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Consider the reaction: 2N2O(g) + O2(g) + 2N768). Which of the following will cause a shift...
Consider the reaction: 2N2O(g) = O2(g) + 2N2 (g). Which of the following will ensure the reaction proceeds to completion. 1. Remove o 2. Remove 3. Add Neither 1.2 or 3 1 and 3 only O 2 only 2 and 3 only All of 1, 2, and 3
Question 10 4 pts Consider the reaction: 2N2O(g) = O2(g) + 2N2 (g). Which of the following will ensure the reaction proceeds to completion. 1. Remove o 2. Remove 3. Add 1 and 3 only 2 and 3 only Neither 1.2, or 3 All of 1, 2, and 3 2 only Question 7 4 pts When an acid is reacted with a base the expected products would be? HTML Editora B I VA A - IX E 331 XX, EE...
2. Consider the reaction: 2 O(g) ⇌ (g) + 2 (g). Which of the following will cause a shift in the equilibrium to the right? 1. Add more O 2. Remove 3. Remove A) 1 and 2 only B) 1 and 3 only C) 2 and 3 only D) All of 1, 2, and 3 E) Neither 1, 2, or 3 please mention which the right answer from the following options given le chatelier's principle
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. Consider the following reaction at equilibrium. CO2(g) + 2 H2O(l) = CH2(g) + 2O2(g) AH° = +890 kJ Which two of the following...
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.
tant " (16) In question (12) the removal of so, (g) will shift the equilibrium to the (a) right (b) left (c) no shift. (17) In question (12) an increase in pressure will shift the equilibrium to (a) left (b) right (c) middle (d) no shift (18) in question (12) assuming the reaction is endothermic to the right, a decrease in temperature will shift the equilibrium to the (a) left (b) right (c) no shift since it is an equilibrium...
Given the following reactions N2 (g) + O2 (g) → 2NO (g) ΔH = +180.7 kJ 2N2O (g) → O2 (g) + 2N2 (g) ΔH = -163.2 kJ the enthalpy of reaction for 2N2O (g) → 2NO (g) + N2 (g) is ________ kJ.
Mark ALL CHOICES that would cause a shift to the REACTANT side for this reaction based on LeChatlier's principle. 2SO2(g)+ O2(g) ⇌ 2SO3(g) + heat Question 2 options: 1) Remove catalyst 2) Remove SO2 3) Decrease pressure 4) Add O2 5) Remove SO3
3. Consider the following reaction at equilibrium. + C(s) + H2O (g) + Heat CO (g) +H, (g) a. Is this reaction endothermic or exothermic? (1 point) 2 b. In which direction (right or left) will the equilibrium shift if the following stresses are applied to the reaction at equilibrium? (4 points) i. Remove heat ii. Add CO (g) iii. Remove H20 (g) iv. Add H2 (g)
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