Chemical Kinetics

$$\begin{gathered} \mathrm{For} \mathrm{the} \mathrm{reaction}, \\ 5{\mathrm{Br}}^{-}\left(\mathrm{aq}\right) + {\mathrm{BrO}}_3^{-}\left(\mathrm{aq}\right) + 6{\mathrm{H}}^{+}\left(\mathrm{aq}\right) \to 3{\mathrm{Br}}_2\left(\mathrm{aq}\right) + 3{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right) \\ \mathrm{If}, -\frac{∆\left[{\mathrm{Br}}^{-}\right]}{∆\mathrm{t}}= 0.05 \mathrm{mol} {\mathrm{L}}^{-1} {\min }^{-1}, -\frac{∆\left[{\mathrm{BrO}}_3^{-}\right]}{∆\mathrm{t}} \mathrm{in} {\mathrm{molL}}^{-1} {\min }^{-1} \mathrm{is} \end{gathered}$$

• 0.005

• 0.05

• 0.5

• 0.01

For the reaction $5{\mathrm{Br}}^{-}\left(\mathrm{aq}\right) + 6{\mathrm{H}}^{+}\left(\mathrm{aq}\right) + {\mathrm{BrO}}_3^{-} \to 3{\mathrm{Br}}_2\left(\mathrm{aq}\right) + 3{\mathrm{H}}_2\mathrm{O} \left(\mathrm{l}\right) \mathrm{if}, -\frac{∆\left[{\mathrm{BrO}}_3^{-}\right]}{∆\mathrm{t}}= 0.01 \mathrm{mol} {\mathrm{L}}^{-1}{\min }^{-1}, \frac{∆\left[{\mathrm{Br}}_2\right]}{∆\mathrm{t}}\mathrm{in} \mathrm{mol} {\mathrm{L}}^{-1}{\min }^{-1}\mathrm{is}$

• 0.01

• 0.3

• 0.03

• 0.005

The half-life of Th²³² is 1.4 × 10¹⁰ years and that of its daughter element Ra²³⁸ is 7 years. What amount (most nearly) weight of Ra²³⁸ will be in equilibrium with 1 gm of Th²³²?

• 5.0 gm

• 1.95 × 10^-9 gm

• 2 × 10^-10 gm

• 5 × 10^-10 gm

Which of the following are the correct representations of a zero order reaction, where A represents the reactant?

• I, II, III

• I, II, IV

• II, III, IV

• 1, III, II

Which of the following statement(s) is/are true

• The pressure of a fixed amount of an ideal gas is proportional to its temperature only

• Frequency of collision increases in proportion to the square root of temperature

• The value of van der Waal's constant'a' is smaller for ammonia than for nitrogen

• If a gas is expanded at constant temperature, the kinetic energy of the molecules decrease

For the reaction 2A + B → C, the values of initial rate at different reactant concentrations are given in the table below. The rate law for the reaction is :

• Rate = k[A]²[B]²

• Rate = k[A]²[B]

• Rate = k[A][B]

• Rate = k[A][B]²

For a reaction scheme A $\stackrel{{\mathrm{k}}_1}{\to } \mathrm{B} \stackrel{{\mathrm{k}}_2}{\to }\mathrm{C}$, if the rate of formation of B is set to be zero then the concentration of B is given by:

• (k₁ + k₂)[A]

• (k₁ - k₂)[A]

• $\left(\frac{{\mathrm{k}}_1}{{\mathrm{k}}_2}\right)\left[\mathrm{A}\right]$

• k₁k₂[A]

The given plots represent the variation of the concentration of a reactant R with time for two different reactions (i) and (ii). The respective orders of the reactions are

• 0, 1

• 0, 2

• 1, 0

• 1, 1

A bacterial infection in an initial wound grows N₀(t) = N₀ exp(t), here the time t is in hours A dose of antibiotic, taken orally , needs 1 hour to reach the wound. Once it reaches there , the bacterial Population goes down as $\frac{\mathrm{dN}}{\mathrm{dt}}= -5{\mathrm{NH}}^2$ . what will be plot of $\frac{{\mathrm{N}}_0}{\mathrm{N}}\mathrm{Vs} \mathrm{t} \mathrm{after} 1 \mathrm{hour}$

For the reaction of H₂ with I₂, the rate constant is 2.5 × 10^-4 dm³ mol^-1s^-1 at 327°C and 1.0 dm³ mol^-1s^-1 at 527°C. The activation energy for the reaction, in kJ mol^-1 is: (R= 8.314 Jk^-1mol^-1)

• 166

• 150

• 59

• 72