5. For the following exothermic reaction, tell how the equilibrium will shift in response to... 2H2O2(aq) + 2H2O(l) + O2(g) (a) allowing O2 to escape. (b) adding H20 [trick question!). no effect forward direction (c) increasing the total pressure. backward direction (d) increasing the temperature. backward reaction (e) justify your answer to part d. exothermic reactions are favoured by decrease in temparature, and endothermic reactions are favoured by increase in temparature. forward reaction is exothermic and backward reaction is endothermic
5. For the following exothermic reaction, tell how the equilibrium will shift in response to... 2H2O2(aq)...
Help please! Show work 5. For the following exothermic reaction, tell how the equilibrium will shift in response to... 2H2O2(aq) = 2H20(1) + O2(g) (a) allowing O2 to escape. (b) adding H20 [trick question!). (c) increasing the total pressure. (d) increasing the temperature. (e) justify your answer to part d.
The following reaction is exothermic. Which change will shift the equilibrium to the right? 2 SO2(g) 02(8)2 S03(g) O A) Adding SO3 O B) Increase volume O c) Increase the temperature OD) Adding catalyst 0 E) Increase pressure
2SO2 (g) + O2 (g) <---> 2SO3 (g) The reaction is exothermic. How does the equilibrium shift at: a) increase of [O2]? b) decrease of [SO3]? c) increase in pressure? d) increase in the volume of the container? e) increase in temperature? f) addition of catalyst?
4. For the following reaction, tell how the equilibrium yield of iron(III) trichloride is affected by... 6C12(8) + 2Fe2O3(s) = 4FeCl3(s) + 302(8) (a) increasing Pa, (b) adding Fe20.. (c) selectively removing O2(e). (d) adding a catalyst. (e) removing part of the FeCl. (1) decreasing the total pressure.
8H2(g) + Se(s) - 8H2S(g) K = 4. For the following reaction, tell how the equilibrium yield of iron(III) trichloride is affected by... 6C12(g) + 2Fe2O3(s) = 4FeCl3(s) + 302(8) (a) increasing Pa, (b) adding Fe2O3. (c) selectively removing O2(g). (d) adding a catalyst. (e) removing part of the FeCl3. () decreasing the total pressure.
The following reaction is exothermic. Which change will shift the equilibrium to the right? 2 SO2 (g) + O2 (g) = 2 So, (9) o Adding So, Decreasing the volume of the reaction flask Removing O2 Heating the reaction QUESTION 11 A positive AGⓇ for a reaction implies The reaction is never spontaneous The products predominate at equilibrium The reaction is always spontaneous The reactants predominate at equilibrium ОО QUESTION 12 Which of the following is TRUE regarding AG and...
Name: 1. An exothermic reaction is allowed to reach equilibrium. If the temperature of the reaction mixture is decreased, the equilibrium will shift towards the product side: True False [1pt] 2. For the reaction C(s) + H2O(g) CO(g) + H2(g) a decrease in concentration of C(s) will cause the reaction to shift to the left oTrue False [1pt] 3. Define the following terms: [1.5pts] a. Activation Energy b. Exothermic Reaction c. Equilibrium [1p) 4. Determine the equilibrium constant K C(s)...
QUESTION 1 The following reaction is endothermic. Which change will shift the equilibrium to the right? 2 503(9) = 2 SO2(g) + O2(9) removing SO3 adding SO2 none of the other answers are correct decreasing the volume (increasing the pressure) decreasing the temperature w
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...
For an exothermic reaction, how does raising the temperature of the reaction shift the equilibrium?