The product concentrations increase slightly with time

we can conclude that
a. ∆Ηο > 0 and ∆So < 0
b. ∆Ho < 0 and ∆So < 0
c. ∆Ho > 0 and ∆So > 0
d. ∆Ho < 0 and ∆So > 0
e. ∆Go < 0 at all temperatures

2. Calculate ∆Go of formation, in kJ/mol, for H3PO4.

CHM-115-A	Sample Exam 1
c. It increases the rate of the reaction. d. It decreases the rate of the reaction.
a. O(g)	O3(g) = O2(g) + O(g) O(g) + O3(g) → 2O2(g)	(fast)
a. O(g)	O3(g) = O2(g) + O(g) O(g) + O3(g) → 2O2(g)	(slow)
b. O3(g) c. O2(g) d. O2(g) and O(g) e. O3(g) and O2(g)
Copyright by James P. Birk

CHM-115-A Sample Exam 1

14. Consider the following energy diagram for a chemical reaction. The lower 14. b

d. the same reaction at higher temperature.

e. an intermediate in the reaction.

23. Consider the following reaction
CaO(s) + CO2(g) = CaCO3(s) The equilibrium constant expression is
a. K = [CaCO3]/[CaO]
b. K = [CaO][CO2]/[CaCO3]
c. K = 1/[CO2]
d. K = [CO2]
e. K = [CaCO3]/[CaO][CO2]

24. For the reaction, MgCl2(s) + ½O2(g) = MgO(s) + Cl2(g), K = 2.98. For the reaction, 2Cl2(g) + 2MgO(s) = 2MgCl2(s) + O2(g), K is a. 1.73
b. 0.113
c. -8.88
d. 0.579
e. 0.336

a. b.

c. d.