Use standard free energy data from the table below to calculate the standard free energy change for the reaction below (at 298 K). CoCl2(g) Co(g) + Cl2(g) Your answer should include four significant figures. Substance AG kJ 'f mol kJ of mol AH₤ $298 mol K J CoCl2(g) -269.9 -312.5 109.2 Co(g) 0 0 30.10 Cl2(g) 0 0 223.0 Provide your answer below: kJ/mol

Use standard free energy data from the table below to calculate the standard free energy change for the reaction below (at 298 K). CoCl2(g) Co(g) + Cl2(g) Your answer should include four significant figures. Substance AG kJ 'f mol kJ of mol AH₤ $298 mol K J CoCl2(g) -269.9 -312.5 109.2 Co(g) 0 0 30.10 Cl2(g) 0 0 223.0 Provide your answer below: kJ/mol

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

Chapter17: Spontaneity, Entropy, And Free Energy

Section: Chapter Questions

Problem 1RQ: Define the following: a. spontaneous process b. entropy c. positional probability d. system e....

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For the reaction NO(g)+NO2(g)N2O3(g) , use tabulated thermodynamic data to calculate H and S. Then use those values to answer the following questions. (a) Is this reaction spontaneous at 25°C? Explain your answer. (b) If the reaction is not spontaneous at 25°C, will it become spontaneous at higher temperatures or lower temperatures? (c) To show that your prediction is accurate, choose a temperature that corresponds to your prediction in part (b) and calculate G . (Assume that both enthalpy and entropy are independent of temperature.)
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Enthalpy changes often help predict whether or not a process will be spontaneous. What type of reaction is more likely to be spontaneous: an exothermic or an endothermic one? Provide two examples that support your assertion and one counterexample.
Given the following information at 25C, calculate G at 25C for the reaction 2A(g)+B(g)3C(g) Substance Hf(kJ/mol) S(J/molK) A(g) 191 244 B(g) 70.8 300 C(g) 197 164 a 956 kJ b 956 kJ c 346 kJ d 346 kJ e 1.03 103 kJ
For the reaction at 298 K, 2NO2(g)N2O4(g) the values of H and S are 58.03 kJ and 176.6 J/K, respectively. What is the value of G at 298 K? Assuming that H and S do not depend on temperature, at what temperature is G = 0? Is G negative above or below this temperature?
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