For each of the following reactions: (a) Write the Equilibrium expression (b) Ca

Question

For each of the following reactions: (a) Write the Equilibrium expression (b) Calculate the Equilibrium Constant, Kc (c) Determine the DIRECTION of the reaction (d) Determine if the reaction is in Equilibrium (e) Determine the effect of INCREASING the temperature (f) Determine the effect of increasing the concentration of ONE of the reactants. (g) Determine the effect of increasing the volume of the container. (h) Determine the effect of increasing the Pressure in the container. Reaction 1: N204(g) 2NO2(g) Reaction 2: CO2(g) + H20(I) H2CO3(aq) Each reaction is allowed to come to equilibrium, and then the volume is changed as indicated. Predict the effect (right shift, left shift, or no effect) of the indicated volume change. (a) CO(g) + H2O(g) CO2(g) + H2(g) (volume is decreased) (b) PCI3(g) ? CI2(g) PCI5 (g) (volume is increased) (c) CaCO3(s) CaO(s) + CO2(g) (volume is increased) The following reaction Is endothermic: NH_3 (g) + H2O(I) NH4OH (aq) (a) What is the value of the Equilibrium Constant, Kc, for this reaction. (b) What is the effect of of increasing temperature of the reaction mixture. (c) What is the effect of decreasing temperature of the reaction mixture

Explanation / Answer

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Reaction -1

    2 NO2 (g) <=> N2O4 (g)

a)Equilibrium expression for reaction –

[NO2 (g)]2/[N2O4(g)]

b) The Equilibrium Constant Kc -

The Equilibrium Constant Kc =[NO2 (g)]2/[N2O4 (g)]

c) Direction of reaction-

Addition of NO equilibrium shift to the right

Addition of NO equilibrium shift to the left

Removal of NO equilibrium shift to the left

Removal of NO equilibrium shift to the right

d) At equilibrium the forwards and reverse rates are equal

The forward rate = kf [N2O4]

The reverse rate = kr [NO2]2

e) Effect of increasing the temperature –

Reaction is endothermic, so increasing temperature reaction shift to the right. The intensity of the brown color increases as the temperature increases.   Therefore, an increase in temperature yields more NO2.

f) Effect of increasing concentration of one reactant-

Addition of NO equilibrium shift to the right

Addition of NO equilibrium shift to the left

g)

Increase in container volume, so decrease in pressure. Equilibrium shift to the right.

h) Increase in pressure, decreases volume of container so equilibrium shifts to the left.

Reaction -2

CO2 (g) + H2O (l) ===== H2CO3 (aq)

a)Equilibrium expression for reaction –

[H2CO3]/[CO2]

b) The Equilibrium Constant Kc –

Kc =[H2CO3(aq)]/[CO2(g) ]

c) Direction of reaction-

Addition of H2CO3 equilibrium shift to the right

Addition of CO2 equilibrium shift to the left

d) At equilibrium the forwards and reverse rates are equal

The forward rate = kf [H2CO3]

The reverse rate = kr [CO2]

f) Effect of increasing concentration of one reactant-

Addition of H2CO3 equilibrium shift to the right

Addition of CO2 equilibrium shift to the left

CO2 increased in above equilibrium so more carbonic acid is formed.

g) Increase in container volume, no effect.

h) Increase in pressure, no effect

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