QUESTION 1 The addition of an acid to the following equilibrium Ag2CO3/(s) 2Ag (

Question

QUESTION 1 The addition of an acid to the following equilibrium Ag2CO3/(s) 2Ag (aq) + Co32 (aq) causes... A shift to the left. More Ag2CO3(s) forms. A shift to the right because Ag+ is removed from the system. A shift to the right because Co3 is removed from the system A shift to the left because CO32- (aq) is added to the system. QUESTION 2 For the following equilibrium [CuH20)12+ (aq)+ 4NH3 [Cu(NH3)42 (aq) +4H20 ) What color would be seen after the addition of an acid? QUESTION 3 For the following equilibrium Agl(s)Ag (aq)(aq) The addition of Na2S causes what species to dissolve? QUESTION 4 For the following equilibrium 4CI(aa)+ [Co2(aq) [CoCl42(a)+6H200 How does the addition of HCI effect the equilibrium It causes a shift right and more reactants are formed It causes a shift left and more products are formed. The addition does not effect the equilibrium It causes a shift to the right and more products are formed QUESTION 5 For the following exothermic reaction 2NO2(g) N2O4(g) +heat How wil the equilibrium shift if heat is added from the system. Hint (answer is one word only)

Explanation / Answer

According to the Le-Charterlier's principle,

(1) If the temperature is raised, reaction will proceed in the direction in which some heat can destroy (absorbed) so that temperature of the system remains 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 in a direction which will bring about lowering f pressure. This implies that the equilibrium 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. If the concentration of reactants decreases or increasing the concentration of products the reaction will take place in the backward 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 pressure ,addition of an inert gas will shifts the equilibrium in the direction in

            which there is increase in the no . of moles of the gases  

Question 1 : Upon addition of acid it reacts with CO3 2- , so that the concentration of the product decreases so the reaction shifts in forward direction that is in the right.

Therefore third option is correct

Question 2 : By the addition of acid it reacts with NH3(base) so the concentration of reactants decreases thereby it proceeds towards in left side so the complex [Cu(H2O)4]2+ is formed more so it appears green blue colour

Question 4: By the addition of HCl the concentration of Cl- increases thereby the concentration of reactants increases so forward reaction takes place.so more products formed.

Therefore last option is correct

Question 5 :Since it is exothermic reaction is forward direction, addition of heat shifts the equilibrium in the back ward direction.

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