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# Equilibrium Constant and LeChatelier's Principle

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1, Calculate Ke for the following (equilibrium concentrations given below substances)

a) PCl5 (g) + heat &#8596; PCl3 (g) + Cl2 (g)
[0.105] [0.219] [0.219]

b) 2 SO2 (g) + O2 (g) &#8596; 2 SO3 (g) + heat
[0.0500] [0.0500] 0.103]

c) CO2 (g) + H2 (g) &#8596; CO (g) + H2O (g)+ heat
[0.245] [0.245] 0.575] [0.575]

2. For each of the equilibria in problem #1 predict (1) how Ke is affected by an increase in temperature, (2) predict how the equilibrium will shift when pressure is decreased, (3) predict how the equilibrium will shift when the concentration of the underlined substance is increased, and (4) predict how the equilibrium will shift when the temperature is decreased.

https://brainmass.com/chemistry/chemical-equilibrium/equilibrium-constant-and-lechatelier-s-principle-257921

#### Solution Summary

This solution explains how to calculate K values based on given concentrations and explains how the following factors will affect the equilibriums:

1) Increase in temperature
2) Decrease in pressure
3) Concentration of one species is increased.
4) Decrease in temperature

\$2.19

## Equilibrium Constants and LeChatelier's Principle

1. For a certain chemical reaction, &#61508;H&#61616;= -156 kJ. Assuming the reaction is at equilibrium, classify each of the following actions by whether it causes a leftward shift, a rightward shift, or no shift in the direction of the net reaction.
a. a decrease in temperature R L no shift
b. an increase in temperature R L no shift

2. The K of the reaction:
NO2(g) + NO3(g) &#61683;N2O5(g)
a. at equilibrium the concentration of products and reactants is about the same
b. at equilibrium the concentration of products is much greater than the concentration of reactants
c. at equilibrium the concentration of reactants is much greater than that of the products
d. there are no reactants left over once the reaction reaches equilibrium

3. For the reaction HCONH2(g)&#61683;NH3(g) +CO(g); K = 4.84 at 400K What can be said about this reaction at this temperature?
a. The equilibrium lies far to the right (Guessed this and was wrong)
b. The reactions will proceed very slowly
c. the reaction contains significant amounts of products and reactants at equilibrium
d. the equilibrium is far to the left

4. The industrial production of lime (CaO) from calcium carbonate is accomplished via the following reaction: CaCO3(s) &#61683;CaO(s) + CO2(g)
Given the following data:
Temperature (K) K
298 1.93*10-23
1200 1.01