Analyze the table below.According to the table, if a process is spontaneous and has a positive AS, whatmust be true of its enthalpy change, AH?Enthalpy ChangeEntropy ChangeExothermic (-AH)Increase (+AS)Exothermic (-AH)Decrease (-AS)Endothermic (+AH)Increase (+AS)Endothermic (+AH) Decrease (-AS)ABсAH must be positive.AH must be negative.Spontaneous Reaction?Yes, -AG at any temperatureOnly at low temps, if |T AS| < |AH|Only at high temps, if IT AS| > |AH|No, +AG at any temperatureThere is no way to know the enthalpy change.D The enthalpy change depends on temperature.

Gibbs free energy change(∆G), entropy change(∆S), and enthalpy change(∆H) are related through the…

According to the table, if a process is spontaneous and has a positive AS, what must be true of its enthalpy change, AH? Enthalpy Change Entropy Change Exothermic (-AH) Increase (+AS) Exothermic (-AH) Decrease (-AS) Increase Increase (+AS) (+AS) Decrease (-AS) Endothermic (+AH) Endothermic (+AH) A B AH must be positive. AH must be negative. Spontaneous Reaction? Yes, -AG at any temperature Only at low temps, if |T AS| < |AH| Only at high temps, if IT AS| > |AH| No, +AG at any temperature

According to the table, if a process is spontaneous and has a positive AS, what must be true of its enthalpy change, AH? Enthalpy Change Entropy Change Exothermic (-AH) Increase (+AS) Exothermic (-AH) Decrease (-AS) Increase Increase (+AS) (+AS) Decrease (-AS) Endothermic (+AH) Endothermic (+AH) A B AH must be positive. AH must be negative. Spontaneous Reaction? Yes, -AG at any temperature Only at low temps, if |T AS| < |AH| Only at high temps, if IT AS| > |AH| No, +AG at any temperature

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

Consider these reactions: Reaction 1: H2(g) + Cl2(g) 2HCI(g) AH = -184.6 kJ Reaction 2: 20F2(g)- O2(g) + 2 F2(g) AH = -49.4 kJ Reaction 3: N2(g) + 202(g) 2NO2(g) AH = +66.4 kJ Reaction 2 can be described as an [Select] [ Select ] reaction
5.54
(Q5) Consider an endothermic reaction that takes place in 553 mL of solution. If the reaction requires 4,380 J of energy and the initial temperature of the solution is 26.2, what will the final solution temperature be? (3 sf) The density of solution is 1.00 g/mL and the specific heat of the solution is the same as that of water.
A chemist measures the energy change AH during the following reaction: C;Hg(9)+50,(g) → 3 CO2(9)+4H,0(1) AH=-2220. kJ Use the information to answer the following questions. endothermic. This reaction is... x10 exothermic. Suppose 10.9 g of C,Hg react. Yes, absorbed. Yes, released. Will any heat be released or absorbed? No. If you said heat will be released or absorbed in the second part of this question, calculate how much heat will be released or absorbed. Round your answer to 3 significant digits.
4) A 154.11 gtsample of concrete, with a specific heat capacity of 0.88 J/(g*•C), initially has a temperature of 22.4 °C. If 841.50 J of energy is released from the sample: a) Determine the change in temperature, in oC (do not round). [A3] b) Determine the anticipated final temperature, in C (round to 2 decimal places). [A2]
Calculate AHO,xn for each of the following using data from Appendix B. (a) 2 H2S(g) + 3 02(g) → 2 SO2(g) + 2 H20(g) kJ (b) SiO2(s) + 4 HF(g) → SİF4(g) + 2 H20(/) kJ
What is the heat of formation of FeO, based on the data
Use the following information to answer the question: What is the ΔH (in kJ/mol) for the following reaction? (Show work) CS2(l) + 3 O2(g) → CO2(g) + 2 SO2(g) Given: C(s) + O2(g) → CO2(g); ΔHf = -393.5 kJ/mol S(s) + O2(g) → SO2(g); ΔHf = -296.8 kJ/mol C(s) + 2 S(s) → CS2(l); ΔHf = 87.9 kJ/mol