Question

Is the statement true or false, with respect to the specified reaction in each case?

H2(g) + F2(g)<-->2HF(g)
If a vessel, containing an equilbrium mixture of these gases, is pressurized by adding helium gas, then the equilibrium position will shift to the right.

2SO3(g)<-->2SO2(g) + O2(g)
If an equilbrium mixture of these gases is released into a vessel of larger volume, then the equilibrium position will shift to the right.

Fe3+(aq) + SCN-(aq)<-->FeSCN2+(aq)
If KOH is dissolved in this solution, then the equilibrium position will shift to the left. (Note that Fe(OH)3 is insoluble.)


H2O(g) + CO(g)<-->H2(g) + CO2(g)
If CO gas is removed from an equilbrium mixture of these gases, then the equilibrium position will not shift.


2SO3(g)<-->2SO2(g) + O2(g) (Endothermic)
If the temperature is decreased, then the equilibrium constant for this reaction equation will remain the same.

Answer 1

According to the Le-Charterlier's principle ,

(1) If the temperature is raised , reaction will proced in the direction in which some heat can destroy(absorbed) so that temperature of the systemremains constant.

Thus increase in temperature shifts the equilibrium in the forward direction of those reactions which proceed with absorption of heat (endothermic reactions), and in the back ward direction of those reactions which proceed with the evolution of heat ( exothermic reactions)

(2) If the pressure is increased , reaction will takes place ina direction which will bring about lowering of pressure.This implies that theequilibrium will shifts in the direction which produces the smaller no . of gas molecules.

(3)If the concentration of reactants is increased or product is removed , the reaction will take place in the forward direction.

(4) Catalyst speeds up both forward &backward reactions to the same extent but does not have any effect on Equilibrium point.

(5)---> When the no. of moles of reactants &products are same the addition of inert gas has no effect

----> for a reaction at constant preure ,addition of an inert gas will shifts the equilibrium in the direction in

which thereisincrease in the no . of moles of the gases

H2(g) + F2(g)<-->2HF(g)
If a vessel, containing an equilbrium mixture of these gases, is pressurized by adding helium gas, then the equilibrium position will shift to theright.(False)
Since no. of moles of reactants &products are same the addition of inert gas has no effect
2SO3(g)<-->2SO2(g) + O2(g)
If an equilbrium mixture of these gases is released into a vessel of larger volume, then the equilibrium position will shift to the right.(true)

Fe3+(aq) + SCN-(aq)<-->FeSCN2+(aq)
If KOH is dissolved in this solution, then the equilibrium position will shift to the left. (Note that Fe(OH)3 is insoluble.) (False)
---> since we are increasing the concentration of the reactants ---> right side
H2O(g) + CO(g)<-->H2(g) + CO2(g)
If CO gas is removed from an equilbrium mixture of these gases, then the equilibrium position will not shift.(false)---> since we are decreasing the concentration of the reactants --->left side
2SO3(g)<-->2SO2(g) + O2(g) (Endothermic)
If the temperature is decreased, then the equilibrium constant for this reaction equation will remain the same.(false)Since K = Ae^(-Ea/RT)WhereA = constantEa = activation energyT = absolute temperatureR = gas constantSo Equilibrium constant , K depends upon T