# Chemical Equilibrium Pre and P

1) The given reaction is

N2 + 3 H2 ——-> 2 NH3 +heat

Heat is a product of the reaction, i.e, the reaction releasesheat into the surroundings. Hence, ΔH for the forward reaction(formation of NH3 from N2 and H2)has negative value and consequently, the reverse reaction(decomposition of NH3 to form N2 andH2) has positive ΔH (ans).

I explained the answer; however choices (a) and (b) are bothsame. Kindly check the question and choose the correct option.

2) The equilibrium reaction is

N2O4<======> 2 NO2 ; ΔH =56.9 kJ

The equilibrium constant is

K =[NO2]2/[N2O4]

K remains constant at a particular temperature.

When excess NO2 is added, [NO2] increasesand hence [N2O4] must increase to keep Kconstant. This is possible only when the equilibrium shifts in thereverse direction, producing more N2O4.

Therefore, (c) is the correct statement.

3) Assume ideal behavior of the gases. The pressure of an idealgas is inversely proportional to the volume. Again, as per the gaslaw, the volume of an ideal gas is directly proportional to thenumber of moles of the gas. Therefore, the higher the number ofmoles of gases, the higher is the volume and consequently, thelower is the pressure.

When the pressure is lowered, the equilibrium will shift in thedirection where the number of moles of gases is more. Since theforward reaction proceeds with an increase in the number of molesof gaseous products, hence the equilibrium shifts to the right.Therefore, statement (b) is correct.

4) The enthalpy change for the reaction is positive. Hence thereaction is endothermic. Endothermic reactions are favored by hightemperatures, hence the equilibrium shifts to the right, producingmore NO2. Thus, statement (b) is correct.

5) A catalyst alters the rate of both the forward and thereverse reactions, but keeps the position of the equilibriumunchanged. Hence, a reaction at equilibrium is unaffected by theaddition of a catalyst. Statement (d) captures the correctessence.

6) The equilibrium constant, Keq depends only on thetemperature of the system. Any effect that aims to change thetemperature of the system will alter the value of Keq.Since statements (b) and (c) both describe a change in temperature(b increases the temperature while c reduces the temperature).Hence, both the processes will change the value of Keq.Therefore, both (b) and (c) are correct.

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