Average Take Home Test

Document Sample
Average Take Home Test Powered By Docstoc
					                            “Average Take Home Test”
                                                  Name____________________________________


1. CH4(g) + H2O(g) + heat  CO(g) + 3 H2(g) : Which way will the equilibrium shift if:
  a) water is removed ________________
  b) temperature is increased ______________
  c) CO is removed _____________
  d) volume of the container is tripled _____________

2. At 90oC, the equilibrium constant is 6.8E-2 for the reaction: H2(g) + S(s)  H2S(g); if 0.15 mol
hydrogen and 1.0mol sulfur are heated in a 1.0 liter container, what will be the concentration of
H2S at equilibrium? _________________

3. At a certain temperature, 4.0 mol NH3 is introduced into a 2.0L container and the NH3
partially dissociates by the reaction: 2 NH3(g)  N2(g) + 3 H2(g); at equilibrium, 2.0 mol of
NH3 remains. What is the value of K for this reaction? ________________

4. The following equilibrium pressures were observed for the Haber reaction:
PNH3 = 3.1E-2 atm; PN2 = 8.5E-1; PH2 = 3.1 E –3. Calculate the value for the equilibrium
constant Kp. ____________________

5. What does the Kc equal in problem #4? ____________________

6. For the reaction: H2(g) + Br2(g)  2 HBr(g) , Kp = 3.5E4 at 1495 K. What is the value of Kp
for the following reactions at 1495K?
 a) HBr(g)  ½ H2(g) + ½ Br2(g)        _______________
 b) 2HBr(g)  H2(g) + Br2(g)          _______________
 c) ½ H2(g) + ½ Br2(g)  HBr(g)       _______________________


7. Write the expressions for K for the following reactions:
 a) P4(s) + 5 O2(g)  P4O10(s)                             ______________


 b) C(s) + H2O(g)  CO(g) + H2(g)                           ______________

8. The reaction H2(g) + I2(g)  2 HI(g) has a Kp = 45.9 at 763K. A particular equilibrium
mixture at that temperature contains gaseous HI at a partial pressure of 4.00 atm and the
hydrogen gas at a partial pressure of 0.200 atm. What is the partial pressure of I2? _________

9.At a certain temperature, K = 9.1E-4 mol/L for the reaction: FeSCN2+(aq)  Fe3+(aq) + SCN-(aq)
Calculate the concentrations of all three species in a solution which is initially 2.0M FeSCN2+
[FeSCN2+] =___________ [Fe3+] = __________ [SCN-] = __________

10. At a particular temperature, K = 4.0E-7 mol/L for the reaction: N2O4(g) 2 NO2(g)
In an experiment, 1.0 mol N2O4 is placed in a 10.0L vessel. Calculate the concentrations of
N2O4____________ and NO2_______________ when this reaction reaches equilibrium.

				
DOCUMENT INFO
Shared By:
Categories:
Tags:
Stats:
views:31
posted:8/13/2012
language:Unknown
pages:1