Consider the reaction:
2SO2(g) + O2(g) <--> 2SO3(g) 600°C
In a certain experiment, 2.00 mol of SO2, 1.50 mol of O2, and 3.00 mol of SO3 were placed in a 1.00 L vessel. After the system reached equilibrium, 3.50 mol of SO3 were found to be present.
[O2] at equilibrium
[SO2] at equilibrium
Kc
Calculate Kp for the following reaction:
2NOBr(g) <--> 2NO(g) + Br2(g)
given that a 1.0 L vessel was initially filled with 4.0 atm of pure NOBr, and after equilibrium was established, the partial pressure of NOBr gas was 2.5 atm.
Consider the reaction:
2NOCl(g) <--> 2NO(g) + Cl2(g)
where Kc = 1.55x10-5 at 35°C. In an experiment, 1.0x10-1 mol of NOCl, 1.0x10-3 mol of NO, and 1.0x10-4 mol of Cl2 are mixed in a 2.0 L flask. In which direction will the system proceed to reach equilibrium?
Consider the reaction:
PCl5(g) <--> PCl3(g) + Cl2(g)
6.0 mol of PCl5 are placed in an empty 10.0 L vessel at 230°C. When equilibrium is reached, an analysis of the mixture indicated that 1.0 mol of Cl2 is present.
How many moles of PCl5 are present at equilibrium?
What is the concentration of Cl2 at equilibrium?
What is the value of the equilibrium constant?
Consider the reaction at 700K:
CO(g) + H2O(g) <--> CO2(g) + H2 (g)
The equilibrium constant for the reaction at 700 K is 5.10. Calculate the equilibrium concentrations of all reactants and products in an experiment where 3.00 mol of CO and 3.00 mol of H2O are mixed in a 1.00 L flask at 700 K.
[CO]
[H2O]
[CO2]
[H2]
Consider the following equilibrium:
H2(g) + CO2(g) <--> H2O(g) + CO(g)
with Kc = 0.873. 0.50 mole of H2 is mixed with 0.50 mol of CO2 in a 3.0 L reaction vessel at 2000 K. Calculate the equilibrium concentration of CO at this temperature.
N2O4(g) decomposes according to the equation:
N2O4(g) <--> 2NO2(g)
Pure N2O4 was placed in a closed flask at 127°C at a pressure of 4.38x10-2 atm. After the system reached equilibrium, the total pressure was found to be 7.43x10-2 atm. Caculate the value of Kp for this reaction.
Consider the reaction:
2NH3(g) <--> N2(g) + 3H2(g)
at a temperature where Kc = 3.0x10-8. In an experiment, 1.0x10-3 mol NH3, 1.0x10-1 mo H2, and 1.0 mol N2 are mixed in a 5.0 L vessel.
In which direction will the system shift to reach equilibrium?
Consider the reaction:
CaCO3(s) <--> CaO(s) + CO2(g)
for which Kc = 8.0x10-3 at 750°C
1.00 mol of CaCO3(s) is sealed inoto a 5.0 L flask at 750°C. Calculate the equilibrium concentration of CO2(g).
How many moles of CaO are produced?
Calculate Kp
Kp
In a different experiment at the same temperature, 0.500 mol of SO2 and 0.350 mol of SO3 were mixed in a 1.000 L container. When the system reached equilibrium, 0.0450 mol of O2 was found to be present.
Calculate the equilibrium concentrations of SO2 and SO3.
Answer in the same order as listed above and separate with a comma.