2Al(s) + 3C12(g) -> 2AICI3(s) The above reaction is not spontaneous under standard conditions, but becomes spontaneous as the temperature decreases. Which choice below is true at standard conditions? Ο Α. ΔΗ +, ΔS+ Ο Β. ΔΗ -, ΔS+ O C. AH +, AS O D. AH -, AS -

2Al(s) + 3C12(g) -> 2AICI3(s) The above reaction is not spontaneous under standard conditions, but becomes spontaneous as the temperature decreases. Which choice below is true at standard conditions? Ο Α. ΔΗ +, ΔS+ Ο Β. ΔΗ -, ΔS+ O C. AH +, AS O D. AH -, AS -

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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#5 Q9
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a. Which of the following is TRUE if ΔEsys = -341 J? The system is losing 341 J, while the surroundings are gaining 341 J. Both the system and the surroundings are losing 341 J. The system is gaining 341 J, while the surroundings are losing 341 J. Both the system and the surroundings are gaining 341 J. b. Which of the following is TRUE if ΔEsys = 411 J? The system is gaining 411 J, while the surroundings are losing 411 J. Both the system and the surroundings are losing 411 J. The system is losing 411 J, while the surroundings are gaining 411 J. Both the system and the surroundings are gaining 411 J. None of the above is true.
The table below shows the values of the standard enthalpies of formation of the substances involved in the reaction shown below. With these data, the value of the enthalpy of the reaction ∆°RX for this reaction will be: Select one:a. -744.9b. -4519c. -130.4d. -4219
For a particular reaction, AH° = 67.7 kJ and AS° = 126.9 J/K. Assuming these values change very little with temperature, at what temperature does the reaction change from nonspontaneous to spontaneous? T = K Is the reaction in the forward direction spontaneous at temperatures greater than or less than the calculated temperature? less than greater than
2H2O(g) ----> 2H2(g) + O2(g) The reaction above is only spontaneous at temperatures above 2000K. Is the reaction endothermic (+ΔH) or exothermic (-ΔH)?
In a biochemical reaction, A + B ® C with DG= 30 kJ/mol. Which of the following reactions, if any, might be effectively coupled to this reaction so that it becomes more spontaneous? I. C + D -> B + E Delta G = –40 kJ/mol II. C + D -> B + E Delta G = +40 kJ/mol
The following reaction is endothermic. 2NH3(g) → N2(g) + 3H2(g) This means the reaction A. will be spontaneous at high temperatures. B. will be spontaneous at low temperatures. C. is not spontaneous at any temperature. D. is spontaneous at all temperatures.
49.For the decomposition of hydrogen peroxide to water and oxygen, H2O2(g) ⟶⟶ H2O(g) + O2(g) ΔΔH° = -106 kJ, and ΔΔS° = +0.0580 kJ/K. In what temperature range is the reaction spontaneous (ΔΔG° < 0)? A. The temperature must be greater than 1.83××103 K B. The temperature must be less than 1.83 ××103 K. C. The temperature must be between 225 K and 1.83 ××103 K. D. ΔΔG° is always less than zero. E. ΔΔG° is never less than zero.
If the process is exothermic and not spontaneous, then what must be TRUE? O a. AS0 O c. AH=0 O d. AS> 0
For each reaction, calculate ΔH°rxn, ΔS°rxn, and ΔG°rxn at 25 °C and state whether or not the reaction is spontaneous. If the reaction is not spontaneous, would a change in temperature make it spontaneous? If so, should the temperature be raised or lowered from 25 °C?a. 2 CH4( g)------->C2H6( g) + H2( g)b. 2 NH3( g)------> N2H4( g) + H2( g)c. N2( g) + O2( g)-------->2 NO( g)d. 2 KClO3(s)-------->2 KCl(s) + 3 O2( g)
At what temperatures will a reaction be spontaneous if AH = +158 kJ and AS = +411 %3D J/K? O The reaction will never be spontaneous. O The reaction will be spontaneous at any temperature. O All temperatures above 384 K O All temperatures below 384 K