WorksheetsHonors Equilibrium 21-22 (NO ICE TABLES)
Total questions: 56
Worksheet time: 40mins
How does a catalyst affect a reaction at equilibrium?
It makes the reaction shift right
It makes the reaction shift left
It doesn't affect the equilibrium position
SO2 + O2 <=> SO3
If the concentration of SO2 is increased, the equilibrium position of the reaction will shift ___________.
SO2 + O2 <=> SO3
If the equilibrium position shifts to the right, the concentration of O2 will ___________.
N2 + O2 <=> 2NO
If O2 is removed, the concentration of N2 will _______.
For the reaction...
N2 (g) + 3 H2(g) <=> 2 NH3 (g)
If the pressure in the system is increased, which substance(s) will increase in concentration?
N2
H2
N2 and H2
NH3
N2 + O2 <=> 2NO: Δ H = +182 kJ mol-1.
If the temperature is increased the equilibrium position will shift _______.
What is the Keq expression for this reaction?
2 NO(g) + O2(g) ⇌ 2 NO2(g)
Keq = [NO2]2 / [NO]2 [O2]
Keq = [NO]2 [O2] / [NO2]2
Keq = [NO]2 [O2] [NO2]2
Keq = [NO2]2 / [NO]2 + [O2]
2SO2(g) + O2(g) <=> 2SO3(g): ΔΗ = - 197 kJ mol -1
Which of the following will NOT shift the equilibrium position to the right?
An equilibrium constant with a large value, e.g. Keq = 1000, indicates…
A very fast reaction
Products are favored at equilibrium
Reactants are favored at equilibrium
Nothing useful at all
Le Chatelier's Principle states that if a (dynamic) equilibrium is disturbed by changing the conditions, the equilibrium position..
moves to increase the change
moves to counteract the change
does not change
Changes in pressure will only affect substances that are in the __________ state.
gaseous
liquid
solid
aqueous
SO2 (g) + NO2 (g) <=> SO3 (g) + NO (g)
had reached a state of equilibrium, was found to contain
0.40 mol L-1 SO3 , and 0.30 mol L-1 NO,
0.15 mol L-1NO2 , and 0.20 mol L-1 SO2.
Calculate the equilibrium constant for this reaction.
What is the equilibrium expression for:
Fe3O4(s) + 4H2(g) <=> 3Fe(s) + 4H2O(g)
Keq =
[Fe]3 [H2O]4 / [Fe3O4] [H2]4
[Fe3O4] [H2]4 / [Fe]3 [H2O]4
[H2O]4 / [H2]4
[Fe] [H2O] / [Fe3O4] [H2]
For the reaction...
H2 (g) + Cl2 (g) <=> 2HCl (g) + heat
If the pressure in the system is increased, the equilibrium position will _______.
shift to the left
shift to the right
not shift
Removing O2(g) will
H2(g)+Cl2(g)⇌2HCl(g)
The forward reaction is exothermic. What will happen to the equilibrium if the temperature is increased?
equilibrium shifts right
equilibrium shifts left
You cannot predict the effect
no change
heat + N2 + O2 <−> 2NO
If the heat is removed from the chemical system, the concentration of N2 will _______.
For the equilibrium
2SO3(g) ↔ 2SO2(g) + O2(g)
Keq = 4.08x10-3 at 1000K
Comment on the equilibrium position.
Products are favored at equilibrium
Reactants are favored at equilibrium
Equilibrium stays put
An analysis of the concentrations at equilibrium in a 1 L flask yields the following results:
[NOCl] = 0.30, [NO] = 1.2, and [Cl2] = 0.60
Calculate the equilibrium constant for the following reaction: 2 NOCl(g) ↔ 2 NO(g) + Cl2(g)
(a)
N2 + O2 <=> 2NO: Δ H = +182 kJ mol-1.
If the temperature is increased the equilibrium position will shift _______.
2 NO(g) + O2(g) ⇌ 2 NO2(g)
Identify the incorrect statement about achieving equilibrium.
achieved when product and reactant concentrations are equal
achieved when forward and reverse reaction rates are same
achieved when concentration of reactants is stable/constant
achieved when concentration ratio of reactants to products becomes stable, thus fixing the equilibrium constant (equilibrium position)
8 seconds
20 seconds
Around what time does the reaction reach equilibrium?
25 min
70 min
45 min
80 min
Changes in pressure will only affect substances that are in the ______ state.
solid
gas
liquid
When the rate of the forward reaction is equal to the rate of the backward reaction, the system is said to be in _____
Chemical Balance
Chemical Constant
Chemical Reaction
Chemical Equilibrium
For the reaction...
