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Chemical Kinetics Chemistry - Chemical Kinetics

Bihar Board (BSEB) - STD 12 Science - Chemistry (BSEB - English Medium). 61 questions in this chapter.

Question types

Chemical Kinetics question types

61 questions across 6 question groups — pick any mix to generate a Chemistry paper with step-by-step answer keys.

61
Questions
6
Question groups
5
Question types
Sample Questions

Chemical Kinetics questions

One sample from each question group in this chapter. Select any group above to see the full set with answer keys.

Q 1M.C.Q [1M]1 Mark
Which of the following is not a first order reaction?
  • A
    $CH _3 COOCH _3+ H _2 O \xrightarrow{ H ^{+}} CH _3 COOH + CH _3 OH$
  • ✓
    $CH _3 COOC _2 H _5+ NaOH \rightarrow CH _3 COONa + C _2 H _5 OH$
  • C
    $2 H _2 O _2 \rightarrow 2 H _2 O + O _2$
  • D
    $2 N_2 O _5 \rightarrow 4 NO _2+ O _2$

Answer: B.

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Q 2M.C.Q [1M]1 Mark
The unit of rate constant of a second order reaction is :
  • A
    mol $L^{-1}sec^{-1}$
  • B
    $mol^{-1}L^{-1}sec^{-1}$
  • ✓
    $mol^{-1}L~sec^{-1}$
  • D
    $\operatorname{mol} L \sec ^{-1}$

Answer: C.

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Q 3M.C.Q [1M]1 Mark
If the rate equation for a reaction is $\frac{dx}{dt}=k[H]^{1/2}[B]^{1/2}$, the order of reaction is:
  • A
    2
  • B
    $\frac{1}{2}$
  • C
    $\frac{3}{2}$
  • ✓
    1

Answer: D.

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Q 61 Marks Question1 Mark
The rate constant for a first order reaction is $60~s^{-1}$. How much time will it take to reduce the initial concentration of the reactant to its 1/16th value?
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Q 91 Marks Question1 Mark
The rate of a reaction becomes four times on increasing temperature from 293 K to 313 K. Find out the activation energy of the reaction assuming it does not change with temperature. ($R=8.314$ J $K^{-1}mol^{-1}$ log 2 = 0.3010)
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Q 101 Marks Question1 Mark
For the reaction $A\rightarrow B,$ the rate of reaction becomes 27 times when the concentration of A is increased 3 times. What is the order of the reaction?
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Q 13Short Answer Type Questions [2M]2 Marks
Analyse the given graph, drawn between concentration of reactant vs. time.
Image
(a) Predict the order of reaction.
(b) Theoretically, can the concentration of the reactant reduce to zero after infinite time? Explain.
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Q 14Short Answer Type Questions [2M]2 Marks
For the reaction, $2 N_2 O _{5(g)} \rightarrow 4 NO _{2(g)}+ O _{2(g)}$, the rate of formation of $NO _{2(g)}$ is $2.8 \times 10^{-3} ms^{-1}$. Calculate the rate of disappearance of $N _2 O _{5(g) \text {. }}$
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Q 163 Marks Question3 Marks
The decomposition of A into product has value of k as $4.5\times10^{3}s^{-1}$ at $10^{\circ}C$ and energy of activation $60~kJ~mol^{-1}$. At what temperature would k be $1.5\times10^{10}s^{-1}$?
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Q 183 Marks Question3 Marks
For a reaction $2 H _2 O _2 \frac{ I ^{-}}{\text {alkaline medium }} 2 H _2 O + O _2$
the proposed mechanism is as given below:
(1) $H_{2}O_{2}+I^{-}\rightarrow H_{2}O+IO^{-}$ (slow)
(2) $H_{2}O_{2}+IO^{-}\rightarrow H_{2}O+I^{-}+O_{2}$ (fast)
(i) Write rate law for the reaction.
(ii) Write the overall order of reaction.
(iii) Out of steps (1) and (2), which one is rate determining step?
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Q 193 Marks Question3 Marks
A first order reaction is 50% completed in 40 minutes at 300 K and in 20 minute at 320 K. Calculate the activation energy of the reaction. (Given: log 2=0.3010, log 4=0.6021, $R=8.314$ $J~K^{-1}$ mol).
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Q 203 Marks Question3 Marks
The decomposition of $N _2 O _5$ in $CCl _4$ solution follows the first order rate law. The concentration of $N _2 O _5$ measured at different time intervals are given ahead:
Time $(t) \sec$08016041060011301720
$\left[ N _2 O _2\right] mol /$ litre5.55.04.84.03.42.41.6

Calculate its rate constant at 410 sec and 1130 sec. What does these result show?
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Q 264 Marks Questions4 Marks
The rate constant for the first order decomposition of $H_{2}O_{2}$ is given by the following equation: $log~k=14.2-\frac{1.0\times10^{4}K}{T}$. Calculate $E_a$ for this reaction and rate constant k if its half-life period be 200 minute.
( given $R =8.314 J K ^{-1} mol^{-1}$)
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