Problem 1If a reaction is either at equilibrium or spontaneously proceeds forwardtowards equilibrium, then the following is always true (check all applicable boxes, checking an incorrectbox brings negative points and cancels a correct answer):AS< 0univ= 0AS univAS,> 0AS n 2 AS,ASrxn< AS.surrunivrxnsurrAGn <0AG = 0AG, > 0AG,> 0rxnrxnrxnrxnProblem 2Check below Check below>0if AS xn< 0if ASrxnPredict the sign of ASxnby checking a box of yourchoice on the right of eachreaction.incorrect box brings negative 2Na(s) + 2H,O(1)points.2KCIO (s) → 2KCIO,(s) + O2(g)S(s) + O2(9)→ SO2(9)Checkingan→ 2NAOH(aq) + H,(g)

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Problem 1 If a reaction is either at equilibrium or spontaneously proceeds forward towards equilibrium, then the following is always true (check all applicable boxes, checking an incorrect box brings negative points and cancels a correct answer): AS, < 0 'univ AS = 0 univ AS. 'univ > 0 AS. rxn 2 AS ASvn < AS, surr rxn surr AG° rxn AG = 0 AG xn > 0 AG >0 rxn rxn

Problem 1 If a reaction is either at equilibrium or spontaneously proceeds forward towards equilibrium, then the following is always true (check all applicable boxes, checking an incorrect box brings negative points and cancels a correct answer): AS, < 0 'univ AS = 0 univ AS. 'univ > 0 AS. rxn 2 AS ASvn < AS, surr rxn surr AG° rxn AG = 0 AG xn > 0 AG >0 rxn rxn

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

Chapter13: Chemical Equilibrium

Section: Chapter Questions

Problem 8ALQ: Le Chteliers principle is stated (Section 12-7) as follows: If a change is imposed on a system at...

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Le Chteliers principle is stated (Section 12-7) as follows: If a change is imposed on a system at equilibrium, the position of the equilibrium will shift in a direction that tends to reduce that change. The systemN2(g)+3H2(g)2NH3(g) is used as an example in which the addition of nitrogen gas at equilibrium results in a decrease in H2 concentration and an increase in NH3, concentration. In the experiment the volume is assumed to be constant. On the other hand, if N2 is added to the reaction system in a container with a piston so that the pressure can be held constant, the amount o f NH3 actually could decrease, and the concentration of H2 would increase as equilibrium is reestablished. Explain how this can happen. Also, if you consider this same system at equilibrium, the addition of an inert gas. holding the pressure constant, does affect the equilibrium position. Explain why the addition of an inert gas to this system in a rigid container does not affect the equilibrium position.
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7-41 The equilibrium constant at 1127°C for the following endothermic reaction is 571: If the mixture is at equilibrium, what happens to K if we: (a) Add some H2S? (b) Add some H2? (c) Lower the temperature to 1000°C?
Consider the decomposition equilibrium for dinitrogen pentoxide: 2N2O5(g)4NO2(g)+O2(g) At a certain temperature and a total pressure of 1.00 atm, the N2O5 is 0.50% decomposed (by moles) at equilibrium. a. If the volume is increased by a factor of 10.0. will the mole percent of N2O5 decomposed at equilibrium be greater than, less than. or equal to 0.50%? Explain your answer. b. Calculate the mole percent of N2O5 that will be decomposed at equilibrium if the volume is increased by a factor of 10.0.
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Fou m Costants 12 C he llown Sreactions and correponding equilibenum constants Reaction A K-1) Reaction B(A-9.2- 1021 Reaction C( Reaction D (-5.6- 1015) Reaction E (K Al equilibrium which reaction has the highest product. concentration 14-10) -6.3- 102) 2800000
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You Counselting Wellbeing &Health COVID-19 [N,O] (H,O] 1 O e. Ke = Question 18 Consider the following equilibrium reaction: Answer saved H2CO3 (aq) = H (aq) + HCO3 (aq); K = 5.0 x 10-7 Marked out of If the initial concentrations of the species are: 1 [H,CO3] = 0.020 M; [H*] = 6.00 x 10-5 M; [HCO] = 4.00 x 10-5 M P Flag question Which one of the statements below describes the relationship between Q and K and then the correct direction of chemical change? Select one: O a. Q> K, so the reaction moves to the right. O b. Q = K, so the reaction is at equilibrium. O C Q>K so the reaction moves to the left. O d. Q< K. so the reaction moves to the left. O e. Q< K, so the reaction moves to the right. Clear my choice 19 * A ENG 18°C Mostly cloudy
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