(1)How would you change the volume of the reaction container that holds the foll
ID: 1009106 • Letter: #
Question
(1)How would you change the volume of the reaction container that holds the following reaction in order to increase the yield of SF6? S(s) + 3 F2(g) SF6(g) (a) Increase the volume of the container.(b) Cannot be predicted.(c) Decrease the volume of the container. (d)Do not change the volume of the container.
(2)Consider the following reaction at equilibrium. What effect will adding 1 atm of Ar to the reaction mixture have on the system? 2 H2S(g) + 3 O2(g) 2 H2O(g) + 2 SO2(g)
(e)The reaction will shift to the left in the direction of reactants.
(3)What will happen to the following exothermic reaction at equilibrium if the pressure is decreased?
N2(g) + 3H2(g) 2NH3(g)
(e)The reaction will shift to the left in the direction of reactants.
(3)What will happen to the following exothermic reaction at equilibrium if the pressure is decreased?
N2(g) + 3H2(g) 2NH3(g)
Explanation / Answer
According to Le Chatelier’s Principle, at equilibrium if a system is subjected to a change of thermodynamics quantities like concentration, temperature or pressure; the equilibrium of system shifts in that direction which undo the effect of the change of these thermodynamics quantities.
Le Chatelier’s Principle mainly explains three different equilibrium changes:
1. Equilibrium change due to change in the concentration of the system.
2. Equilibrium change due to change in the volume or pressure of the system.
3. Equilibrium change due to change in the temperature of the system
(1)How would you change the volume of the reaction container that holds the following reaction in order to increase the yield of SF6? S(s) + 3 F2(g) SF6(g)
(a) Increase the volume of the container.(b) Cannot be predicted.(c) Decrease the volume of the container. (d)Do not change the volume of the container.
The correct answers is decrease the volume.
If equilibrium of gaseous of molecules is condensed than the pressure of equilibrium is increased. This increased pressure will be partially relieved by a shift of equilibrium in the less gaseous molecules.
(2)Consider the following reaction at equilibrium. What effect will adding 1 atm of Ar to the reaction mixture have on the system? 2 H2S(g) + 3 O2(g) 2 H2O(g) + 2 SO2(g)
(a)No effect will be observed.
(b)The equilibrium constant will increase.
(c)The reaction will shift to the right in the direction of products.
(d)The equilibrium constant will decrease.
(e)The reaction will shift to the left in the direction of reactants.
No effect will be observed because Ar neither reactant not product.
(3)What will happen to the following exothermic reaction at equilibrium if the pressure is decreased?
N2(g) + 3H2(g) 2NH3(g)
(a)More N2 and H2 will be produced.
(b)There will be no change in concentrations.
(c)More NH3 will be produced.
(d)Less N2 and H2 will be produced.
If equilibrium of gaseous of molecules is expanded than the pressure of equilibrium is decreased. This decreased pressure will be partially restored by a shift of equilibrium in the more gaseous molecules.
Thus the correct answer is (a)More N2 and H2 will be produced.
(a)No effect will be observed.
(b)The equilibrium constant will increase.
(c)The reaction will shift to the right in the direction of products.
(d)The equilibrium constant will decrease.
(e)The reaction will shift to the left in the direction of reactants.
No effect will be observed because Ar neither reactant not product.
(3)What will happen to the following exothermic reaction at equilibrium if the pressure is decreased?
N2(g) + 3H2(g) 2NH3(g)
(a)More N2 and H2 will be produced.
(b)There will be no change in concentrations.
(c)More NH3 will be produced.
(d)Less N2 and H2 will be produced.
If equilibrium of gaseous of molecules is expanded than the pressure of equilibrium is decreased. This decreased pressure will be partially restored by a shift of equilibrium in the more gaseous molecules.
Thus the correct answer is (a)More N2 and H2 will be produced.
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