Use the observations about each chemical reaction in the table below to decide the sign (positive or negative) of the reaction enthalpy AH and reaction entropy AS. Note: if you have not been given enough information to decide a sign, select the "unknown" option. reaction observations conclusions ΔΗ is (pick one) ♥ This reaction is endothermic and proceeds slower at temperatures below 130. °C. AS is (pick one) ♥ ΔΗ is This reaction is always spontaneous, but proceeds faster at temperatures above |(pick one) ♥ B 132. °С. AS is (pick one) v This reaction is spontaneous except below ΔΗ is (pick one) ♥ 16. °C but proceeds at a slower rate below 115. °C. AS is (pick one) ♥

Use the observations about each chemical reaction in the table below to decide the sign (positive or negative) of the reaction enthalpy AH and reaction entropy AS. Note: if you have not been given enough information to decide a sign, select the "unknown" option. reaction observations conclusions ΔΗ is (pick one) ♥ This reaction is endothermic and proceeds slower at temperatures below 130. °C. AS is (pick one) ♥ ΔΗ is This reaction is always spontaneous, but proceeds faster at temperatures above |(pick one) ♥ B 132. °С. AS is (pick one) v This reaction is spontaneous except below ΔΗ is (pick one) ♥ 16. °C but proceeds at a slower rate below 115. °C. AS is (pick one) ♥

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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You discover a new chemical reaction that has a standard entropy change equal to 167.1 J/mol•K and a standard enthalpy change of 60.20 kJ/mol at 296 K. Calculate the change in free energy (in kJ) for this reaction. Report your answer to the tenths place and do not include units. Include the correct sign in your answer
5. The above reaction was performed again, but this time in a constant-pressure calorimeter attached to a frictionless piston. Over the course of the process, the total volume of the gaseous contents of the calorimeter decreased by 100.4 mL. If the pressure outside of the piston was 1.000 atm, determine AHoa for this process in kJ. Recall that 101.325 J=1 L atm.
Given the following reaction: 9C (s) + 12H2 (g) + 3/2 O2 (g) → 3C3H7 OH (1) If the enthalpy change is -954 kJ and entropy increases: blank 1: is the reaction exothermic or endothermic? blank 2: is the reaction spontaneous or non-spontaneous?
The reaction 4AI (s) + 302 (g)→ 2 Al203 (s) AH° = -3351 kJ is and therefore heat is by the reaction. thermoneutral, neither released nor absorbed O endothermic, absorbed exothermic, released exothermic, absorbed endothermic, released
Hint: No calculations are required. For the reaction 2HBr(g) + Cl2(g)- >2HCI(g) + Br2(g) AH° = -81.1 kJ and AS° =-1.20 J/K At standard conditions, this reaction would be product favored O at all temperatures. O at relatively high temperatures. O at no temperature. O at relatively low temperatures.
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options for all: 1. Reactants. 2. Products.
Read the descriptions of physical or chemical changes in the table below. Then decide whether the change will be spontaneous, if you can. Change A gas condenses to a liquid, neither absorbing nor releasing heat. An exothermic chemical reaction between a solid and a liquid results in gaseous products. Two liquids mix, neither absorbing nor releasing heat. Is this change spontaneous? Yes. No. Can't decide with information given. ○ Yes. ○ No. Can't decide with information given. Yes. No. ○ Can't decide with information given.
Consider the reaction: 2 H,0(g) → 2H,(g) + 0,(g) If 2.0 moles of H2O(g) are converted to H2(g) and 02(g) against a pressure of 1.0 atm at 125 °C, what is the change in internal energy for this reaction? R-8.314 1/mol K AH- 483.6 kl/mol
1. A reaction with AH° = -64.0 kJ/ mole has K = 1.00 X 108 at 25.0 °C. What would be the value of K at 0.00 °C? 2. A reaction with AH° = 618.0 kJ/mole has K = 1.00 X 1060 at 25.0 °C. What would be the value of K at 500.0 °C?
Using H° data, calculate the standard enthalpy change for the reaction at 298K. 2 NH3(g) HNO3(aq) --> NO2(g) 2 H20(1) AH° (KJ/mol) -46.19 -206.6 33.84 -285.83 (Note: the table AH values are located directly below the corresponding compound, this is the number found in the Appendix)
Read the descriptions of physical or chemical changes in the table below. Then decide whether the change will be spontaneous, if you can. Change During an endothermic chemical reaction, four moles of gaseous reactants are turned into two moles of gaseous products. A solid precipitates from a solution, releasing heat as it does so. A solid absorbs heat and turns to a gas. Is this change spontaneous? Yes. O No. O Can't decide with information given. O Yes. O No. O Can't decide with information given. O Yes. O No. O Can't decide with information given.