Practice ProblemATTEMPT
Calculate the standard entropy change for the following reactions at
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Chemistry
- Predict whether the standard entropy change for the following reactions at 25 °C will be positive, negative, or too close to call. (a) 2 CO2(g) → 2 CO(g) + O2 (g) (b) 3 O2(g) → 2 O3(g) (c) 2 NaHCO3(s) → Na2CO3(s) + H2O(l) + CO2(g)arrow_forwardCalculate ΔS°298 for the following changes.(a) SnCl4(l) ⟶ SnCl4(g)(b) CS2(g) ⟶ CS2(l)(c) Cu(s) ⟶ Cu(g)(d) H2 O(l) ⟶ H2 O(g)(e) 2H2(g) + O2(g) ⟶ 2H2 O(l)(f) 2HCl(g) + Pb(s) ⟶ PbCl2(s) + H2(g)(g) Zn(s) + CuSO4(s) ⟶ Cu(s) + ZnSO4(s)arrow_forwardConsider the reaction: KCIO4(s) →KCI(s) + 202(g) and the table of values given on the right. Do you expect this reaction to be spontaneous at room temperature? Why? (A) Yes, because AGrxn is negative. (B) Yes, because Hrxn is negative. (C) Yes, because AHrxn is positive. (D) No, because AGrxn is positive. (E) No, because Hrxn is positive. Substance AG fº (kJ/mol) KCIO4(s) -300.4 KCI(s) -408.2 02(8) 0 ΔΗ,° (kJ/mol) -433 -437 0arrow_forward
- Using the standard molar entropies in Appendix C, calculatethe standard entropy change, ΔS°, for the “water-splitting”reaction at 298 K:2 H2O(l)---->2 H2(g) + O2(g) (a) 326.3 J/K (b) 265.7 J/K (c) 163.2 J/K (d) 88.5 J/K(e) -326.3 J/Karrow_forwardQUESTION 22 At what temperature, in Kelvin, does the following reaction change from spontaneous to non-spontaneous 2 A (aq) + 2 B (aq) 2 C (aq) + 1 D (aq) if AH° (A)= 0.8219 kJ/mol, AH° (B) = -40.5308 kJ/mol, AH° (C) = -85.3178 kJ/mol, and AH (D) = -70 8643 kJ/mol AS (A)= 76.117 J/(mol K), AS (B) = -15.8072 J/(mol K), AS (C) = 18.4425 J/(mol K), and AS" (D) = -8.6387 J/(mol K)arrow_forwardFor which reaction will ΔS be positive? Group of answer choices N2O4(g) ⟶ 2 NO2(g) 2 H2(g) + O2(g) ⟶2 H2O(g) 3 NO(g) ⟶NO2(g) + N2O(g) 2 SO2(g) + O2(g) ⟶2 SO3(g)arrow_forward
- 10:59 1 Question 13 of 20 Submit Which of the following sets of conditions is true for an exothermic reaction that is spontaneous at all temperatures? A) AH 0, AS 0 D) AH > 0, AS 0, ΔG <0arrow_forwardWithout doing any calculations, predict the sign of ΔH foreach of the following reactions:(a) NaCl(s)---->Na+ (g) + Cl-(g)(b) 2 H(g)---->H2(g)(c) Na(g)---->Na+ (g) + e-(d) I2(s)---->I2(l)arrow_forwardPredict the sign of the entropy change for the following processes. Indicate the reason for each of your predictions.(a) One mole liquid water at room temperature ⟶ one mole liquid water at 50 °C(b) Ag+(aq) + Cl−(aq) ⟶ AgCl(s)(c) C6 H6(l) + (15)/(2) O2(g) ⟶ 6CO2(g) + 3H2 O(l)(d) NH3(s) ⟶ NH3(l)arrow_forward
- In which process is ΔH > 0 at constant pressure? CH3OH(g) à CH3OH(l) H3O+(aq) à H2O(l) + H+(aq) 2 NO2(g) à N2O4(g)arrow_forward(a) Calculate ASuniy for the reaction H,02(1) – H,O,(g) at 175.0°C. Enter your answer in the box provided. J/K mol (b) Is the reaction spontaneous, nonspontaneous, or an equilibrium process? Select the best single answer. spontaneous nonspontaneous an equilibrium processarrow_forwardAssume that the following reaction occurs at constantpressure:2 Al(s) + 3 Cl2(g)------> 2 AlCl3(s)(a) If you are given ΔH for the reaction, what additionalinformation do you need to determine ΔE for the process?(b) Which quantity is larger for this reaction? (c) Explainyour answer to part (b).arrow_forward
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