1. Using LeChâtelier’s principle, determine whether the reactants or products ar
ID: 1009755 • Letter: 1
Question
1. Using LeChâtelier’s principle, determine whether the reactants or products are favored and the direction of the shift in equilibrium (left or right) in the following examples. 2CO(g) + O2(g) 2CO2(g) + heat
a. Remove O2
b. Lower the temperature
c. Add CO
d. Remove CO2
e. Decrease pressure
2. Consider the following equilibrium reaction for the production of sulfur trioxide. SO2(g) + O2(g) SO3(g) Hº = -196.6 kJ
a. Write a balanced equation with the heat value on the proper side of the equation.
b. Determine the shift in equilibrium (left or right) and if the concentration of the reactants or products increases in the following examples. • Adding more SO3 • Removing heat • Increasing pressure by decreasing the volume, because reactants and products are gases
c. Adding more SO2
d. Removing O2
e. Removing SO3
Explanation / Answer
1) 2CO(g) + O2(g) -------> 2CO2(g) + heat
a) Removel of Oxygen:
Equilibrium moves towards the left side (reactants) because the reactants concentration is decreasing.
According to the LeChâtelier’s principle equilibrium moves towards the lower concentration side.
b) Lower the temperature:
The reaction is the Exothermic reaction, If we decrease the Temperature the reaction moves towards the right side (towards the products).
c) Add CO:
Add CO means Increase the concentration of the one of the reactant, Hence the reaction moves towads the right side (product formation side).
d) Remove CO2:
Here Removel of CO2 means concentration of products decreasing, That means the reaction moves towards the lower concentrated products side (right side).
e) Decrease pressure:
The reactans and the products are gases. Hence, decreasing the pressure can show the same influence on reactants and products that means no change in the equilibrium.
2) a) 2SO2(g) + O2(g) --------> 2SO3(g) Hº = -196.6 kJ (Balanced equation)
b) Adding more SO3:
Products concentration increasing, equilibrium moves towards the lower concentration side means left side.
Removing heat:
It is the Exothemic reaction means, The equilibrium moves towards the right side.
Increasing pressure by decreasing the volume:
All are gases can show the same influence that means no change in the equilibrium.
c) Adding more SO2:
Increasing the concentration of the reactants, That means equilibrium moves towards the right side.
d) Removing O2:
Here, Decreasing the concentration of reactants means the equilibrium moves towards the left side.
e) Removing SO3:
Here the concentration of the product decreasing, That means the equilibrium moves towards the right side.
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