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Test: Rate of a Chemical Reaction - Chemistry MCQ


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10 Questions MCQ Test Physical Chemistry - Test: Rate of a Chemical Reaction

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Test: Rate of a Chemical Reaction - Question 1

How many times will the rate of the elementary reaction 3X + Y → X2Y change if the concentration of the substance X is doubled and that of Y is halved?

Detailed Solution for Test: Rate of a Chemical Reaction - Question 1

Since it is an elementary reaction, its rate law r1= k [A] 3[B]
When the concentrations are changed the new rate will be r2= k (2[A])3([B]/2) = 4k[A]3[B]
So, r2=4r1.

Test: Rate of a Chemical Reaction - Question 2

What is the rate law for acid hydrolysis of an ester such as CH3COOC2H5 in aqueous solution?

Detailed Solution for Test: Rate of a Chemical Reaction - Question 2

Acid hydrolysis of ester, CH3COOC2H5 + H2O → CH3COOH + C2H5OH
The order of the reaction may be altered sometimes by taking reactant in excess compared to the other.
The rate law R= k [CH3COOC2H5] [H2O] however water is present in excess.
So, R= k [CH3COOC2H5].

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Test: Rate of a Chemical Reaction - Question 3

The reaction NO2 + CO → NO + CO2 takes place in two steps. Find the rate law.
2NO2 → NO + NO3 (k1) – slow
NO3 + CO → CO2 + NO2 (k2) – fast

Detailed Solution for Test: Rate of a Chemical Reaction - Question 3

In any reaction the slowest step is the rate determining step, the rate of the overall reaction depends on this step. So, 2NO2 → NO + NO3(k1) is the rate determining step. Therefore the rate law R= k1[NO2]2.

Test: Rate of a Chemical Reaction - Question 4

The rate constant of a reaction is k=3.28 × 10-4 s-1. Find the order of the reaction.

Detailed Solution for Test: Rate of a Chemical Reaction - Question 4

Given,
k= 3.28 × 10-4 s-1
The general formula to find the units for rate constant, k=(mol L-1)1-ns-1 where n is the order of the reaction. The value of n must be 1 for (mol L-1)1-ns-1 to become s-1. Therefore, k=3.28 × 10-4s-1 represents a first order reaction.

Test: Rate of a Chemical Reaction - Question 5

The decomposition of NH3 on platinum surface is zero order reaction. If k = 2.5 × 10-4 mol L-1s-1 the rate of production of H2 is

Detailed Solution for Test: Rate of a Chemical Reaction - Question 5

Test: Rate of a Chemical Reaction - Question 6

What is the concentration of the reactant in a first order reaction when the rate of the reaction is 0.6 s-1 and the rate constant is 0.035?

Detailed Solution for Test: Rate of a Chemical Reaction - Question 6

Given, R=0.6 s-1 and k= 0.035
For a first order reaction R= k [A]

Test: Rate of a Chemical Reaction - Question 7

For the reaction A + H2O → products, find the rate of the reaction when [A] = 0.75 M, k= 0.02.

Detailed Solution for Test: Rate of a Chemical Reaction - Question 7

Given,
[A] = 0.75 M, k= 0.02
The reaction belongs to pseudo first order reaction so, the unit is s-1
R= k [A]= 0.02 × 0.75= 0.015 s-1.

Test: Rate of a Chemical Reaction - Question 8

For a reaction A +B → C, the experimental rate law is found to be R=k[A]1[B]1/2. Find the rate of the reaction when [A] = 0.5 M, [B] = 0.1 M and k=0.03.

Detailed Solution for Test: Rate of a Chemical Reaction - Question 8

Given, [A] = 0.5 M, [B] = 0.1 M and k= 0.03
From the rate law it is evident that the order of the reaction is 1+ 0.5 = 1.5 = 3/2
Therefore the unit of k= (mol L-1)1-1.5 s-1 = (L/mol)1/2 s-1
R= k[A]1[B]1/2 = 0.03 × 0.5 × 0.11/2 = 4.74 × 10-2(L/mol)1/2 s-1.

Test: Rate of a Chemical Reaction - Question 9

For a second-order reaction, what is the unit of the rate of the reaction?

Detailed Solution for Test: Rate of a Chemical Reaction - Question 9

the unit of the rate of the reaction is Lmol-1s-1.
For a second order reaction, rate=k[A]2
molL−1s−1=k(molL−1)2
k=Lmol−1s−1

Test: Rate of a Chemical Reaction - Question 10

The rate law for the reaction involved in inversion of cane sugar is R=k [C12H22O11] [H2O].

Detailed Solution for Test: Rate of a Chemical Reaction - Question 10

The reaction for the inversion of cane sugar is C12H22O11 + H2O → glucose + fructose.
In this reaction water is present in excess and belongs to a pseudo first order reaction, even though the molecularity is 2 the order of the reaction is 1 so the rate law R=k[C12H22O11].

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