Week 1 IBDP2 HL - Equilibria Kc calculations

Last updated over 1 year ago

8 questions

Instructions

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.

Week 1 IBDP2 HL - Equilibria Kc calculations

Last updated over 1 year ago

8 questions

Instructions

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 H2 are 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)