UNIVERSITY OF NEW ENGLAND CHEM 1011 WEEKS 5-7 EXAM QUESTIONS & ANS… EXAM
P R O F E S S I O N A L P R A C T I C E M AT E R I A L S
University of New England
CHEM 1011 Weeks 5-7 Exam
Questions & Answers 2026-
2027 (Rationales)
Verified Answers Exam Ready With Rationales
32 QUESTIONS
DOCUMENT OVERVIEW
This document contains 32 exam questions with correct answers and detailed rationales related to
fundamental concepts in chemistry. It is suitable for reinforcing understanding of chemical equilibrium,
reaction quotients, and acid-base theories. Students can utilize this resource for effective study,
comprehensive review, and preparation for certification exams.
CONTENTS
01 Chemical Equilibrium Q1–Q9
02 Reaction Quotients Q10–Q12
03 Acid-Base Theory Q13–Q21
Page 1
, 04 Dissolution Reactions Q22–Q25
05 Properties of Solutions Q26–Q29
06 Buffers and Indicators Q30–Q32
E XA M Q U EST I O N S
Q1 QUESTION 1 OF 32
For the reaction F2(g) ⇌ 2 F(g), the equilibrium constant at 223 °C is 7.3 x 10-13. If a sample of F2 is heated to
223 °C and allowed to reach equilibrium
CORRECT ANSWER
nearly all of F2 will remain unreacted, with a very small amount of F present
RATIONALE
A very small equilibrium constant indicates that the formation of products is highly unfavorable, favoring the
reactants instead; thus, at equilibrium, almost all of the F2 will remain unreacted, resulting in minimal F production.
This illustrates the principle of dynamic equilibrium where the concentrations of reactants and products stabilize at
a ratio dictated by the equilibrium constant.
Q2 QUESTION 2 OF 32
At equilibrium
CORRECT ANSWER
the rate of the forward reaction is equal to the rate of the reverse reaction and the concentration of the
reactants and products can be very different
RATIONALE
At equilibrium, dynamic stability occurs when the rates of the forward and reverse reactions are equal, allowing for
constant concentrations of reactants and products, although their absolute amounts may vary significantly. This
concept illustrates the principle of reversibility in chemical reactions, emphasizing that equilibrium does not imply
equal concentrations but rather a balance of reaction rates.
Page 2
P R O F E S S I O N A L P R A C T I C E M AT E R I A L S
University of New England
CHEM 1011 Weeks 5-7 Exam
Questions & Answers 2026-
2027 (Rationales)
Verified Answers Exam Ready With Rationales
32 QUESTIONS
DOCUMENT OVERVIEW
This document contains 32 exam questions with correct answers and detailed rationales related to
fundamental concepts in chemistry. It is suitable for reinforcing understanding of chemical equilibrium,
reaction quotients, and acid-base theories. Students can utilize this resource for effective study,
comprehensive review, and preparation for certification exams.
CONTENTS
01 Chemical Equilibrium Q1–Q9
02 Reaction Quotients Q10–Q12
03 Acid-Base Theory Q13–Q21
Page 1
, 04 Dissolution Reactions Q22–Q25
05 Properties of Solutions Q26–Q29
06 Buffers and Indicators Q30–Q32
E XA M Q U EST I O N S
Q1 QUESTION 1 OF 32
For the reaction F2(g) ⇌ 2 F(g), the equilibrium constant at 223 °C is 7.3 x 10-13. If a sample of F2 is heated to
223 °C and allowed to reach equilibrium
CORRECT ANSWER
nearly all of F2 will remain unreacted, with a very small amount of F present
RATIONALE
A very small equilibrium constant indicates that the formation of products is highly unfavorable, favoring the
reactants instead; thus, at equilibrium, almost all of the F2 will remain unreacted, resulting in minimal F production.
This illustrates the principle of dynamic equilibrium where the concentrations of reactants and products stabilize at
a ratio dictated by the equilibrium constant.
Q2 QUESTION 2 OF 32
At equilibrium
CORRECT ANSWER
the rate of the forward reaction is equal to the rate of the reverse reaction and the concentration of the
reactants and products can be very different
RATIONALE
At equilibrium, dynamic stability occurs when the rates of the forward and reverse reactions are equal, allowing for
constant concentrations of reactants and products, although their absolute amounts may vary significantly. This
concept illustrates the principle of reversibility in chemical reactions, emphasizing that equilibrium does not imply
equal concentrations but rather a balance of reaction rates.
Page 2
