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)Using Le Chatelier's Principle, What will happen to the number of moles of SO3 in equilibrium with SO2 and O2 in the reaction? 2SO3(g) ⇌ 2SO2(g) + O2(g) in each of the following cases: 1. Oxygen is added to reaction container. 2. The pressure is increased by decreasing the volume of the reaction container. 3. In the rigid container (i.e. constant volume), the pressure is increased by adding argon gas. 4. The temperature of the reaction container is decreased (Note:...
1) The reaction below is exothermic 2SO2 (g) + O2(g) ⇌ 2SO3(g) + heat Le Châtelier's Principle predicts that _______ will result in an increase in the number of moles of SO3 (g) in the reaction container. Which direction will the reaction shift: ? left or right A) increasing the volume of the container B) increasing the amount of SO2 C) removing some oxygen D) increasing the temperature E) decreasing the pressure 2) Consider the following reaction at equilibrium: 2SO2 (g) + O2 (g) ⇌ 2SO3 (g) + heat ΔH...
Le Chatelier's Principle 3. For Part Ill, use Le Châteller's Principle to explain the colour changes observed in test tubes 2 and 3 upon the addition of HC and A . Also, explain the observed colour changes in the test tubes placed in hot and cold water. (4 marks) Test Tube 2: Test Tube 3: Hot Water bath: Cold Water bath: Extension: 1. NaCl(aq) + HCl(aq) = NaCl(aq) + H2O + Cl2(g) When the above system is cooled, gas bubbles...
According to Le Chatelier’s Principle, does the equilibrium shift in the direction of products or reactants when O2 is added to the equilibrium mixture of each of the following reactions? 3O2 (g) ↔ 2O3 (g) 2. 2CO2 (g) ↔ 2CO (g) + O2 (g) 3. 2SO2 (g) + O2 (g) ↔ 2SO3 (g) 4. 2SO2 (g) + 2H2O (g) ↔ H2S (g) + 3O2 (g)
8.53 Use Le Châtelier's principle to predict the direction of equi- librium shift and the changes that will be observed (color, amount of precipitate, etc.) in the following equilibria when the indicated stress is applied: a. heat +Co2 (aq) +4CI (aq)2 COCL (aq); colorless blue pink The equilibrium mixture is heated. b.heat+Co2 (aq) + 4CI (aq)e CoCL (aq); blue pink is added to the equilibrium mixture. colorless Co c. Fe3 (aq) + 6SCN (aq) Fe(SCN),(aq); red brown colorless SCN is...
For the following endothermic reaction system at equilibrium: 2SO3(g) <---> 2SO2(g) + O2(g) Choose the changes that will shift the equilibrium position to the right. (Select all that apply.) Add Ne(g) Add SO2(g) Remove SO3(g) Decrease temperature Add a catalyst Increase temperature Decrease volume
The general form of a chemical reaction is aA + bB = cC +dD Where A and B are reactants in the forward direction and C and D are products in the forward direction. The lower case letters are the stoichiometric coefficients for the balanced equation. The general form of the equilibrium constant equation is then: Keq = [C]c[D]d/[A]a[B]b Part I: Q vs. K Q: reaction quotient can be calculated for a reaction at any concentration values of reactants and...
Using Le Chatelier's Principle to predict the result of changing Nitrogen monoxide and ozone react to form nitrogen dioxide and oxygen, like this: The reaction is exothermic. Suppose a mixture of NO, O, NO2 and O2 has come to equilibrium in a closed reaction vessel. Predict what change, if any, the perturbations in the table below will cause in the composition of the mixture in the vessel. Also decide whether the equilibrium shifts to the right or left. shift in...
Thermochemical equations 5. Given 2NO → N2 + O2 ∆H= -180.7 determine the enthalpy of the reverse reaction? Is the reverse reaction endothermic or exothermic? 6. Given H2 + F2 → 2HF ∆H= -537 kJ a) How much heat is required to react 9.5 g F2 with H2? b) What mass of H2 is needed to react with F2 with -294 kJ of energy? Hess Law State Hess’s Law 8. Use the standard reaction enthalpies given below to determine ΔH°...
A reaction vessel contains an equilibrium mixture of SO2, O2,, and SO3. The reaction proceeds such that: 2SO2 (g) + O2 (g) ----> <---- 2SO3 (g) The partial pressures at equilibrium are Pso2=0.001111 atm PO2 = 0.002728 atm PSO3 =0.0166 Calculate the Kp for the reaction.