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WorksheetsEquilibrium
Total questions: 25
Worksheet time: 23mins
For the reaction 2H2S(g)<---> 2H2(g) + S2(g), kp= 2.4 x10-4 at 1073 K. A reaction mixture contains 0.112 atm H2, 0.055 atm of S2 and 0.445 atm of H2S. Is the reaction at equilibrium? if not, which way will it proceed
Yes it is at equilibrium
No, to the right
No, to the left.
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 _______.
N2 (g) + 3 H2 (g) <=> 2 NH3 (g)
If the pressure in the system is increased, which substance(s) will increase in concentration?
2 NO(g) + O2(g) ⇌ 2 NO2(g)
2SO2(g) + O2(g) <=> 2SO3(g): ΔΗ = - 197 kJ mol -1
Which of the following will NOT shift the equilibrium position to the right?
If a (dynamic) equilibrium is disturbed by changing the conditions, the position of equilibrium................
Hydrogen can be produced by this reaction.
CO(g) + H2O(g) ⇌ CO2(g) + H2(g)
In an experiment 4.20 mol of carbon monoxide were mixed with 2.00 mol of steam. When the reaction reached equilibrium, 1.60 mol of hydrogen had been formed.
What is the value of the equilibrium constant, Kc, for this reaction?
0.30
0.41
1.54
2.46
When one mole of ammonia is heated to a given temperature, 50% of the compound dissociates and the following equilibrium is established.
NH3(g) ⇌ 0.5N2(g) + 1.5H2(g)
What is the total number of moles of gas present in this equilibrium mixture?
1.5
2.0
2.5
3.0
A and B react together in this reversible reaction.
A + 3B ⇌ C + 2D
A mixture of 10 mol of A and 10 mol of B were left to reach equilibrium. The equilibrium mixture contained 4 mol of B.
What is the total amount, in moles, of substances in the equilibrium mixture?
14
16
18
20
Hydrogen is produced by the reaction of methane with steam. The reaction mixture reaches a state of dynamic equilibrium.
CH4(g) + H2O(g) ⇌ CO(g) + 3H2(g) ∆H = +206 kJ mol−1
Which of the following shows how the equilibrium yield of hydrogen and the value of the equilibrium constant are affected by the changes shown?
Change: Increase pressure
Effect on equilibrium yield of H2(g): decrease
Effect on value of Kc: decrease
Change: Add a catalyst
Effect on equilibrium yield of H2(g): increase
Effect on value of Kc: no effect
Change: Increase temperature
Effect on equilibrium yield of H2(g): increase
Effect on value of Kc: increase
Change: Remove CO(g) as formed
Effect on equilibrium yield of H2(g): increase
Effect on value of Kc: increase
Methanol is synthesised from carbon monoxide and hydrogen according to the equation below.
CO(g) + 2H2(g)⇌ CH3OH(g) ∆H = −91 kJ mol−1
Which one of the following changes would not affect the value of the equilibrium constant and would not increase the yield of methanol?
increase in temperature
decrease in temperature
increase in pressure
decrease in pressure
At elevated temperatures ammonium carbonate, NH2COONH4, is in equilibrium with NH3 and CO2 according to the equation;
NH2COONH4(s) ↔ 2 NH3(g) + CO2(g)
What is the equilibrium expression for this reaction?
K = 2 [NH3][CO2]
[NH2COONH4]
K = [NH3]2[CO2]
[NH2COONH4]
K = 2 [NH3][CO2]
K = [NH3]2[CO2]
CO2(g) + H2(g) ↔ CO(g) + H2O(l)
heat + N2 + O2 ↔ 2NO
If the heat is added to the chemical system, the equilibrium will shift _______.
For the following reaction: H2(g) + Cl2 (g) ↔ 2HCl(g), calculate the concentration of HCl when Keq= 2.3x10-5, [H2]= 0.0056mol, [Cl2]= 0.0048mol.
6.2 x 10-10 M
2.5 x 10-5 M
1.1 M
1.2 M
Fe3O4(s) + 4H2(g) <=> 3Fe(s) + 4H2O(g)
Kc =
Methanol can be produced from hydrogen and carbon monoxide.
