Week 1 IBDP2 HL - Equilibria Kc calculations

Posljednje ažuriranje almost 2 years ago

Instrukcije

Week 1 IBDP2 HL - Equilibria Kc calculations

Posljednje ažuriranje almost 2 years ago

Instrukcije

These questions are graded mild (easiest) to very hot (challenging).

Please progress through them and jump up a level if you need more challenge

Mild - Calculate the value for Kc

Warm- Determine the equilibrium constant

Hot - Apply knowledge of Kc and calculate Kc using concentration changes

Very Hot - some extra thought needed for these

(Don't forget that if the number of moles/molecules on both sides of the equation are equal, you do not need to determine concentrations.

Mild: Calculate the value for Kc.
2 NO₂(g) ⇄ N₂O4(g)
2.00 moles of NO₂ and 1.60 moles of N₂O₄ are present in a 4.00 dm³ flask at equilibrium.

Mild
1. CO (g) + H₂O (g) ⇄ CO₂ (g) + H₂ (g)
1.60 moles CO, 1.60 moles H₂O, 4.00 moles CO₂ and 4.00 moles H₂ are in an 8.00 dm³flask at equilibrium.

Warm
Determine equilibrium concentrations
1. 2 SO₂ (g) + O₂ (g) ⇄ 2 SO₃ (g) Kc = 798
At equilibrium, [SO₂] = 4.20 and [SO₃] = 11.0M. Calculate the equilibrium [O₂] in this mixture.

Warm
2 SO₂ (g) + O₂ (g) ⇄ 2 SO₃ (g) Kc = 680
0.600 moles of SO₂ and 0.600 moles of O₂ are present in a 4.00 dm³ flask at equilibrium. Calculate the SO₃ equilibrium concentration.

Warm
1. 2 SO₃(g) ⇄ 2 SO₂(g) + O₂(g) Kc = 1.47x10^-3
4.00 moles of SO₂ and 5.00 moles O₂ are present in a 2.00 dm³ container once at equilibrium. Calculate the equilibrium concentration of SO₃ and the number of moles SO₃ present

Hot
2NO₂(g) ⇌ N₂O₄(g) Two sets of equilibrium data are listed for the same temperature.
Container 1 2.00 dm³ 0.12 moles NO₂ 0.16 moles N₂O₄
Container 2 5.00 dm³ 0.26 moles NO₂ ? moles N₂O₄
Determine the number of moles N₂O₄ in the second container.

Hot
Calculate the value for Kc
a. 2 SO₂ (g) + O₂ (g) ⇄ 2 SO₃ (g)
When a 0.600 moles of SO₂and 0.600 moles of O₂ are placed into a 2.00 dm³container and allowed to reach equilibrium, the equilibrium [SO₃] is to be 0.250.
b. When 4.0 moles H₂ and 2.0 moles Br₂ are placed in a 1.0 dm³container the equilibrium [HBr] = 3.0.
c. H₂ (g) + S (s) ⇄ H₂S (g)
6.0 moles H₂S are placed in a 2.0 dm³ container. At equilibrium 5.0 moles H₂are present.

Challenge
The following equilibrium is established at temperature T when 1.00 mol of HI is contained. It is found that 22% of the HI has broken down. Calculate Kc.
2 HI(g) ⇌ H₂(g) + I₂(g)

Week 1 IBDP2 HL - Equilibria Kc calculations

Week 1 IBDP2 HL - Equilibria Kc calculations

Mild: Calculate the value for Kc.2 NO2(g) ⇄ N2O4(g)2.00 moles of NO2 and 1.60 moles of N2O4 are present in a 4.00 dm3 flask at equilibrium.

Mild1. CO (g) + H2O (g) ⇄ CO2 (g) + H2 (g)1.60 moles CO, 1.60 moles H2O, 4.00 moles CO2 and 4.00 moles H2 are in an 8.00 dm3flask at equilibrium.

Warm Determine equilibrium concentrations1. 2 SO2 (g) + O2 (g) ⇄ 2 SO3 (g) Kc = 798 At equilibrium, [SO2] = 4.20 and [SO3] = 11.0M. Calculate the equilibrium [O2] in this mixture.

Warm 2 SO2 (g) + O2 (g) ⇄ 2 SO3 (g) Kc = 680 0.600 moles of SO2 and 0.600 moles of O2 are present in a 4.00 dm3 flask at equilibrium. Calculate the SO3 equilibrium concentration.

Warm1. 2 SO3(g) ⇄ 2 SO2(g) + O2(g) Kc = 1.47x10-3 4.00 moles of SO2 and 5.00 moles O2 are present in a 2.00 dm3 container once at equilibrium. Calculate the equilibrium concentration of SO3 and the number of moles SO3 present

Hot 2NO2(g) ⇌ N2O4(g) Two sets of equilibrium data are listed for the same temperature.Container 1 2.00 dm3 0.12 moles NO2 0.16 moles N2O4Container 2 5.00 dm3 0.26 moles NO2 ? moles N2O4Determine the number of moles N2O4 in the second container.

ChallengeThe following equilibrium is established at temperature T when 1.00 mol of HI is contained. It is found that 22% of the HI has broken down. Calculate Kc. 2 HI(g) ⇌ H2(g) + I2(g)

Mild: Calculate the value for Kc.2 NO2(g) ⇄ N2O4(g)2.00 moles of NO2 and 1.60 moles of N2O4 are present in a 4.00 dm3 flask at equilibrium.

