For questions 9-13. Consider the reaction 2NOCI(g) = 2NO(g) + C12(g). If this reaction is at equilibrium, what happens when the following changes occur? 13. The container volume is decreased. shift to right shift to left no reaction both shifts to right and left

For questions 9-13. Consider the reaction 2NOCI(g) = 2NO(g) + C12(g). If this reaction is at equilibrium, what happens when the following changes occur? 13. The container volume is decreased. shift to right shift to left no reaction both shifts to right and left

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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Which equilibrium shows a increase in [products] when the volume increases? 1.2H₂(g) + O₂(g) 2H₂O(g) II. Cl₂(g) + PCl3(g) PC15 (g) III. H₂(g) + 1₂(g) 2HI(g) IV. 2NH3(g) N2 + 3H₂(g) III and IV IV || I and II OI
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12. Use Le Châtelier's principle to predict what will happen if the temperature of the following equilibrium system is decreased. The reaction in the forward direction is endothermic. 4C1 Co(H₂O) pink 1 CoCl₂ + 6H₂O purple/blue A) The equilibrium will shift to the left. B) The equilibrium solution will become more purple. C) The equilibrium will shift to the right. D) The concentration of chloride ion will decrease. E) There will be no change.
7. Given the following equilibrium systems, note the direction the equilibrium will shift [→,-, NC, no change] when the named "stress" is applied. 2 NH3(g) + 92.5 kJ a 1 2 3 4 5 6 7 Stress Remove N2 (g) Add NH3 (9) Remove H2 (9) Remove NH3 (g) Add O2 (g) Decrease Pressure Add Heat N2(g) + 3 H2 (g) Equilibrium Shift
Consider the following equilibrium: Cl2(3) + F2(3) = 2CIF(g) with Keg = 19.9 If we begin with O.100 atm chlorine and 0.100 atm fluorine, what are the partial pressures of CIF and F2 at equilibrium? O 0.20 atm, 0.0 atm O 19.9 atm, 0.00 atm 0.138 atm, 0.031 atm 0.182 atm, 0.009 atm O 0.10 atm, 0.050 atm
Question 5 Consider the equilibrium reaction: N2(g) + t 3 H2(g) 2 NH3(g) AH = -91.8 kJ (exothermic) Using Le Chatelier's Principle, select all methods that this equilibrium can be shifted to the right to increase production of NH3. Please select all correct responses. There is more than one correct answer. a. Increase [H2] Ob. Decrease [H2] O c. Increase [N2] ☐ d. Decrease [N2] Oe. Increase [NH3] ☐ f. Decrease [NH3] ☐ g. Increase the pressure on the system. ☐ h. Decrease the pressure on the system. ☐ i. Increase the temperature on the system. Oj. Decrease the temperature on the system. A Moving to another question will save this response. CH 5p
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.
4 NH3(g) +5 O2(g) = 4 NO(g) + 6 H,0(g) AH =-904.4 kJ Consider the equilibrium system represented in the reaction above. Will the concentration of NO increase, decrease, or remain the same when the following experimental changes are made: a. NH, is added d. The volume of the container is reduced b. [H,O] is increased e. A catalyst is added c. O, is removed f. The temperature is increased
For items 4-6, refer to the following reaction: CH4 (g) + H20 (g) e CO (g) + 3H2 (g) 4. Which is the response of the equilibrium system if the pressure is increased? A. Shift towards the right B. Shift towards the left. C. There is no change in the equilibrium D. There is not enough information. 5. If the Kc of the reaction is 0.26 at a given temperature and the following concentrations are present, [CH4] = 0.20, [H20] = 0.010, [CO] = 0.024, [H2] = 0.020, is the reaction at equilibrium? If not, in which direction will it proceed? A. Yes, the reaction mixture is ate equilibrium. B. No, it will proceed from right to left. C. No, it will proceed from left to right. D. Cannot be determined. 6. Given the standard Gibbs energy of the following specie at 298 K, A;G/ kJ mol-1 : CH4 (g)= -50.72, H20 (g) = -228.57, CO (g) = -137.17, H2(g) = 0, determine the K of the reaction. В. О.944 С. 8.14 х 1024 D. 1.06 Е. 1.61 А. 1.23 х 10-25
A container is initially filled with pure SO3. After a period of time, the following equilibrium is established: 2SO₂ (g) + O2 (g) →2SO3 (g) 25 Keq = 7.0 × 10 2 What does this equilibrium mixture contain? Select one: a. equal amounts of reactants and products b. 60% reactants and 40% products c. mostly products d. mostly reactants
Chapter 1 question 6: Ammonia has been studied as an alternative "clean" fuel for internal combustion engines, since its reaction with oxygen produces only nitrogen and water vapor, and in the liquid form it is easily transported. An industrial chemist studying this reaction fills a 50.0L tank with 4.6 mol of ammonia gas and 4.5 mol of oxygen gas, and when the mixture has come to equilibrium measures the amount of nitrogen gas to be 1.2 mol. Calculate the concentration equilibrium constant for the combustion of ammonia at the final temperature of the mixture. Round your answer to 2 significant digits.
QUESTION 4 Adding a catalyst to an equilibrium system will: produce more products at equilibrium. produce more reactants at equilibrium. not change the amount of reactants or products at equilibrium.