For the reaction: ${\mathrm{H}}_2 + {\mathrm{I}}_2 \to 2\mathrm{HI},$ the differential rate law is

• $-\frac{\mathrm{d} \left[{\mathrm{H}}_2\right]}{\mathrm{dt}}=-\frac{\mathrm{d} \left[{\mathrm{I}}_2\right]}{\mathrm{dt}}=2\frac{\mathrm{d}\left[\mathrm{HI}\right]}{\mathrm{dt}}$

• $-\frac{\mathrm{d} \left[{\mathrm{H}}_2\right]}{\mathrm{dt}}=-2\frac{\mathrm{d} \left[{\mathrm{I}}_2\right]}{\mathrm{dt}}=\frac{\mathrm{d}\left[\mathrm{HI}\right]}{\mathrm{dt}}$

• $-\frac{\mathrm{d} \left[{\mathrm{H}}_2\right]}{\mathrm{dt}}=-\frac{\mathrm{d} \left[{\mathrm{I}}_2\right]}{\mathrm{dt}}=\frac{\mathrm{d}\left[\mathrm{HI}\right]}{\mathrm{dt}}$

• $-\frac{\mathrm{d} \left[{\mathrm{H}}_2\right]}{\mathrm{dt}}=\frac{\mathrm{d} \left[{\mathrm{I}}_2\right]}{\mathrm{dt}}=\frac{\mathrm{d}\left[\mathrm{HI}\right]}{\mathrm{dt}}$

Which is a correct integrated rate equation?

• $\mathrm{k} = -\frac{2.303}{\mathrm{t}} \log \frac{\mathrm{a}}{\mathrm{a} - \mathrm{x}}$

• $\mathrm{k} = \frac{-2.303}{\mathrm{t}} \log \frac{\mathrm{a} - \mathrm{x}}{\mathrm{a}}$

• - d (a - x) = kdt

• All are integrated rate equations

373.

For which order reaction, the unit of rate constant is time^-1?

• Zero order

• First order

• Second order

• Third order

For a first order reaction, the half-life period is

• dependent on the square of the initial concentration

• dependent on first power of initial concentration

• dependent on the square root of initial concentration

• independent on initial concentration

A radioactive isotope having t_1/2 = 3 days was read after 12 days. If 3g of isotope is contained in container, the initial weight of isotope was

• 12g

• 24g

• 36g

• 48g

After how many seconds will the concentration of the reactant in a first order reaction be halved if the rate constant is 1.155 x 10^-3 s^-1?

• 600

• 100

• 60

• 10

For a reaction, $\mathrm{A} + 2\mathrm{B} \to \mathrm{C}, \mathrm{rate} \mathrm{is} \mathrm{given} \mathrm{by} +\frac{\mathrm{d}\left[\mathrm{C}\right]}{\mathrm{dt}}= \mathrm{k} \left[\mathrm{A}\right] \left[\mathrm{B}\right],$hence, the order of the reaction is

• 3

• 2

• 1

• 0

In a multistep reaction, the overall rate of reaction is equal to the

• rate of slowest step

• rate of fastest step

• average rate of various step

• the rate of last step

The first order integrated rate equation is

• k = $\frac{\mathrm{x}}{\mathrm{t}}$

• k = $\frac{2.303}{\mathrm{t}} \log \frac{\mathrm{a}}{\mathrm{a} - \mathrm{x}}$

• k = $\frac{1}{\mathrm{t} } \ln \frac{\mathrm{a}}{\mathrm{a} - \mathrm{x}}$

• k = $\frac{1}{\mathrm{t}}\frac{\mathrm{x}}{\mathrm{a}(\mathrm{a} - \mathrm{x})}$

For nuclear fusion reactions, the fusion temperature is of the order of

• 10⁵ K

• 10³ K

• 10⁷ K

• 100 K