Mild1. CO (g) + H2O (g) ⇄ CO2 (g) + H2 (g)1.60 moles CO, 1.60 moles H2O, 4.00 moles CO2 and 4.00 moles H2 are in an 8.00 dm3flask at equilibrium.

Warm Determine equilibrium concentrations1. 2 SO2 (g) + O2 (g) ⇄ 2 SO3 (g) Kc = 798 At equilibrium, [SO2] = 4.20 and [SO3] = 11.0M. Calculate the equilibrium [O2] in this mixture.

Warm 2 SO2 (g) + O2 (g) ⇄ 2 SO3 (g) Kc = 680 0.600 moles of SO2 and 0.600 moles of O2 are present in a 4.00 dm3 flask at equilibrium. Calculate the SO3 equilibrium concentration.

Warm1. 2 SO3(g) ⇄ 2 SO2(g) + O2(g) Kc = 1.47x10-3 4.00 moles of SO2 and 5.00 moles O2 are present in a 2.00 dm3 container once at equilibrium. Calculate the equilibrium concentration of SO3 and the number of moles SO3 present

Hot 2NO2(g) ⇌ N2O4(g) Two sets of equilibrium data are listed for the same temperature.Container 1 2.00 dm3 0.12 moles NO2 0.16 moles N2O4Container 2 5.00 dm3 0.26 moles NO2 ? moles N2O4Determine the number of moles N2O4 in the second container.

ChallengeThe following equilibrium is established at temperature T when 1.00 mol of HI is contained. It is found that 22% of the HI has broken down. Calculate Kc. 2 HI(g) ⇌ H2(g) + I2(g)

Mild: Calculate the value for Kc.
2 NO₂(g) ⇄ N₂O4(g)
2.00 moles of NO₂ and 1.60 moles of N₂O₄ are present in a 4.00 dm³ flask at equilibrium.

Mild
1. CO (g) + H₂O (g) ⇄ CO₂ (g) + H₂ (g)
1.60 moles CO, 1.60 moles H₂O, 4.00 moles CO₂ and 4.00 moles H₂ are in an 8.00 dm³flask at equilibrium.

Warm
Determine equilibrium concentrations
1. 2 SO₂ (g) + O₂ (g) ⇄ 2 SO₃ (g) Kc = 798
At equilibrium, [SO₂] = 4.20 and [SO₃] = 11.0M. Calculate the equilibrium [O₂] in this mixture.

Warm
2 SO₂ (g) + O₂ (g) ⇄ 2 SO₃ (g) Kc = 680
0.600 moles of SO₂ and 0.600 moles of O₂ are present in a 4.00 dm³ flask at equilibrium. Calculate the SO₃ equilibrium concentration.

Warm
1. 2 SO₃(g) ⇄ 2 SO₂(g) + O₂(g) Kc = 1.47x10^-3
4.00 moles of SO₂ and 5.00 moles O₂ are present in a 2.00 dm³ container once at equilibrium. Calculate the equilibrium concentration of SO₃ and the number of moles SO₃ present

Hot
2NO₂(g) ⇌ N₂O₄(g) Two sets of equilibrium data are listed for the same temperature.
Container 1 2.00 dm³ 0.12 moles NO₂ 0.16 moles N₂O₄
Container 2 5.00 dm³ 0.26 moles NO₂ ? moles N₂O₄
Determine the number of moles N₂O₄ in the second container.

Challenge
The following equilibrium is established at temperature T when 1.00 mol of HI is contained. It is found that 22% of the HI has broken down. Calculate Kc.
2 HI(g) ⇌ H₂(g) + I₂(g)

Mild: Calculate the value for Kc.
2 NO₂(g) ⇄ N₂O4(g)
2.00 moles of NO₂ and 1.60 moles of N₂O₄ are present in a 4.00 dm³ flask at equilibrium.

Mild
1. CO (g) + H₂O (g) ⇄ CO₂ (g) + H₂ (g)
1.60 moles CO, 1.60 moles H₂O, 4.00 moles CO₂ and 4.00 moles H₂ are in an 8.00 dm³flask at equilibrium.

Warm
Determine equilibrium concentrations
1. 2 SO₂ (g) + O₂ (g) ⇄ 2 SO₃ (g) Kc = 798
At equilibrium, [SO₂] = 4.20 and [SO₃] = 11.0M. Calculate the equilibrium [O₂] in this mixture.

Warm
2 SO₂ (g) + O₂ (g) ⇄ 2 SO₃ (g) Kc = 680
0.600 moles of SO₂ and 0.600 moles of O₂ are present in a 4.00 dm³ flask at equilibrium. Calculate the SO₃ equilibrium concentration.

Warm
1. 2 SO₃(g) ⇄ 2 SO₂(g) + O₂(g) Kc = 1.47x10^-3
4.00 moles of SO₂ and 5.00 moles O₂ are present in a 2.00 dm³ container once at equilibrium. Calculate the equilibrium concentration of SO₃ and the number of moles SO₃ present

Hot
2NO₂(g) ⇌ N₂O₄(g) Two sets of equilibrium data are listed for the same temperature.
Container 1 2.00 dm³ 0.12 moles NO₂ 0.16 moles N₂O₄
Container 2 5.00 dm³ 0.26 moles NO₂ ? moles N₂O₄
Determine the number of moles N₂O₄ in the second container.

Challenge
The following equilibrium is established at temperature T when 1.00 mol of HI is contained. It is found that 22% of the HI has broken down. Calculate Kc.
2 HI(g) ⇌ H₂(g) + I₂(g)