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1. There are three parts to this question. 2 moles of gaseous PCl5, are heated at...

1. There are three parts to this question. 2 moles of gaseous PCl5, are heated at 502 K till equilibrium is reached at a total pressure of 1 atm. (a) Calculate the composition at equilibrium and also the percentage of PCl5 decomposed at 502 K. (KoP = 0.46). (b) If the pressure of the system given in part (a) is raised to 10 atm at the same temperature of 502 K, calculate the percent of PCl5 decomposed. Compare your results in part (a) and part (b) and explain the significance of increasing the pressure of the system for the decomposition of PCl5. (c) If the system already contains 1 mole of Cl2 in addition to the 2 moles of PCl5, calculate the percent of PCl5 decomposed. The equilibrium pressure under this condition is 1 atm.

Solutions

Expert Solution

The decomposition reaction is:

Now, we know that:

Where:

Xi is the mole fraction of the compound i

Then:

Using the ICE table:

So:

We know by the Le Chatelier's principle, if we raise the pressure, the equilibrium move towards to the side with more number of moles. Then:

If the initial number of moles are:

Then, we have to make a new ICE table:

queen_honey_blossom answered 1 year ago

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