If the rate equation for a reaction is $\frac{dx}{dt}=k[H]^{1/2}[B]^{1/2}$, the order of reaction is:
- A2
- B$\frac{1}{2}$
- C$\frac{3}{2}$
- ✓1
Answer: D.
View full solution →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.
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6
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01
M.C.Q (1 Marks)
33 Q→021 Marks Question
6 Q→032 Marks Questions
8 Q→043 Marks Question
8 Q→055 Marks Questions
5 Q→064 Marks Questions
1 Q→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.
The unit of rate constant of a second order reaction is :
- Amol $L^{-1}sec^{-1}$
- B$mol^{-1}L^{-1}sec^{-1}$
- ✓$mol^{-1}L~sec^{-1}$
- D$\operatorname{mol} L \sec ^{-1}$
Answer: C.
View full solution →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.
View full solution →Who gave the theory of ionisation?
- AFaraday
- ✓Arrhenius
- COstwald
- DRutherford
Answer: B.
View full solution →The rate of zero order reaction $A+B \longrightarrow C$ is :
- ✓Rate $= K [ A ]^0[B]^0$
- BRate $= K [ A ]^1[B]^0$
- CRate $= K [ A ]^0[B]^1$
- DNone of these
Answer: A.
View full solution →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?
View full solution →The rate constant for first order reaction is 0.0005 $min^{-1}$. Calculate its half-life.
View full solution →If in a chemical reaction $A+B \rightarrow Product$ rate low is given by $R=K[A]^{1/2}[B]^{3/2}$ find the order of reaction.
View full solution →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?
View full solution →Define threshold energy.
A first order reaction takes 40 min for 30% decomposition calculate $t_{1/2}$.
View full solution →What is the effect of temperature on the rate constant of reaction? How can this temperatures effect on rate constant be represented quantitatively?
Analyse the given graph, drawn between concentration of reactant vs. time.
(a) Predict the order of reaction.
(b) Theoretically, can the concentration of the reactant reduce to zero after infinite time? Explain.
(a) Predict the order of reaction.
(b) Theoretically, can the concentration of the reactant reduce to zero after infinite time? Explain.
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 $N _2 O _{5(g) \text {. }}$
View full solution →What is the order of a reaction?
Calculate the half-life of a first order reactions from their rate constants given below :
(a) $200~s^{-1}$
(b) $2~min^{-1}$
(c) $4~year^{-1}$
View full solution →(a) $200~s^{-1}$
(b) $2~min^{-1}$
(c) $4~year^{-1}$
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 $1.5\times10^{10}s^{-1}$?
View full solution →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?
View full solution →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?
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).
View full solution →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:
Calculate its rate constant at 410 sec and 1130 sec. What does these result show?
View full solution →| Time $(t) \sec$ | 0 | 80 | 160 | 410 | 600 | 1130 | 1720 |
| $\left[ N _2 O _2\right] mol /$ litre | 5.5 | 5.0 | 4.8 | 4.0 | 3.4 | 2.4 | 1.6 |
Calculate its rate constant at 410 sec and 1130 sec. What does these result show?
For the decomposition of azoisopropane to hexane and nitrogen at 543 K , the following data is obtained :
Calculate the rate constant.
View full solution →| $t( sec )$ | $P$ (mm of Hg ) |
| 0 | 35.0 |
| 360 | 54.0 |
| 720 | 63.0 |
Calculate the rate constant.
A first order reaction takes 30 min for 50% completion, what would be time for its 90% completion.
What do you understand by rate of a reaction? What factors affect the rate of a reaction? Discuss.
Find the expression for first order reaction###How will you know that a reaction is of first order.
What is the difference between order of a reaction and its molecularity?
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 $R =8.314 J K ^{-1} mol^{-1}$)
View full solution →( given $R =8.314 J K ^{-1} mol^{-1}$)
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