**Educational Assessment**1) **Which of the following statements is TRUE?** A) ΔS_universe is always greater than zero for a nonspontaneous process. B) Exothermic processes decrease the entropy of the surroundings. C) Entropy is not temperature dependent. D) Entropy is an extensive property. E) None of the above are true.2) **For a given reaction, ΔH = +35.5 kJ/mol and ΔS = +83.6 J/K·mol. The reaction is spontaneous ________. Assume that ΔH and ΔS do not vary with temperature.** A) at all temperatures B) at T < 425 K C) at T < 298 K D) at T > 425 K E) at T > 298 K3) **What element is being reduced in the following redox reaction?** \[ \text{H}_2\text{O}_2(l) + \text{ClO}_2(aq) \rightarrow \text{ClO}_2^-(aq) + \text{O}_2(g) \] A) C B) N C) O D) H E) Cl

The condition of spontaneity of a reaction is that overall change in Gibbs free energy should be…

1) Which of the following statements is TRUE? A) ASuniverse is always greater than zero for a nonspontaneous process. B) Exothermic processes decrease the entropy of the surroundings. C) Entropy is not temperature dependent. D) Entropy is an extensive property. E) None of the above are true. 2) For a given reaction, AH = +35.5 kJ/mol and AS = +83.6 J/Kmol. The reaction is spontaneous Assume that AH and AS do not vary with temperature. A) at all temperatures B) at T < 425 K C) at T < 298 K D) at T > 425 K E) at T > 298 K 3) What element is being reduced in the following redox reaction? H₂O2(1) + ClO2(aq) → ClO₂¯(aq) + O2(g) C) O A) C B) N D) H E) Cl

1) Which of the following statements is TRUE? A) ASuniverse is always greater than zero for a nonspontaneous process. B) Exothermic processes decrease the entropy of the surroundings. C) Entropy is not temperature dependent. D) Entropy is an extensive property. E) None of the above are true. 2) For a given reaction, AH = +35.5 kJ/mol and AS = +83.6 J/Kmol. The reaction is spontaneous Assume that AH and AS do not vary with temperature. A) at all temperatures B) at T < 425 K C) at T < 298 K D) at T > 425 K E) at T > 298 K 3) What element is being reduced in the following redox reaction? H₂O2(1) + ClO2(aq) → ClO₂¯(aq) + O2(g) C) O A) C B) N D) H E) Cl

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

For a particular reaction at 199.1 °C, AG = -159.63 kJ, and AS = 894.41 J/K. Calculate AG for this reaction at 13.8 °C. AG = kJ
Mg(s) + 2HCI(aq) MgCl, (aq) + H2 (g) + 1550kJ For this reaction at 25°C, Change in enthalpy: [ Select ] O because [ Select] • Change in entropy: [ Select ] O because [ Select ] · Change in Gibbs free energy: [ Select] thus • This reaction is [ Select ]
Consider the following reaction: 2 H,S(g) + 30,(g) –- 2 H,O(g) + 2 SO,(g) and the following table of standard enthalpies of formation and standard absolute entropies: compound AH (kJ mol") s° (JK' mol") H,S(g) -20.6 205.8 02(g) 205.2 H2O(g) |-241.8 188.8 So,(9) |-296.8 248.2
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?
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.
What is AS for the following reaction? 2Cl2(g) + SO2(g) SOCI₂(g) + Cl₂O(g) Substance: Cl₂(g) SO2(g) SOCI2(g) C1₂O(g) 223.0 248.1 309.8 266.1 S(J/K. mol):
38. For this process at 25 °C: H2O(g) H2O (A) AH is negative as energy is released. (B) AH is negative as energy is absorbed. (C) AH is positive as energy is released. (D) AH is positive as energy is absorbed.
What is entropy, and what is ΔS for a reaction, and what does it mean if ΔS is positive or negative?
Compare what will happen to the entropy of the whole system in the following two scenarios: A) if the oil molecules are all clumped together and the clump is surrounded by water and B) if the oil molecules are spread out evenly throughout the water, each individual oil molecule surrounded by water?
Consider the following reaction: Sr(OH)2(s) → Sr2+(aq) + 2 OH-(aq) ΔHorxn = -19.3 kJ/ mol Sorxn = -218.3 J/ K mol Which of the following statements is true? Group of answer choices: - the reaction is always non-spontaneous - The reaction is nonspontaneous at all temperatures - The reaction is spontaneous only at high temperature - The reaction is spontaneous only at low temperature - ΔG < 0 and the reaction is always spontaneous