142 worked out problems
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Chapter 15
a.
The decomposition of PCl5 occurs via the reaction
PCl5(g)
<--> PCl3(g) +
Cl2(g)
A sample of PCl5 is
placed in a reaction vessel held at 250 °C at an initial
pressure of 1.10 atm. When equilibrium is attained, the pressure of PCl5 is
0.33 atm. Calculate Kp for this reaction. [1.77] solution
b.
Suppose
that H2(g) and CH4(g) are brought into contact
with C(s) at 500 °C
with PH2=
0.20 atm and PCH4 = 3.0 atm. Is the reaction
C(s) + 2H2(g)<--> CH4(g) Kp 2.69 x 103
at equilibrium? If not, which direction will the reaction proceed
towards equilibrium? What is the equilibrium pressures of each? [H2
= 0.036 atm, CH4 = 3.082 atm] solution
c. An unknown mass of NH4Cl(s) is placed in an evacuated container and allowed to come to equilibrium at 500K:
1 NH4Cl(s)
<-->1 NH3(g)
+ 1 HCl(g)
At equilibrium, the total pressure is 6.2 atm. What is the value of Kp
for this equilibrium? [9.61] solution
d. NH4Cl(s)
<-->1 NH3(g)
+ 1 HCl(g)
A
flask is filled with 3.2 atm of NH3(g)
and 1.5 atm of HCl(g) at 300 K. Once equilbrium is achieved, Ptotal = 2.50 atm. Calculate Kp for this reaction. [0.84] solution
e. At
500 K, the following equilibrium exists, with a Kc = 1.0 x 102
1 H2(g)
+ 1 F2(g)
<--> 2
HF (g)
In
a particular experiment, 3.0 mol of F2(g)
and 3.0 mol of H2(g)
are added to a 2.0 L flask. Calculate the equilibrium concentration of
each species.[HF = 2.50 M, F2 = 0.25 M, H2
= 0.25 M] solution
~MEO 23 Feb 06