Chapter 15 Worksheet 8
Supplemental Instruction
Iowa State University
Leader:
Course:
Instructor:
Date:
Prina
Chem 178
Dr. Meyer
02/04/2015
1) Methanol, CH3OH, is produced commercially by the catalyzed reaction of carbon monoxide and hydrogen.
CO(g) + 2 H2(g)<-> CH3OH(g)
An equilibrium mixture in a 2.00 L vessel is found to contain 0.0406 mol CH3OH, 0.170 mol CO and 0.302 mol H2
at 500. K. Calculate Kp at this temperature.
0.0062
Q<K
Q=Kc
Q>Kc
2) At 100 C the equilibrium constant for the reaction COCl2(g) ?? CO(g) + Cl2(g) has a value of Kc = 2.19 X 10 ^10. Are the following mixtures of COCl2, CO, and Cl2 at 100 C at equilibrium? If not, indicate the direction that the
reaction must proceed in order to reach equilibrium.
a) [COCl2] = 2.00 x 10 ^-3 M, [CO] = 3.3 X 10 ^-6 M, [Cl2] = 6.62 X 10^-6 M left
b) [COCl2] = 4.50 x 10 ^-2 M, [CO] = 1.1 X 10 ^-7 M, [Cl2] = 2.25 X 10^-6 M right
c) [COCl2] = 0.010 M, [CO] = [Cl2] = 1.48 X 10^-6 M equilibrium
3) Initially, 1.0 mol of NO(g) and 1 mol of Cl2(g) were added to a 1 L container. As a result of the reaction the
equilibrium concentration of NOCl(g) became 0.96 M. Using the ICE table methodology determine the value of the
equilibrium constant KC for this reaction.
2NO(g) +Cl2(g) <-> 2NOCl (g)
1107.6
1060 Hixson-Lied Student Success Center  515-294-6624  sistaff@iastate.edu  http://www.si.iastate.edu
4) For the reaction: H2(g) + I2(g)<------> 2HI(g) Kc=55.3 at 700K. In a 2.00 L flask containing an equilibrium
mixture of the three gases,there are 5.5x10^-2 g H2(g) and 4.33g I2(g). What is the mass of the HI(g) in the flask?
Mass=20.6g
5) Hydrogen and Iodine gas react together to form hydrogen iodide gas . The equation for this reaction is
H 2 (g) + I 2 (g) ↔ 2HI(g)
The equilibrium constant for this reaction is 7.1 x 10 2 at 25 °C. If the current concentration of gases are
[H ] 0 = 0.81 M
[I ] 0 = 0.44 M
[HI] 0 = 0.58 M
what direction will the reaction shift to reach equilibrium?