|Exercise: Chemical Equilibrium||
1. Consider the reaction
Note that heat appears on the product side - the system is giving up heat, therefore H is negative, H = - 92.2 kJ
Using Le Châtelier's Principle, predict what will happen to [NH3] if:
- N2 is added?
- H2 is removed?
- T is decreased?
- Ar is added?
Predict how the equilibrium will shift (right, left, or neither) if:
- V is increased?
2. Consider the gas phase reaction:
2 HI H2 + I 2
Keq = 2.06 x 10-2 @ 458°C
If both hydrogen and iodine are measured to have concentrations of 0.0135 M each at 458°C, what is the concentration hydrogen iodide?
3. Consider the gas phase reaction:
2 HBr H2 + Br2
Keq = 1.5 x 10-5 @ 1400 K
Calculate the concentrations of all species at equilibrium if we start with 0.15 moles each of hydrogen bromide and bromine in a 0.500 L container at 1400 K.
4. Consider the gas phase dissociation of carbon dioxide to carbon monoxide and oxygen @ 1000 K.
If 0.200 moles of carbon dioxide is placed in a 1.00 L container at 1000 K calculate the concentrations of all species at equilibrium. Keq = 4.5 x 10-23 @ 1000 K.
In addition to these exercises you should familiarize yourself with text materials.
© R A Paselk
Last modified 4 December 2008