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

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

Decide whether each of the following statements is true or false.  If false, change the wording of the statement to make it true.   a) The magnitude of the equilibrium constant is always independent of temperature. b) When two chemical equations are added to give a net equation, the equilibrium constant for the net equation is the product of the equilibrium constants of the summed equations. c) The equilibrium constant for a reaction has the same value as K for the reverse reaction.  d) Only the concentration of CO2 appears in the equilibrium expression for the reaction: CaCO3 (s) ↔ CaO (s) + CO2 (g). e) For the reaction CaCO3 (s) ↔ CaO (s) + CO2 (g), the value of K is numerically the same whether the amount of CO2 is expressed as molarity or as gas pressure.

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

|For the equilibrium system CuO (s) + CO (g) = Cu (s) + CO2 (g), predict the effect that the indicated stress will have on the specified quantity. a) The effect of adding CO on the amount of Cu (s) b) The effect of adding CO2 on [CO] c) The effect of removing CuO on the [CO2] d) The effect of a catalyst on the amount of Cu (s) Do any of the stresses affect the value of K?

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

Consider the equilibrium reaction. 3A +B= 2C After multiplying the reaction by a factor of 2, what is the new equilibrium equation? new equilibrium equation: 6A + 2B = 4C Create the equilibrium-constant expression, K, for the new equilibrium reaction. Answer Bank IAP Ke = [B) [B) LA Answer Bank [C] [AP K = [B] (B] [B] (A) If the initial reaction contains 1.79 M A, 1.53 M B, and 2.39 M C, calculate K, for the new equilibrium reaction. K = Incorrect

What effect will adding additional O2 (g) to the following equilibrium system have, once equilibrium is reestablished? 2 CO2 (g) 2 CO (g) + O2 (g) ∆H ̊ = -514 kJ a) The concentration of CO(g) will increase b) The concentration of CO2 (g) will decrease c) The equilibrium constant for the reaction will increase d) The concentration of CO2 (g) will increase

Consider the equilibrium  2NO(g)⇌N2(g)+ O2(g) For which ΔH = -180kJ mol-1 how will adding H2(g) affect an equilibrium mixture of the three gases? a) Reaction will proceed to the left to generate more reaction b) reaction will proceed to the right to generate more product c) there will be no change to the equilibrium mixture

Please explain why the answer you get is correct. Thank you very much for all of your help!