Equilibrium Module 1

Course Name:  Chemistry
Course No.132 NT
Teacher:  Bill Cook
Teacher's Email:  bcook@icc.edu

No. of Questions= 5


1.  Which expression correctly describes the equilibrium constant for the following reaction?

4 NH3(g)  +  5 O2(g) dblaro.jpg (896 bytes)  4 NO(g)  +  6 H2O(g)

a) wpe7.jpg (2330 bytes)
b) wpe8.jpg (2333 bytes)
c) wpe9.jpg (1997 bytes)
d) wpeB.jpg (2303 bytes)
e) wpeA.jpg (2246 bytes)
2.  The equilibrium constant at 1300 K for the reaction

H2(g)  +  Br2(g) dblaro.jpg (896 bytes)   2 HBr(g) 

is 1.6 x 105. The value of K for the reverse reaction is:

a) 6.3 x 10-6
b) -1.6 x 105
c) 1.6 x 10-5
d) 1.6 x 105
e) 6.3 x 10-5
3.  The equilibrium constant for the reaction

H2(g)  +  I2(g) dblaro.jpg (896 bytes) 2 HI(g)

is 62.5 at 800 K. What is the equilibrium concentration of I2 if [HI] = 0.20 M and [H2] = 0.10 M?

a) 3.2 x 10-2 M
b) 8.0 x 10-4 M
c) 6.4 x 10-3 M
d) 0.20 M
e) 0.10 M
4.  Calculate Kc for the reaction: Fe(s) + H2O(g) dblaro.jpg (896 bytes) FeO(s) + H2(s)   given the following information.

H2O(g) + CO(g) dblaro.jpg (896 bytes) H2(g) + CO2(g)     Kc = 1.65

Fe(s) + CO2(g) dblaro.jpg (896 bytes) FeO(s)(s) + CO(g)     Kc = 1.35

a) 3.00
b) 1.22
c) 0.818
d) 2.23
e) 0.300
5.  For which of the following equilibria would Kc = Kp?
a)
b)
c)
d)
e)



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