SO2 + O2 <−> SO3
If the equilibrium shifts to the right, the concentration of O2 will ___________.
increase
decrease
double
stay the same
The following factors affect the position of equilibrium EXCEPT
Concentration
State of Matter
Temperature
Pressure
The forward reaction points towards the __________.
The forward reaction forms the substance __________.
The reverse reaction points towards the __________.
The reverse reaction forms the substance __________.
SO2 + O2 <−> SO3
If the equilibrium shifts to the left, the concentration of SO3 will ___________.
SO2 + O2 <−> SO3
If the equilibrium shifts to the left, the concentration of SO2 will ___________.
heat + N2 + O2 <−> 2NO
If O2 is removed, the concentration of N2 will _______.
heat + N2 + O2 <−> 2NO
If NO is removed from the system, the concentration of N2 will _______.
heat + N2 + O2 <−> 2NO
If the heat is removed to the chemical system, the equilibrium will shift _______.
heat + N2 + O2 <−> 2NO
If the heat is removed from the chemical system, the concentration of N2 will _______.
heat + N2 + O2 <−> 2NO
If the heat is added to the chemical system, the concentration of O2 will _______.
H2 (g) + Cl2 (g) <−> 2HCl (g) + heat
If the pressure in the system is increased, the equilibrium will _______.
N2 (g) + 3 H2 (g) <−> 2 NH3 (g)
If the pressure in the system is increased, which substance will increase in concentration?
N2 (g) + 3 H2 (g) <−> 2 NH3 (g)
If the pressure in the system is decreased, which substance will increase in concentration?
How is the reaction quotient used to determine whether a system is at equilibrium?
At equilibrium, the reaction quotient is undefined.
The reaction is at equilibrium when Q < K.
The reaction is at equilibrium when Q > K.
The reaction is at equilibrium when Q = K.
If the reaction quotient Q has a smaller value than the related equilibrium constant, K, _________
the reaction is at equilibrium
the reaction is not at equilibrium, and will make more products at the expense of the reactants
the reaction is not at equilibrium, and will make more reactants at the expense of the products
the value of K will not increase until it is equal to Q
If the reaction quotient Q has a value larger than the related equilibrium constant, K _________
the reaction is at equilibrium
the reaction is not at equilibrium, and will make more products at the expense of reactants
the reaction is not at equilibrium, and will make more reactants at the expense of products
the value of K will increase until it is equal to Q
The value of the equilibrium constant, Kp for the reaction below is 3.1 × 10-4 at 700K.
N2 (g) + 3H2 (g) ↔ 2NH3 (g)
Given the initial partial pressure of the gases, PN2 = 0.411 atm; PH2 = 0.903 atm; PNH3 = 0.224 atm, calculate the value of the reaction quotient, Q.
Q = 0.0437
Q = 0.1658
Q = 0.6036
Q = 0.1352
The value of the equilibrium constant, Kp for the reaction below is 3.1 × 10-4 at 700K.
N2 (g) + 3H2 (g) ↔ 2NH3 (g)
Given the initial partial pressure of the gases, PN2 = 0.411 atm; PH2 = 0.903 atm; PNH3 = 0.224 atm. Predict the direction in which the reaction will proceed at 700 K.
Since Q > Kp, the equilibrium will proceed to the left to bring the value Q down to 3.1 × 10-4.
Since Q > Kp, the equilibrium will proceed to the right to bring the value Q down to 3.1 × 10-4.
Since Q > Kp, the equilibrium will proceed to the left to bring the value Q up to 3.1 × 10-4.
Since Q > Kp, the equilibrium will proceed to the right to bring the value Q up to 3.1 × 10-4.
For the reaction system:
2HI (g) ↔ H2 (g) + I2 (g)
Kc = 0.020 at 720 K
If the initial concentrations of HI, H2 and I2 are all 1.50 × 10-3 M at 720 K, which one of the following statements is correct?
The system is at equilibrium.
The concentrations of HI and I2 will increase as the system is approaching equilibrium.
The concentration of HI will increase as the system is approaching equilibrium.
The concentration of H2 and I2 will increase as the system is approaching equilibrium.
For the reaction, N2O4 (g) ↔ 2NO2 (g), Kc = 0.21 at 100oC. At initial, the [N2O4] = 0.12 M and [NO2] = 0.55 M. Is the reaction at equilibrium? If not, in which direction it is progressing?
Yes, the reaction is at equilibrium.
No, the reaction is not at equilibrium. Qc < Kc, therefore the reaction will proceed from left to right until Qc = Kc.
No, the reaction is not at equilibrium. Qc > Kc, therefore the reaction will proceed from right to left until Qc = Kc.
No, the reaction is not at equilibrium. Qc < Kc, therefore the reaction will proceed from right to left until Qc = Kc.
