Rate of a Chemical Reaction

In a pseudo first order hydrolysis of ester in water, the following results are obtained:

(i) The average rate of reaction between the time interval 30 to 60 seconds and

(ii) The pseudo first order rate constant for the hydrolysis of ester is?

The rate of reaction for $\mathrm{A}\to \mathrm{Products}$ is $10 \mathrm{moles}/\mathrm{lit}/\mathrm{minute}$ when ${\mathrm{t}}_1=2 \min$. The rate of reaction when ${\mathrm{t}}_2=12 \min$, in the same unit is ;

Which is correct regarding moderate reactions

Formation of fossil fuels is a moderate reaction.

What is moderate reaction?

Which of the following is a moderate reaction?

Inversion of cane sugar in aqueous solution is an example of moderate reaction.

For a given reaction $3\mathrm{A}\mathrm{ }+\mathrm{B}\to \mathrm{C}+\mathrm{D}$ the rate of reaction can be represented by

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

Units of rate of a reaction is $\mathrm{mol} {\mathrm{L}}^{-1}$.

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

The instantaneous rate of reaction depends on the change in concentration of an infinity small time interval, expressed as the limit or derivation of expression.

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: