2 NOBr(g) 2 NO(g) + Br,(g) AH = 16.1 kJ How does the equilibrium shift after the following stresses? d) Increase the container volume Which way does it proceed? A) Forward B) Reverse C) Neither D) Can't say Which way does it proceed? A) Forward B) Reverse C) Neither D) Can't say e) Add a catalyst f) Add some N2 Which way does it proceed? A) Forward B) Reverse C) Neither D) Can't say

2 NOBr(g) 2 NO(g) + Br,(g) AH = 16.1 kJ How does the equilibrium shift after the following stresses? d) Increase the container volume Which way does it proceed? A) Forward B) Reverse C) Neither D) Can't say Which way does it proceed? A) Forward B) Reverse C) Neither D) Can't say e) Add a catalyst f) Add some N2 Which way does it proceed? A) Forward B) Reverse C) Neither D) Can't say

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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= The reaction 2HBr(g) ⇒ H₂(g) + Br₂(g) measures [HBr] = 0.177 M, [H₂] = 0.223 M, and [Br₂] = 0.111 M after 5 seconds. If Kc = 1.05 at 25°C, in which direction is the reaction moving to reach equilibrium? Q = 0.790, moving forward (to the right) to reach equilibrium Q = 0.140, moving forward (to the right) to reach equilibrium Q = 0.140, moving reverse (to the left) to reach equilibrium Q = 0.790, moving reverse (to the left) to reach equilibrium
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Canvas n Question 51 Consider the equilibrium system below at 25 C. A2 (g) + B2 (9) 2 AB (g) Which is correct if, at equilibrium, [A] = 0.130 M, [B] = 0.110, and [AB] = 1.72 M? AGO = AGO 13.2, and equilibrium is reactant rich -13.2, and equilibrium is reactant - rich AGO = -13.2, and equilibrium is product - rich O AGOⓇ 13.2, and equilibrium is product - rich = 1 Question 52 ute the reaction below between H3CCN and KOH.
When a chemical reaction is at equilibrium, Q (the reaction quotient) is equal to K (the equilibrium constant). If a stress is applied to the mixture that changes the value of Q, then the system is no longer at equilibrium. To regain equilibrium, the reaction will either proceed forward or in reverse until Q is equal to Konce again. Alternatively, equilibrium can be disrupted by a change in temperature, which changes the value of K. The result however is the same, and the reaction will proceed forward or in reverse until Q is equal to the new K. Le Châtelier's principle summarizes this idea: If a stress is applied to a reaction mixture at equilibrium, a net reaction occurs in the direction that relieves the stress.
For the following endothermic reaction equilibrium: 2S03 (g) = 2S02 (g) + 02 (g) Decide if each of the following changes will increase the value of K (T= temperature) Yes add S03 No add a catalyst No decrease the volume Yes increase the T No add NE (g) Yes decreased the T Remove S03
2NO+O₂ → 2NO₂ AH = -27.18 kJ/mol of NO₂ This system is at equilibrium. Increasing the temperature of the system will cause: a decrease in the volume of the system a) b) a decrease of [NO] c) an increase [NO₂] d) an increase in the [0₂] e) no observable reaction
The following system is at equilibrium:X(s) + 3Y(g) = Z(g)Classify each of the following actions by whether it causes a leftward shift, a rightward shift, or no shift in the direction of the net reaction. Drag the appropriate items to their respective bins. • View Available Hint(s) Reset Help Add more X Increase the volume Remove some X Decrease the volume Leftward shift Rightward shift No shift
1. 2NO(g) + O₂(g) ⇒ 2NO₂(g) Consider the reaction Which would decrease the partial pressure of NO₂(g) at equilibrium? A) Increasing the volume of the system B) Adding a noble gas to increase the pressure of the system C) Adding NO(g) to the system D) Adding an appropriate catalyst E) Decreasing the volume of the system for which ΔΗ<0.
The synthesis of CaCO3 uses this chemical reaction. CaO(aq) + CO2(g) ——> CaCO3(s) + 180 kJ Identify three stresses that can be imposed on the equilibrium to maximize the amount of CaCO3 present. Be specific about what, if any, compounds are involved in those stresses.
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6. For the following reaction at equilibrium, which change will cause the equilibrium to shift to the right? 2NOBr(g) 2NO(g) + Bra(g) AH = +30 kJ/raw a) Decrease the container volume. b) Add some NO(g). c) Remove some NOBr(g). d) Increase temperature. e) Add a catalyst.
3.) For the following equilibrium reaction2NO2(g) ↔N2O4(g) + Δlook in the Tro text to see what LeChatelier's principle states about gases. Assume that the reaction occurs in an enclosed movable piston. [Hint: remember that PV=nRT] a.) The pressure of the reaction is increased. b.) The volume of the reaction is decreased. c.) The volume of the reaction is increased.