ICE Table
Equilibrium
Le Châtelier’s Prinicple
Acid and base
pH scales
100
Write an ICE table (but don’t solve it) for 1.0 M SO3 reacting with 2.0 M H2O according to the equation SO3(g) + H2O(g) D H2SO4(g)
YES!
100
What is the mass action equation of:
NH4CO2NH2(s)⇌2NH3(g)+CO2(g)
2NH3(g)+CO2(g)
100
Predict the effect of increasing the volume of the container
CO(g) + H2 <--> C(s) + H2O(g)
Shift to the left
100
Which is a weaker acid
hydrocyanic acid vs. nitric acid
hydrocyanic acid
100
A solution at pH 11.5 is
basic
200
In the reaction 2 NO2(g) <--> N2O4(g) the initial concentration of N2O4 was 0.100 M and NO2 was 0.000 M. At equilibrium, the concentration of N2O4 was measured as 0.009 M. Calculate Kc.
Kc= 0.27
200
Initial concentrations at 800 K are set to [H2O]0 = 0.500 M; [CO]0 = 0.200 M; [H2]0 = 0.300 M with solid carbon present.
𝐂𝐎(𝒈) + 𝐇𝟐(𝒈) ⟶ 𝐂(𝒔) + 𝐇𝟐𝐎(𝒈)
200
What would happen to the position of the equilibrium when more Hg is added to the system.
2HgO(s) <--> Hg(l) + O2
No shift
200
Which is the strongest base:
Ammonia with Kb of 1.8 x 10-5 or Aniline with Kb 7.4 x 10-10
Ammonia
200
What is the pH of a 0.0235 M HCl solution?
1.629
300
If a solution with the concentrations of I2 and I- both equal to 1.00 x 10-3M before reaction gives an equilibrium concentrations of I2 of 6.61 x 10-4M, what is the equilibrium constant for the reation?
Kc= 776
300
A mixture of SO2 and O2 was maintained at 800K until the system reached equilibrium mixture contained 5.0 x 10-2 M SO3, 3.5 x 10-3 M O2, and 3.0 x 10-3 M SO2, calcuate Kp.
7.9 x 104
300
What will happen if the temperature is increased
2NO(g) + H2(g) <--> N2O(g) + H2O(g) + heat
Shift from right to left
300
True or False: A week base has a weak conjugated acid.
False
300
What is the pH of a 6.50 x 10-3 M KOH solution?
11.8
400
The equilibrium constant Kc for the decomposition of PCl5 (g) into PCl3(g) and Cl2 is 0.0211. What are the equilibrium concentrations of PCl5, PCl3, and Cl2 in a mixture that initially contained only PCl5 at a concentration of 1.0M
PCl5 <--> PCl3 + Cl2
PCl5= 0.87M
PCl3= 0.135M
Cl2= 0.135M
400
Free bee for being brave-ish!
what is the mass action of H2(g) + CO2(g) ⇌ H2O(g) + CO(g)
H2O(g) + CO(g)/H2(g) + CO2(g)
400
If heat is added to an endothermic reaction, in which direction will the equilibrium shift according to Le Chatelier's principle?
To the right
400
CN−(aq)+H2O(l)⇌OH−(aq)+HCN(aq), the stronger acid is HCN, therefor there are more products than reactants.
False
400
A solution has a [H+] concentration of 5.3 x 10-6 M. Is this an acidic or basic solution? Why
?
Acidic
pH= 5.28
500
A mixture consisting initially of 3.00 moles NH3, 2.00 moles of N2, and 5.00 moles of H2, in a 5.00 L container was heated to 900K, and allowed to reach equilibrium. Determine the equilibrium concentration for each species present in the equilibrium mixture. Kc = 0.0076 @ 900 K
2 NH3(g) 
N2(g) + 3H2(g)
N2= 0.184M
H2= 0.352M
NH3= 1.032M
500
A 1.00 mol sample of NOCl was placed in a 2.00 L reactor and heated to 227°C until the system reached equilibrium. The contents of the reactor were then analyzed and found to contain 0.056 mol of Cl2. Calculate K at this temperature. The equation for the decomposition of NOCl to NO and Cl2 is as follows:
2NOCl(g) <--> 2NO(g) + Cl2 (g)
4.5 x 10-4
500
For the reaction below, what change could cause the equilibrium to shift to the right?
CH4 (g) + 2 H2S(g) <---> CS2(g) + 4H2(g)
Increase the concentration any of the reactants, decrease the pressure on the system, decrease the concentration of any of the product
500
HF(aq) + CN–(aq) HCN(aq) + F–(aq), Which species is the Stonger Brønsted acid in this equilibrium?
HF
500
What is the pH of a 6.2 x 10-5 M NaOH solution?
9.79