Question 1

The units of the rate constant depend on the order of the reaction.

Accepted Answer

A) True 
 B)False

Question 2

Consider the following reaction 8A(g) + 5B(g) F1F1F1S1F1F1F10 8C(g) + 6D(g)
If [C] is increasing at the rate of 4.0 mol L-1s-1, at what rate is [B] changing?

Accepted Answer

A)  -0.40 mol L-1s-1 
B)  -2.5 mol L-1s-1 
C)  -4.0 mol L-1s-1 
D)  -6.4 mol L-1s-1 
E)  none of the above, since its rate of change must be positive 
A)  -0.40 mol L-1s-1 
B)  -2.5 mol L-1s-1 
C)  -4.0 mol L-1s-1 
D)  -6.4 mol L-1s-1 
E)  none of the above, since its rate of change must be positive

Question 3

A chemical reaction of the general type
A F1F1F1S1F1F1F10 2B
is first-order, with a rate constant of 1.52 × 10-4 s-1.
a. Calculate the half-life of A.
b. Assuming the initial concentration of A is 0.067 mol L-1, calculate the time needed for the concentration to fall to 0.010 mol L-1.

Accepted Answer

Question 4

Which one of the following sets of units is appropriate for a third-order rate constant?

Accepted Answer

A)  s-1 
B)  mol L-1 s-1 
C)  L mol-1 s-1 
D)  L2 mol-2 s-1 
E)  L3 mol-3 s-1 
A)  s-1 
B)  mol L-1 s-1 
C)  L mol-1 s-1 
D)  L2 mol-2 s-1 
E)  L3 mol-3 s-1

Question 5

The rate law cannot be predicted from the stoichiometry of a reaction.

Accepted Answer

A) True 
 B)False

Question 6

In the lock and key model of enzyme action, the active site on the enzyme provides an exact fit for the substrate.

Accepted Answer

A) True 
 B)False

Question 7

A reaction is first-order with respect to the reactant R. Which of the following plots will produce a straight line?

Accepted Answer

A)  [R] vs. 1/time 
B)  1/[R] vs. time 
C)  [R]2 vs. time 
D)  1/[R]2 vs. time 
E)  ln[R] vs. time 
A)  [R] vs. 1/time 
B)  1/[R] vs. time 
C)  [R]2 vs. time 
D)  1/[R]2 vs. time 
E)  ln[R] vs. time

Question 8

Consider the following mechanism for the oxidation of bromide ions by hydrogen peroxide in aqueous acid solution. H+  + H2O2   H2O+-OH (rapid equilibrium)
H2O+-OH + Br- F1F1F1S1F1F1F10 HOBr + H2O (slow)
HOBr + H+ + Br- F1F1F1S1F1F1F10 Br2 + H2O (fast)
What is the overall reaction equation for this process?

Accepted Answer

A)  2H2O+-OH + 2Br-  F1F1F1S1F1F1F10 H2O2 + Br2 + 2H2O 
B)  2H+ + 2Br- + H2O2 F1F1F1S1F1F1F10 Br2 + 2H2O 
C)  2H+ + H2O2 + Br- + HOBr F1F1F1S1F1F1F10 H2O+-OH + Br2 + H2O 
D)  H2O+-OH + Br- + H+ F1F1F1S1F1F1F10 Br2 + H2O 
E)  none of the above 
A)  2H2O+-OH + 2Br-  F1F1F1S1F1F1F10 H2O2 + Br2 + 2H2O 
B)  2H+ + 2Br- + H2O2 F1F1F1S1F1F1F10 Br2 + 2H2O 
C)  2H+ + H2O2 + Br- + HOBr F1F1F1S1F1F1F10 H2O+-OH + Br2 + H2O 
D)  H2O+-OH + Br- + H+ F1F1F1S1F1F1F10 Br2 + H2O 
E)  none of the above

The units of the rate constant depend on the order of the reaction.

Consider the following reaction 8A(g) + 5B(g)  8C(g) + 6D(g) If [C] is increasing at the rate of 4.0 mol L^-1s^-1, at what rate is [B] changing?

A chemical reaction of the general type A  2B is first-order, with a rate constant of 1.52 × 10^-4 s^-1. a. Calculate the half-life of A. b. Assuming the initial concentration of A is 0.067 mol L^-1, calculate the time needed for the concentration to fall to 0.010 mol L^-1.

