Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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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![The rate of a chemical reaction depends on the concentrations of the reactants. Let's
consider the general reaction between A and B:
aA + bB = cC+ dD
The dependence of the reaction rate on the concentration of each reactant is given by the
equation called the rate law:
rate = k[A]" [B]"
where k is a proportionality constant called the rate constant. The exponent m determines
the reaction order with respect to A, and n determines the reaction order with respect to
B. The overall reaction order equals the sum of the exponents (m + n).
For example, if m =2 and n = 2 then rate
is 2 +2 = 4.
= k[A]² [B]² and the overall reaction order
The reaction orders are experimentally determined and usually not related to the reaction
stoichiometric coefficients a and b.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F3eeee35f-d659-47ef-946a-5935a7fd8b8f%2F1fc855f8-66c4-4d0a-a516-b1e946522611%2Fdh8hzr_processed.png&w=3840&q=75)
Transcribed Image Text:The rate of a chemical reaction depends on the concentrations of the reactants. Let's
consider the general reaction between A and B:
aA + bB = cC+ dD
The dependence of the reaction rate on the concentration of each reactant is given by the
equation called the rate law:
rate = k[A]" [B]"
where k is a proportionality constant called the rate constant. The exponent m determines
the reaction order with respect to A, and n determines the reaction order with respect to
B. The overall reaction order equals the sum of the exponents (m + n).
For example, if m =2 and n = 2 then rate
is 2 +2 = 4.
= k[A]² [B]² and the overall reaction order
The reaction orders are experimentally determined and usually not related to the reaction
stoichiometric coefficients a and b.
![Consider the reaction of ethyl acetate with sodium hydroxide:
CHз COOC>H (аq) + NaOH(aq) 3 CH;COONa(ag) + CәНь ОН (аq)
The reaction is first order in NaOH and second order overall. What is the rate law?
• View Available Hint(s)
O rate = k[CH3 COOC,H;]² [NaOH]²
O rate = k[CH3 COOC,H;][NAOH]²
O rate= k[NaOH]
O rate = k[CH3COOC,H;]
O rate = k[CH3 COOC,H;][NaOH]
O rate =
k[CH; COOC,H;] [N2OH]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F3eeee35f-d659-47ef-946a-5935a7fd8b8f%2F1fc855f8-66c4-4d0a-a516-b1e946522611%2Fyp59lv_processed.png&w=3840&q=75)
Transcribed Image Text:Consider the reaction of ethyl acetate with sodium hydroxide:
CHз COOC>H (аq) + NaOH(aq) 3 CH;COONa(ag) + CәНь ОН (аq)
The reaction is first order in NaOH and second order overall. What is the rate law?
• View Available Hint(s)
O rate = k[CH3 COOC,H;]² [NaOH]²
O rate = k[CH3 COOC,H;][NAOH]²
O rate= k[NaOH]
O rate = k[CH3COOC,H;]
O rate = k[CH3 COOC,H;][NaOH]
O rate =
k[CH; COOC,H;] [N2OH]
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