96. The graph below shows the change in 100. concentration of reactant Q with time for the reaction Q+B C. 1 101. U.4 03 0.2 102. 0.1 10 20 30 80 90 40 Time/sec. 50 60 70 The reaction is said to be a first order reaction because, 1. the gradient of a line tangent to the curve is same for two or möre points on the curve. 2. the half-life constant. 3. the half-life depends on the initial concentration. 103. LM(g) is 97. The reaction L(g) + M(g) zero order with respect to L. It may be inferred from this that; Ques 1. the reaction rate is constant. 2. the reaction takes place in one step. 3. Lis nol involved in the slow step of the reaction. Rate
96. The graph below shows the change in 100. concentration of reactant Q with time for the reaction Q+B C. 1 101. U.4 03 0.2 102. 0.1 10 20 30 80 90 40 Time/sec. 50 60 70 The reaction is said to be a first order reaction because, 1. the gradient of a line tangent to the curve is same for two or möre points on the curve. 2. the half-life constant. 3. the half-life depends on the initial concentration. 103. LM(g) is 97. The reaction L(g) + M(g) zero order with respect to L. It may be inferred from this that; Ques 1. the reaction rate is constant. 2. the reaction takes place in one step. 3. Lis nol involved in the slow step of the reaction. Rate
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Answer Q 96, 97 & 98
![100. The rate expression for a certain chemical
reaction is Rate = K[X]"[Y]". This means
the reaction is "b" order with respect to Y
96. The graph below shows the change in
concentration of reactant Q with time for the
reaction O+B > C.
1.
the reaction is "a" order with respect to Y
2.
3. the overall order of reaction is (a+b).
101. The activation energy for a reaction,
0.4
1.
is usually different for forward and
backward reactions in a reversible
reaction.
depends on the temperature of the
reaction.
3. is usually the same for forward and
reversed reaclioh in a reverisible
reaction.
2.
0.2
102. The rate law for the reaction
01
2HI -> H, +1, is directly proportional to
the square of hydrogen iodide concentration.
This means that;
1. the reaction is second order with
respect to concentration of hydrogen
iodide.
the reaction is bimolecular.
20
B0 90
40 50
Time/sec.
10
30
70
2.
The reaction is said to be a first order
reaction because,
the gradient of a line tangent to the
curve is same for two or möre points
on the curve.
the half-life constant.
3. the half-life depends on the initial
two hydrogen iodide molecules are
involved in the slow step of the reaction.
3.
1.
103. in a catalysed reaction, the catalyst,
1. remains chemically unchanged at the
end of the reaction.
2.
2. speeds up the rate of the reaction.
remains physically unchanged at the
end of the reaction.
concentration.
3.
97. The reaction L(g) + M(g) - LM(g) is
zero order with respect to L. It may be
inferred from this that;
1. the reaction rate is constant.
2. the reaction takes place in one step.
3.
Questions 104 to 106 relate to the graph below.
Lis not involved in the slow step of the
reaction.
Rate
98. Consider the reaction
H,O,(g) + HI(ag) --> 1,(aq) + 2H,0(1)
The rate of the reaction can be monitored
by measuring changes in the
1. electrical conductivity
2. colour inensity.
3. pH.
Concentration
99. The rate determining step of reaction is
1.
the slow step for the reaction.
one of its elementary reaction.
the step where the species involved
features in the rate law
104. The rate law(s) that could be associated with
curve AB is(are)
1.
2.
3.
Rate = K[B] for a single reactant.
2. Rate = KIA][B] for two reactants
3. Rate = KIAl for a single reactant
168](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F5a34b30f-b24b-4f7d-99ce-077847d6f8ed%2Fae516639-7c1a-4ef2-b2ac-7a2b8dbde692%2Fgbqpxro_processed.jpeg&w=3840&q=75)
Transcribed Image Text:100. The rate expression for a certain chemical
reaction is Rate = K[X]"[Y]". This means
the reaction is "b" order with respect to Y
96. The graph below shows the change in
concentration of reactant Q with time for the
reaction O+B > C.
1.
the reaction is "a" order with respect to Y
2.
3. the overall order of reaction is (a+b).
101. The activation energy for a reaction,
0.4
1.
is usually different for forward and
backward reactions in a reversible
reaction.
depends on the temperature of the
reaction.
3. is usually the same for forward and
reversed reaclioh in a reverisible
reaction.
2.
0.2
102. The rate law for the reaction
01
2HI -> H, +1, is directly proportional to
the square of hydrogen iodide concentration.
This means that;
1. the reaction is second order with
respect to concentration of hydrogen
iodide.
the reaction is bimolecular.
20
B0 90
40 50
Time/sec.
10
30
70
2.
The reaction is said to be a first order
reaction because,
the gradient of a line tangent to the
curve is same for two or möre points
on the curve.
the half-life constant.
3. the half-life depends on the initial
two hydrogen iodide molecules are
involved in the slow step of the reaction.
3.
1.
103. in a catalysed reaction, the catalyst,
1. remains chemically unchanged at the
end of the reaction.
2.
2. speeds up the rate of the reaction.
remains physically unchanged at the
end of the reaction.
concentration.
3.
97. The reaction L(g) + M(g) - LM(g) is
zero order with respect to L. It may be
inferred from this that;
1. the reaction rate is constant.
2. the reaction takes place in one step.
3.
Questions 104 to 106 relate to the graph below.
Lis not involved in the slow step of the
reaction.
Rate
98. Consider the reaction
H,O,(g) + HI(ag) --> 1,(aq) + 2H,0(1)
The rate of the reaction can be monitored
by measuring changes in the
1. electrical conductivity
2. colour inensity.
3. pH.
Concentration
99. The rate determining step of reaction is
1.
the slow step for the reaction.
one of its elementary reaction.
the step where the species involved
features in the rate law
104. The rate law(s) that could be associated with
curve AB is(are)
1.
2.
3.
Rate = K[B] for a single reactant.
2. Rate = KIA][B] for two reactants
3. Rate = KIAl for a single reactant
168
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