Which one of the following sets of units is appropriate for a third-order rate constant?

The rate law cannot be predicted from the stoichiometry of a reaction.

In the lock and key model of enzyme action, the active site on the enzyme provides an exact fit for the substrate.

A reaction is first-order with respect to the reactant R. Which of the following plots will produce a straight line?

Keys to the Study of Chemistry

The Components of Matter

Stoichiometry of Formulas and Equations

The Major Classes of Chemical Reactions

Gases and the Kinetic-Molecular Theory

Thermochemistry: Energy Flow and Chemical Change

Quantum Theory and Atomic Structure

Electron Configuration and Chemical Periodicity

Models of Chemical Bonding

The Shapes of Molecules

Theories of Covalent Bonding

Intermolecular Forces: Liquids, Solids, and Phase Changes

The Properties of Mixtures: Solutions and Colloids

Periodic Patterns in the Main Group Elements: Bonding, Structure, and Reactivity

Organic Compounds and the Atomic Properties of Carbon

Equilibrium: the Extent of Chemical Reactions

Acid-Base Equilibria

Ionic Equilibria in Aqueous Systems

Thermodynamics: Entropy, Free Energy, and the Direction of Chemical Reactions

Electrochemistry: Chemical Change and Electrical Work

The Elements in Nature and Industry

The Transition Elements and Their Coordination Compounds

Nuclear Reactions and Their Applications

Filters

Exam 16: Kinetics: Rates and Mechanisms of Chemical Reactions

The units of the rate constant depend on the order of the reaction.

Consider the following reaction 8A(g) + 5B(g)  8C(g) + 6D(g) If [C] is increasing at the rate of 4.0 mol L-1s-1, at what rate is [B] changing?

A chemical reaction of the general type A  2B is first-order, with a rate constant of 1.52 × 10-4 s-1. a. Calculate the half-life of A. b. Assuming the initial concentration of A is 0.067 mol L-1, calculate the time needed for the concentration to fall to 0.010 mol L-1.

Which one of the following sets of units is appropriate for a third-order rate constant?

The rate law cannot be predicted from the stoichiometry of a reaction.

In the lock and key model of enzyme action, the active site on the enzyme provides an exact fit for the substrate.

A reaction is first-order with respect to the reactant R. Which of the following plots will produce a straight line?

Consider the following mechanism for the oxidation of bromide ions by hydrogen peroxide in aqueous acid solution. H+ + H2O2 H2O+-OH (rapid equilibrium) H2O+-OH + Br-  HOBr + H2O (slow) HOBr + H+ + Br-  Br2 + H2O (fast) What is the overall reaction equation for this process?

Keys to the Study of Chemistry

The Components of Matter

Stoichiometry of Formulas and Equations

The Major Classes of Chemical Reactions

Gases and the Kinetic-Molecular Theory

Thermochemistry: Energy Flow and Chemical Change

Quantum Theory and Atomic Structure

Electron Configuration and Chemical Periodicity

Models of Chemical Bonding

The Shapes of Molecules

Theories of Covalent Bonding

Intermolecular Forces: Liquids, Solids, and Phase Changes

The Properties of Mixtures: Solutions and Colloids

Periodic Patterns in the Main Group Elements: Bonding, Structure, and Reactivity

Organic Compounds and the Atomic Properties of Carbon

Equilibrium: the Extent of Chemical Reactions

Acid-Base Equilibria

Ionic Equilibria in Aqueous Systems

Thermodynamics: Entropy, Free Energy, and the Direction of Chemical Reactions

Electrochemistry: Chemical Change and Electrical Work

The Elements in Nature and Industry

The Transition Elements and Their Coordination Compounds

Nuclear Reactions and Their Applications

Filters

Consider the following reaction 8A(g) + 5B(g)  8C(g) + 6D(g) If [C] is increasing at the rate of 4.0 mol L^-1s^-1, at what rate is [B] changing?

A chemical reaction of the general type A  2B is first-order, with a rate constant of 1.52 × 10^-4 s^-1. a. Calculate the half-life of A. b. Assuming the initial concentration of A is 0.067 mol L^-1, calculate the time needed for the concentration to fall to 0.010 mol L^-1.