Font size
WorksheetsChemical Equilibrium ICE Charts
Total questions: 14
Worksheet time: 44mins
Calculate the equilibrium constant (Kc) for the given reaction
N2 (g) + 3H2 (g) ↔ 2NH3 (g)
At equilibrium [N2] = 0.34 M, [H2] = 0.13 M, and [NH3] = 0.19 M.
48
33
48.0
33.07
Calculate the equilibrium constant (Kc) for the given reaction and tell whether equilibrium lies to the left or the right.
2NO (g) + Br2 (g) ↔ 2NOBr (g)
At equilibrium [NO] = 0.5 M, [Br2] = 0.25 M, and [NOBr] = 3.5 M.
56 lies to the right
200 lies to the right
196 lies to the left
56 lies to the left
Calculate the equilibrium constant (Kc) for the given reaction and tell whether equilibrium lies to the left or the right.
PCl5 (g) ↔ PCl3 (g) + Cl2 (g)
Equilibrium concentrations are: [PCl5] = 0.25 M, [PCl3] = 9.7 × 10-4 M, and [Cl2] = 3.2 × 10-3 M.
1.02 lies to the left
0.000012 lies to the left
1.02 lies to the right
0.000012416 lies to the left
A mixture of 0.500 mol H2 and 0.500 mol I2 was placed in a 1.00L stainless-steel flask at 430⁰C. The equilibrium constant Kc for the reaction H2 (g) + I2 ↔ 2HI (g) is 54.3 at this temperature. Calculate the concentrations of H2, I2 , and HI at equilibrium.
Use ICE Table
[H2] = 0.107 M
[I2] = 0.107 M
[HI] = 0.768 M
[H2] = 0.768 M
[I2] = 0.107 M
[HI] = 0.107 M
[H2] = 0.107 M
[I2] = 0.768 M
[HI] = 0.107 M
[H2] = 0.107 M
[I2] = 0.107 M
[HI] = 0.0768 M
The equilibrium constant (Kc) for the formation of nitrosyl chloride, an orange-yellow compound, from nitric oxide and molecular chlorine is 6.5 x 10 4 at 35 ⁰ C. In a certain experiment, 2.0 x 10 -2 mole of NO, 8.3 x10 -3 mole of Cl2, and 6.8 moles of NOCL are mixed in a 2.0-L flask.
2NO(g) + Cl2 ↔ 2NOCl (g)
Find Q and predict how the reaction will proceed.
2.9 x 10 7 to the left
3.0 x 10 7 to the left
2.89 x 10 7 to the right
2.89 x 10 5 to the left
Consider the following system at equilibrium:
CH4(g) + 2H2O (g) ↔ CO2 (g) + 4H2O (g)
Suppose the concentration of CH4 decreased, in which direction does the reaction shift to reestablish equilibrium?
The reaction shifts to the left
The reaction shifts to the right
Consider the following system at equilibrium:
CH4(g) + 2H2O (g) ↔ CO2 (g) + 4H2 (g)
Suppose the concentration of CH4 decreased, what happens to the concentrations of H2O, CO2, and H2 as the reaction shifts to reestablish equilibrium?
The concentrations of the products, CO2, and H2 will decrease and the reactant H2O, will increase in concentration.
The concentrations of the products, CO2, and H2 will increase and the reactant H2O, will decrease in concentration.
Predict whether the reaction will shift to the right, left or not be affected by an INCREASE in temperature
2H2O2 (g) ↔ 2H2O (g) + O2 (g) exothermic
left
right
no effect
Predict whether the reaction will shift to the right, left or not be affected by an INCREASE in temperature
2H2O2 (g) ↔ 2H2O (g) + O2 (g) endothermic
left
right
no effect
What is the Kc expression for this reaction? 2 NO(g) + O2(g) ⇌ 2 NO2(g)
Kc = [NO2]2 / [NO]2 [O2]
Kc = [NO]2 [O2] / [NO2]2
Kc = [NO]2 [O2] [NO2]2
Kc = [NO2]2 / [NO]2 + [O2]
Consider the following reaction: 2SO2(g) + O2(g) <=> 2SO3(g): ΔΗ = - 197 kJ mol -1 Which of the following will NOT shift the equilibrium position to the right?
Adding more O2
Adding a catalyst
increasing the pressure
Lowering the temperature
What is the equilibrium expression for: Fe3O4(s) + 4H2(g) <=> 3Fe(s) + 4H2O(g) Kc =
[Fe]3 [H2O]4 / [Fe3O4] [H2]4
[Fe3O4] [H2]4 / [Fe]3 [H2O]4
[H2O]4 / [H2]4
[Fe] [H2O] / [Fe3O4] [H2]
If the equilibrium constant is much less than one (K << 1) then
Equilibrium is not established.
Equilibrium lies to the right (products are favored)
Equilibrium lies to the left (reactants are favored)
Neither products or reactants are favored.
Calculate the equilibrium constant (Kc) for the given reaction
H2 (g) + Cl2 (g) ↔ 2HCl (g)
At equilibrium [H2] = 0.42 M, [Cl2] = 0.075 M, and [HCl] = 0.95 M
30.16
29
28.65
31
