Answer:
Which of the following equilibria will shift towards the formation of more products if the reaction...
Which of the following equilibria will shift towards the formation of more products if the reaction at equilibrium is compressed into half its volume? 1. 2N2O(g) = 2N2(g) + O2(g) II. 2CO(g) + O2(g) = 2CO2(g) III. N2(g) + O2(g) = 2NO(g) Both II and III. All three reactions will shift towards the formation of more products.
which of the following equilibrium systems will shift to the right towards the product when the pressure is increased Which of the following equilibrium systems will shift to the right (towards products) increased none of these PC15 (8) - PC13 (s) + C12 (8) all of these 2 Pb (s) + 302 (g) — 2PbO (s) + 2 502 (g) - CH4 (g) + 2O2 (g) → 2H20 (8) + CO2 (g)
Which of the following equilibria will shift to the left when the temperature is increased? [AH (kl/mol) values are given in parentheses.] (Select all that apply.) (a) S + H2 SH2S AH(-20) (b) C + H2O 55CO + H2 AH (131) (c) H2 + CO2= H2O + CO NH(41) (d) MgO + CO2 = MgCO3 AH (–117) (e) 2CO + O2 = 2CO2 AH (-566)
2. A) Which way will the equilibrium of a reaction shift (towards reactants or products) if one of the products formed is a gas? Which way will the equilibrium of a reaction shift (towards reactants or products) if one of the reactants formed is a solid? B) Using what you just described above, examine the following reactions and apply Le Chatelier's principle. Which way will the equilibrium shift? (Towards reactants or products) Circle the dominate side of the reaction. Explain...
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)
+2H2(g)+ CH4(g) +CO2(g)--2CO(g) Δ Predict which direction the equilibrium will shift (left, towards reactants or right, towards products) when you perform the following actions: ft Left Shift Right Action Add CH4s to the reaction Add CO2 to the reaction Add CO to the reaction Add H2 to the reaction Remove CHs from the reaction Remove CO2 from the reaction Remove CO from the reaction Remove H2 from the reaction Increase pressure by reducing volume Cool the reaction mixture Heat the...
Which of the following would increase the yield of the products of the following endothermic reaction? 2H2O(g) + 2Cl2(g) 4HCl(g) + O2(g) ΔH > 0 Question 14 options: 1) Decreasing the temperature of the reaction 2) Adding HCl to the reaction vessel 3) Decreasing the volume of the container 4) Removing Cl2(g) from the reaction vessel 5) Increasing the volume of the container
1. Determine Kp for the following reaction at 315 °C, given that Ke at the same temperature is 1.25 N: (g) +3 H: (g)2NHs (g) 2. Given the following stepwise equilibria, determine the net reaction and the value of Ks. 3. 3. Determine Qe for the following equilibria, compare to K, and state the direction of shift as either "towards products" or "towards reactants". a) H:(g) +h (g) 2 HI (g) Conditions: [H2]s [l;l = [HI] = 0.0020 M, T...
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...
Consider the following equilibrium systems. Which direction will the reactions shift (reactants or products) when cooled? 2CO(g) + O2(g) = 2CO2(8) H2(g) + 12(g) = 2HI(g) H2(g) + 12(s) = 2H1(2) 12(g) = 21(2) AH = -566 kJ AH = -2.70 kJ AH = +53.0 kJ AH = +36.2 kJ _ a. reactants, reactants, reactants, reactants b.reactants, reactants, products, products c. products, products, products, products d. products, products, reactants, reactants | 0 0 0 0