Equilibrium Constant
What is ̇n for the following equation in relating Kc to Kp? N2(g) + 3 H2(g) ? 2 NH3(g)
-2
Consider the following reaction at equilibrium. What effect will reducing the volume of the reaction
mixture have on the system?
Cu (s) + O2 (g) <-> Cu (s) + SO2 (g)
No effect will be observed
The stronger the acid, then which of the following is TRUE?
The Weaker the conjugate base
Calculate the hydroxide ion concentration in an aqueous solution with a pH of 9.85 at 25°C
7.1 × 10-5 M
Determine the pH of a .461M C6H5CO2H solution if the Ka of C6H5CO2H is 6.5x10^-5
PH = 2.26
Express the equilibrium constant for the following reaction.
2NH3 (g) <-> N2 (g) + 3H2 (g)
Kc = [H2]^3 x [N2] / [Nh3]^2
Consider the following reaction at equilibrium. What effect will increasing the temperature have on the system?
Fe3O4 (s) + CO (g) <--> 3FeO (s) + CO2 (g)
deltaH = +35.9kJ
Reaction will shift to the right
What is the conjugate base for H2PO4?
HPO4 ^2-
Determine the [OH-] concentration of a .116M Ba(OH)2 solution at 25C
.232M
Find the percent ionization of a .337M HF solution. The Ka for HF is 3.5x10^-4
3.2%
The reaction below has a Kc value of 61. What is the value of Kp for this reaction at 500 K?
N2 (g) + 3H2 (g) <--> 2Nh3 (g)
3.6x10^-2
What effect will removing NO2 from the system?
S02 (g) + NO2 (g) <--> SO3 (g) + NO (g)
reaction will shift to the left
Which of the following acids will have the strongest conjugate base?
A. HI
B. HCLO4
C. HCL
D. HCN
D
Determine the Ka of an acid whose 0.294 M solution has a pH of 2.80
Ka = 8.5 × 10-6
Which one of the following will form an acidic solution in water?
A) NH4Cl
B) KNO3
C) NaF
D) LiI
E) None of the above solutions will be acidic
A) NH4Cl
Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows:
[N2]eq = 3.6 M, [O2]eq = 4.1 M, [N2O]eq = 3.3 × 10-18 M.
2.0x10^-37
What effect will decreasing the temperature have on the system
CO2 (g) + 2H20 (l) <--> CH4 (g) + 2O2 (g)
deltaH = +890kj
reaction will shift to the left
Which of the following acids is the WEAKEST? The acid is followed by its Ka value.
A) C6H5CO2H, 6.3 × 10-5
B) HBrO, 2.3 × 10-9
C) HClO, 2.9 × 10-8
D) HC2H3O2, 1.8 × 10-5
E) HIO, 2.3 × 10-11
E) HIO, 2.3 × 10-11
Determine Kb for CN- at 25C. The Ka for HCN is 4.9x10^-10
Determine pH of a .227M C5H5N solution at 25C. The Kb of C5H5N is 1.7x10^-9
PH= 9.29
Determine the value of Kp for the following reaction if the equilibrium concentrations are as follows:
P(NOCl)eq = 0.22 atm, P(NO)eq = 0.10 atm, P(Cl2)eq = 0.081 atm.
1.7x10^-2
Consider the following reaction at equilibrium. What effect will increasing the volume have on the system?
2H2S (g) + 3O2 (g) <--> H2O (g) + 2SO2 (g)
reaction will shift to the left
Which of the following is NOT a conjugate acid-base pair?
A) C2H3O2?/HC2H3O2
B) H3O?/OH?
C) H2SO3/HSO3?
D) NH4 +/NH3
E) All of the above are conjugate acid-base pairs
B. H3O/OH
Calculate POH of a solution that contains 3.9x10^-4 M H3O+
POH = 10.59
Determine the pH of a solution that is 0.15 M HClO2 (Ka = 1.1 x 10-2) and 0.15 M HClO (Ka = 2.9 × 10-8).
pH = 1.39