(Q74) A certain process is nonspontaneous at low temperatures. Given that AHrxn = 222.2 kJ and ASrxn = 868 J/K, at what temperature (in °C) will the process become spontaneous? (Report your Celsius temperature to one decimal place --> if your answer has a decimal place of "O" and Canvas chops it off, don't worry about it).

(Q74) A certain process is nonspontaneous at low temperatures. Given that AHrxn = 222.2 kJ and ASrxn = 868 J/K, at what temperature (in °C) will the process become spontaneous? (Report your Celsius temperature to one decimal place --> if your answer has a decimal place of "O" and Canvas chops it off, don't worry about it).

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...

See similar textbooks

Similar questions

One of the reactions that destroys ozone in the upper atmosphere is NO(g) + O3 (9) NO2 (g) + O2 (9) Substance and State AGf (kJ/mol) NO(g) 87 NO₂ (g) 52 0₂ (9) 0 03 (g) 163 a Calculate AGO AGO = Submit (at 298 K) for this reaction. KJ
Use the data below to determine the ΔHrxn for the following reaction: S=S(g) + H2(g) è H-S-S-H(g) (S=S: 425 kj/mol; S-S: 286 kj/mol, H-S: 363 kj/mol, H-H: 432 kj/mol )
What is the change in internal energy, ∆E, for a gas that absorbs 15 J of thermal energy and its volume increases from 1.00 L to 1.20 L against a constant 1.00 atm confining pressure. (Hint: 101.325 J is 1.00 L atm)
Given the data in the table below, H° rxn for the reaction
Arrange the following reactions in order of increasing ΔrxnS and briefly explain your reasoning.a) S(s) + O2(g) ⟶ SO2(g)b) H2(g) + O2(g) ⟶ H2O2(ℓ)c) CO(g) + 3 H2(g) ⟶ CH4(g) + H2O(ℓ)d) C(s) + H2O(g) ⟶ CO(g) + H2(g)
Green plants utilize sunlight to convert CO2 and H2O to glucose (C6H1206) and 02. Use the information in the table below to calculate AHo Substance A H;°(kJ/mol) S° (J/mol*K) CO2(g) -393.5 213.2 H20(1) -285.8 69.9 C6H1206(s) -1273.3 212.1 O2(g) 205.0 134 kJ 2802.5 kJ Cannot be determined – more information is needed. -594 kJ -256.5 kJ
STANDARD MOLAR ENTHALPHY OR FORMATION AND REACTION: Calculate the ∆H° of the following reaction. (Use 3 decimal places for the value of ∆H°f and express your answer as well in 3 decimal places.)
Use data from Appendix attached to calculate ΔS∘rxnΔ�rxn∘ for each of the reactions given. SO2(g)+12O2(g)→SO3(g)SO2(g)+12O2(g)→SO3(g) Express your answer using one decimal place in J/K.
7) Calculate the change in internal energy (AE) for a system that is giving off 25.0 kJ of heat and is changing from 12.00 L to 6.00 L in volume at 1.50 atm pressure. (Remember that 101.3 J = 1 L'atm) A) +25.9 kJ B) -16.0 kJ C) -25.9 kJ D) -24.1 kJ E) 937 kJ Answer: D Diff: 2 Page Ref: 6.4
Consider this reaction: C6H12O6 + 602 à 6CO2 + 6H₂O. What is the standard enthalpy AH°rxn given the standard molar enthalpies of the substances below? Substance C6H12O6 02 CO₂ H₂O AHᵒf (kJ/mol) -1274.4 0 -393.45 -241.8
1,2,3 please
Calculate the ΔGo for a reaction, given the ΔHo for the reaction = -5052.8 kJ and the ΔSo for the reaction = 97.8 J/K Express the answer to 1 decimal place.