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 A.S. Note: if you have not been given enough information to decide a sign, select the "unknown" option. reaction A B с observations This reaction is spontaneous only above 30. °C but proceeds at a slower rate below 199. °C. This reaction is spontaneous only below 19. °C. This reaction is exothermic and proceeds slower at temperatures below 60. °C. conclusions AH is AS is AH is AS is AH is AS is (pick one). (pick one) ✓ (pick one) ✓ (pick one) (pick one) (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 A.S. Note: if you have not been given enough information to decide a sign, select the "unknown" option. reaction A B с observations This reaction is spontaneous only above 30. °C but proceeds at a slower rate below 199. °C. This reaction is spontaneous only below 19. °C. This reaction is exothermic and proceeds slower at temperatures below 60. °C. conclusions AH is AS is AH is AS is AH is AS is (pick one). (pick one) ✓ (pick one) ✓ (pick one) (pick one) (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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Which statement is true of the internal energy of the system and its surroundings following a process in which ΔEsys = +65 kJ? Explain.a. The system and the surroundings both lose 65 kJ of energy.b. The system and the surroundings both gain 65 kJ of energy.c. The system loses 65 kJ of energy and the surroundings gain 65 kJ of energy.d. The system gains 65 kJ of energy and the surroundings lose 65 kJ of energy.
An important step in the synthesis of nitric acid is the conversion of ammonia to nitric oxide, NO. Calculate ΔH∞rxn for the reaction below using the following information; ΔH∞f [NH3(g)] = -45.9 kJ/mol; ΔH∞f [NO(g)] = 90.3 kJ/mol; ΔH∞f [H2O(g)] = -241.8 kJ/mol. 4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(g)
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) e This reaction is spontaneous only below A 99. °C. AS is (pick one) e ΔΗ is (pick one) e B The reaction is never spontaneous. AS is (pick one) e This reaction is spontaneous only above ΔΗ is (pick one) 8 141. °C but proceeds at a slower rate below 179. °C. AS is (pick one) 8
4NH3(g) + 3O2(g) → 2N2(g) + 6H2O(g) ΔrH = -1267 kJ mol-1 For the reaction above, select the correct sign for each of the following: ΔSsurr ΔSsys ΔSuniv Is the reaction spontaneous?
1.Consider the complete combustion of methane gas, CH4(g): Which of the following BEST describes the relationship between ΔH and ΔU? a.ΔH > ΔU b.ΔH = ΔU = 0 c.ΔH = ΔU d.ΔH < ΔU 2.Which of the following reactions would you expect to have the lowest ΔSo? a.CH4(g) + 2O2(g) → CO2(g) + 2H2O(g) b.C2H4(g) + 2O2(g) → 2CO2(g) + 2H2O(g) c.C2H2(g) + 5/2O2(g) → 2CO2(g) + H2O(g) d.C2H6(g) + 7/2O2(g) → 2CO2(g) + 3H2O(g) 3.Which species would you expect to have the lowest standard entropy (So)? a.Cl2(g) b.I2(s) c.F2(g) d.Br2(l)
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 A B C observations This reaction is always spontaneous, but proceeds faster at temperatures below 140. °C. The reaction is never spontaneous. This reaction is spontaneous only above 129. °C but proceeds at a slower rate below 192. °C. AH is AS is conclusions AH is AS is AH is AS is X ✓ (pick one) positive negative unknown (pick one) î (pick one) (pick one) C Ś ↑ (pick one) î
Consider the following reactions at 298 K. 2 03(g) → 3 O₂(g) O₂(g) → 2 0(g) NO(g) + O3(g) → NO₂(g) + O₂(g) ΔΗΘ Aat H ᎪᎻᎾ = -427.0 kJ/mol = 495.0 kJ/mol = -199.0 kJ/mol Apply Hess's law to calculate the standard reaction enthalpy for the reaction NO(g) + O(g) → NO₂(g)
D Try Again Your answer is incorrect. 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 A • reaction A: Your answer is incorrect. • reaction C: Your answer is incorrect. B с observations The reverse of this reaction is always spontaneous. This reaction is exothermic and proceeds slower at temperatures below -26. °C. This reaction is always spontaneous, but proceeds faster at temperatures above 139. °C. AH is AS is conclusions AH is As is AH is AS is X unknown negative ŷ negative ↑ unknown î unknown ↑ positive î S
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
Use the observations about each chemical reaction in the table below to decide the sign (positive or negative) of the reaction enthalpy ▴ and reaction entropy as. Note: if you have not been given enough information to decide a sign, select the "unknown" option. reaction A B C observations The reverse of this reaction is always spontaneous. This reaction is spontaneous except above 64. °C. This reaction is always spontaneous, but proceeds faster at temperatures below 77. °C. AH is AS is conclusions AH is AS is AH is AS is x (pick one) (pick one) (pick one) (pick one) (pick one) (pick one)
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