Chemical Kinetics Test

Result

Chemical Kinetics Test - 72

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Weekly Quiz Competition

Question 1
1 / -0

In a zero order reaction 47.5% of the reactant remains at the end of 2.5 hours. The amount of reactant consumed in one hour is

A
10.5%

B
32.0%

C
52.6%

D
21.0%

Solution
Question 2
1 / -0

The decomposition of A follows first order kinetics by the following equation:

$$4A (g) \xrightarrow{\Delta} B(g) + 2C(g)$$

If initially, the total pressure was $$800$$ mm of Hg and after $$10$$ minutes it is found to be $$650$$ mm of Hg. What is the half-life of A?
(Assume only A is present initially)

A
$$10$$ minutes

B
$$5$$ minutes

C
$$7.5$$ minutes

D
None of these
Question 3
1 / -0

For a reaction: nA→ product, the rate constant and rate of reactions are equal, What is the order of the reaction ?

A
0

B
1

C
2

D
3
Question 4
1 / -0

The time taken for the completion of 90% of a first order reaction is 't' min. What is the time (in sec) taken for the completion of 99% of the reaction ?

A
$$2t$$

B
$$t/30$$

C
$$120t$$

D
$$60t$$
Question 5
1 / -0

For a reaction
$$2A+B\rightarrow C+D$$, the active mass of $$B$$ is kept constant but that of $$A$$ is tripled. The rate of reaction will -

A
Decrease by $$3$$ times

B
Increased by $$9$$ times

C
Increase by $$3$$ times

D
Unpredictable

Solution

According to the given reaction, $$ Rate = k[A]^{2}[B]^{1} $$
When A becomes 3A i.e. triples, the rate will become: $$ Rate^{'} = k[3A]^{2}[B]^{1} = 9k[A]^{2}[B] $$
Thus, rate of reaction is increased by 9 times.
Question 6
1 / -0

For a homogeneous reaction $$A\rightarrow 3B$$, if pressure after sometime $$t$$ was $$P_t$$ and after completion of reaction, pressure was $$P_\infty $$.Then select the correct relation.

A
$$K \times t $$ = ln $$(\cfrac { 2P_\infty }{ 3(P_\infty -Pt) } )$$

B
$$K \times t$$ = ln $$(\cfrac {7 P_\infty }{ 3(P_\infty -Pt) } )$$

C
$$K \times t$$ = ln $$(\cfrac {3P_\infty }{ 2(P_\infty -Pt) } )$$

D
$$K \times t$$ = ln $$(\cfrac {5P_\infty }{ 2(P_\infty -Pt) } )$$

Solution
Question 7
1 / -0

The half life of a first order reaction is 30 min and the initial concentration of the reactant is 0.1 M. If the initial concentration of reactant is doubled, then the half life of the reaction will be

A
1800 s

B
60 min

C
15 min

D
1200 s

Solution
Question 8
1 / -0

The initial concentration of cane sugar in presence of an acid was reduced from $$0.20$$ to $$0.10\ M$$ in $$5$$ hours and to $$0.05\ M$$ in $$10$$ hours, what is the value of $$K$$? $$(in\ hr^{-1})$$

A
$$0.0693$$

B
$$1.386$$

C
$$0.1386$$

D
$$3.465$$
Question 9
1 / -0

The general integrated rate equation for first-order reaction is given by:

A
$$k=\cfrac{2.303}{t}ln\cfrac{[A]_{0}}{[A]_{t}}$$

B
$$k=\cfrac{1}{t}ln\cfrac{[A]_{0}}{[A]_{t}}$$

C
$$k=\cfrac{2.303}{t}log_{10}\cfrac{[A]_{0}}{[A]_{t}}$$

D
$$k=\cfrac{1}{t}ln\cfrac{[A]_{0}}{[A]_{t}}$$
Question 10
1 / -0

The concentration of $$N_{2}O_{5}$$ in liquid bromine varied with time as follows:

$$t/s$$

$$0$$

$$100$$

$$300$$

$$500$$

$$[N_{2}O_{5}]M$$

$$0.12$$

$$0.088$$

$$0.049$$

$$0.026$$

What will be the rate constant and order of reaction?

A
$$k=2\times 10^{-3}s^{-1}$$, order$$=1st$$

B
$$k=3.06\times 10^{-3}s^{-1}$$, zero

C
$$k=4\times 10^{-3}s^{-1}$$, zero

D
None of these

Solution