Supplemental Instruction
Iowa State University / Leader: / Olivia
Course: / CHEM 178
Instructor: / Miller
Date:
Chapter 14
1. For the reaction
a. Write the relationship between the rate of disappearance of NO and the rate of appearance of N2.
b. What is the rate law if the reaction is first order with respect to H2 and second order with respect to NO?
2.For each of the following gas-phase reactions, indicate how the rate of disappearance of each reactant is related to the rate of appearance of each product.
a. H2O2(g)→ H2(g) + O2(g)
b. 2N2O(g) →2N2(g) + O2(g)
c. N2(g) + 3H2(g) → 2NH3(g)
3. Using the rate law expression found in question 1, predict the effect if:
a. The concentration of NO is doubled
b. The concentration of NO is reduced by two-thirds
c. The temperature is reduced
4. Given the following data for the reaction determine the rate law for the reaction.
[CF3] initial (M) / [H2] initial (M) / Rate (M/s)0.10 / 0.10 / 45
0.15 / 0.10 / 67.5
0.20 / 0.20 / 180
0.20 / 0.30 / 270
5. An alteration in the structure of a certain virus follows first-order kinetics with an activation energy of 587 kJ/mol. The half-life of the reaction at 29.60C is 1.62x104 s (1 yr = 3.154x107s). What are the rate constant at 29.60C and the half-life at 320C for the alteration of structure of the virus?
Chapter 15
1. Write Kc expressions for the following reactions:
a.
b.
c.
d.
2. A closed container at 250C is charged with N2O4 a partial pressure of 0.54 atm, and NO2 at a partial pressure of 0.50 atm at equilibrium. What is Kp?
3. Given the equation:
N2(g) + 3H2(g) ⇌ 2NH3(g)
- What will happen if we increase pressure?
- What will happen if we increase volume?
4. Determine how the equilibrium will shift if the following changes are made:
2Cl2(g) + 2H2O(g) 4HCl(g) + O2(g) (deltaHo = +113 kJ)
a. Temperature is increased
b. Volume is increased
c. Pressure is increased
d. HCl is added
f. Cl2 is added
g. H2O is removed
Multiple Choice Questions:
1. The type of chemical equilibrium exemplified by the following reaction is:
BaSO4(s) BA2+(aq) + SO42-(aq)
a. Chemical equilibrium
b. Haber
c. Heterogeneous
d. Homogeneous
e. Mass action
2. The position of equilibrium for the reaction
ZnO(s) + H2(g) Zn(s) + H2O(g)
does not depend upon which of the following: (1) concentration of ZnO(s); (2) concentration of H2(g); (3) concentration of Zn(s); (4) concentration of H2O(g); (5) the value of Kc?
a. (1), (2), (5)
b. (2), (3), (5)
c. (1), (3)
d. (2), (4)
e. (5)
3. Which statement about catalysts and equilibrium is correct?
a. A catalyst does not appear in a rate equation; thus it does not affect the equilibrium.
b. A catalyst finds a new mechanistic pathway that affects concentrations differently.
c. A catalyst affects the rates of the forward and reverse reactions equally; thus, there is no net change in concentrations.
d. Solid catalysts, which are common in several industrial applications, would not affect the equilibrium constant since solids do not appear in the equilibrium-constant expression.
e. A different and unique catalyst is needed for every equilibrium at different temperatures.
4. What is the value of Kc for the following reaction if the equilibrium concentrations are [A] = 0.60 M [B] = 0.35 M [C] = 0.55 M?
2 A(aq) + B(aq) ⇌ 2 C (aq)
a. 0.38
b. 0.42
c. 2.40
d. 2.62