a. Calculating K: A 5.00 dm3 flask at constant temperature contains nitrogen gas, chlorine gas and nitrogen trichloride gas. When the equilibrium system is analyzed it contains 0.0070 mol N2(g), 0.0022 mol Cl2(g) and 0.95 mol NCl3(g). Calculate the equilibrium constant for this reaction.
a. Calculating K:
A 5.00 dm3 flask at constant temperature contains nitrogen gas, chlorine gas and nitrogen trichloride gas. When the equilibrium system is analyzed it contains 0.0070 mol N2(g), 0.0022 mol Cl2(g) and 0.95 mol NCl3(g). Calculate the equilibrium constant for this reaction.
b. Calculating Q – the reaction quotient – (to determine IF a system is at equilibrium):
N2O4(g) ⇌ 2 NO2(g)
|
Experiment |
Initial [N2O4] |
Initial [NO2] |
Equilibrium [N2O4] |
Equilibrium [NO2] |
K |
|
1 |
0.1000 |
0.0000 |
0.0491 |
0.1018 |
|
|
2 |
0.0000 |
0.1000 |
0.0185 |
0.0627 |
|
|
3 |
0.0500 |
0.0500 |
0.0332 |
0.0837 |
|
|
4 |
0.0750 |
0.0250 |
0.0411 |
0.0930 |
|
test |
0.0186 |
0.0626 |
If the gases are present in the above concentrations, is the system at equilibrium?
c. Calculate Equilibrium Concentrations (from Initial concentrations and 1 equilibrium concentration):
An evacuated 2.00 dm3 flask is filled with 0.200 mol of hydrogen iodide. Hydrogen iodide is allowed to decompose into hydrogen and iodine until it reaches equilibrium. You determine that the concentration of hydrogen iodide at equilibrium is 0.078 mol dm-3. Calculate the concentrations of the other gases at equilibrium and then find K.
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