frac{-\mathrm{dc}}{\mathrm{dt}}$ in a rate equation refers to:

For a given reaction $\mathrm{A} \to \mathrm{B}$, rate of disappearance of $\mathrm{R}$ $= \frac{∆\left[\mathrm{R}\right]}{ ∆\left[\mathrm{t}\right]}$.

Thermal decomposition of ${\mathrm{N}}_2{\mathrm{O}}_5$ occurs as per the equation below :

$2{\mathrm{N}}_2{\mathrm{O}}_5\to 4{\mathrm{NO}}_2+{\mathrm{O}}_2$

The correct statement is

For the reaction, $2{\mathrm{SO}}_2+{\mathrm{O}}_2\rightleftharpoons 2{\mathrm{SO}}_3$, the rate of disappearance of ${\mathrm{O}}_2$ is $2\times {10}^{-4} \mathrm{mol} {\mathrm{L}}^{-1} {\mathrm{s}}^{-1}$ . The rate of appearance of ${\mathrm{SO}}_3$ is

For a reaction: ${\mathrm{N}}_2+3{\mathrm{H}}_2\to 2{\mathrm{NH}}_3$, the rate of reaction with respect to ${\mathrm{NH}}_3$will be:

For the reaction, ${\mathrm{N}}_2+3{\mathrm{H}}_2\to 2{\mathrm{NH}}_3$, if $\frac{\mathrm{d}\left[{\mathrm{NH}}_3\right]}{\mathrm{dt}}=2\times {10}^{-4} \mathrm{mol}/\mathrm{L}/\mathrm{s}$, the value of $-\frac{\mathrm{d}\left[{\mathrm{H}}_2\right]}{\mathrm{dt}}$ would be

Higher the activation energy of a reaction, faster is the reaction.

The rate of a multistep reaction is determined by the fastest step in the sequence.

Nitrogen tetraoxide  $\left({\mathrm{N}}_2{\mathrm{O}}_4\right)$ decomposes as
                   ${\mathrm{N}}_2{\mathrm{O}}_4\left(\mathrm{g}\right)\to 2 {\mathrm{NO}}_2\left(\mathrm{g}\right)$

If the pressure of ${\mathrm{N}}_2{\mathrm{O}}_4$ falls from $0.50 \mathrm{atm}$ to $0.32 \mathrm{atm}$ in $30$ minutes, the rate of appearance of ${\mathrm{NO}}_2\left(\mathrm{g}\right)$ is:

Activation energy of a chemical reaction can be determined by ______.

A small increase in temperature of the reacting system, the rate of reaction exceed to large extend. The most appropriate reason for this is-

The rate of a chemical reaction can be expressed in terms of

Consider the reaction $2\mathrm{NO}\left(\mathrm{g}\right)+{\mathrm{O}}_2\left(\mathrm{g}\right)⟶2{\mathrm{NO}}_2\left(\mathrm{g}\right)$. If $\frac{\mathrm{d}\left[{\mathrm{NO}}_2\right]}{\mathrm{dt}}=0.052\mathrm{M}/\mathrm{s}$ then $-\frac{\mathrm{d}\left[{\mathrm{O}}_2\right]}{\mathrm{dt}}$ will be 

The instantaneous rate of reaction $2\mathrm{A}+\mathrm{B}$$\to \mathrm{C}+3\mathrm{D}$ is given by:

In the reaction $\mathrm{A}+3\mathrm{B}⟶2\mathrm{C},$ the rate of formation of $\mathrm{C}$ is