Practice ProblemBUILD
In each of the following reactions, there is one species for which the standard entropy is not listed in Appendix 2. In each case, using the values that are in Appendix 2 and the that is given, determine the value of the missing standard entropy at 25
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- In freezing a mole of liquid water at the freezing point, the enthalpy of fusion is 6.01 KiloJoules per mole. Answer the questions that follow. (A). What is the entropy change of this process (in Joules per Kelvin)? (B). What is the entropy change of the surroundings for this process (in Joules per Kelvin)? Express answer in THREE SIGNIFICANT FIGURES. (C). What is the total entropy change (or the entropy change of the universe) for this process (in Joules per Kelvin)? Express answer in THREE SIGNIFICANT FIGURES.arrow_forwardWithout consulting the tables, what sign do you expect for the change in entropy (delta S) for the following reaction? P4 (g) + 10 Cl2 (g) → 4 PCl5 (g) Select one: a. can not be determined (too close to estimate) b. none of these c. negative d. positivearrow_forwardCalculate ΔGrxn at 308 K under the conditions shown below for the following reaction. Fe2O3(s) + 3 CO(g) → 2 Fe(s) + 3 CO2(g) ΔG° = -28.0 kJ P(CO) = 1.4 atm, P(CO2) = 2.1 atm Group of answer choices +30.0 kJ +31.1 kJ +24.9 kJ -24.9 kJ -31.1 kJarrow_forward
- H3. Consider a reaction for which the value of ΔG∘ = -9.199 kJ/mol at a 298.15 K. What is the value of Keq for this reaction at this temperature? Please give typed answerarrow_forwardFind ∆Stotal (entropy change) when 100 grams of water vapor initially at 200 degrees Celsius undergoes a cyclic process for which heat, qtotal = 1450 Joules. Given: 333.6 J/g and 2256.7 J/g as the heats of fusion and vaporization of water, respectively. Group of answer choices ΔS = 3.06 J/K ΔS = 70.51 J/K ΔS = 306.46 J/K ΔS = 476.95 J/K None of thesearrow_forwardSelect the circumstances under which a reaction would most likely be spontaneous. a. delta H is positive, delta S is positive, and the temperature is low. b. delta H is positive, delta S is negative, and the temperature is low. c. delta H is positive, delta S is negative, and the temperature is high. d. delta H is negative, delta S is negative, and the temperature is high. e. delta H is negative, delta S is positive, and the temperature is high.arrow_forward
- 4.) The normal boiling point of Br2 is 58.8°C, and its molar enthalpy of vaporization is Δ Hvap = + 29.6 kJ/ mol. (a) When Br2 (l) boils at its normal boiling point, does its entropy increase or decrease? (b) calculate the value of Δ S when 1.00 mol of Br2 (l) is vaporized at 58.8°C. Group of answer choices A.) (a) Entropy decreases (b) -503.4 J/K B.) (a) Entropy increases (b) 503.4 J/K C.) (a) Entropy decreases (b) - 89.2 J/K D.) (a) Entropy increases (b) 89.2 J/Karrow_forwardHi, Help with i-k part. The process of melting solid ice to produce water has the following thermodynamic values: Δ H = + 1.44 k c a l / m o l a n d Δ S = + 5.26 c a l / m o l ⋅ K. a) What is the value for Δ G at 263K in cal/mol?b) Is melting ice spontaneous at 263K?c) What about the reverse reaction? Would liquid water spontaneously freeze at 263K?d) Convert 263K to ∘ C. Would you expect ice to melt at this temperature?e) What is the value for Δ G at 283K in cal/mol?f) Is melting ice spontaneous at 283K?g) What about the reverse reaction? Would liquid water spontaneously freeze at 283K?h) Convert 283K to ∘ C. Would you expect ice to melt at this temperature?i) What is the value for Δ G at 273K in cal/mol? (Be careful to only use 3 Sig Figs in your calculations)j) Convert 273K to ∘ C. Would you expect ice to melt at this temperature?k) A Δ G of 0 indicates a system is at equilibrium. Use this to explain which process is spontaneous at 273K, melting or freezing?arrow_forwardFor a spontaneous chemical reaction which of the following are possible signs of ΔΔH and ΔΔS? Select one: a. both b and c b. ΔΔH = (+) and ΔΔS = (-) c. ΔΔH = (-) and ΔΔS = (+) d. neither b nor c Clear my choicearrow_forward
- SOLVE THE FOLLOWING PROBLEMS. Write down your answers CLEARLY. Thank you! Lesson Topic: THERMODYNAMICS (Spontaneous reactions and Gibbs free energy) 1. Use the given standard entropy values to calculate the standard entropy change to convert hydrogen chloride to chlorine in the given reaction: 4HCl ₍g₎ + O2₍g₎ → 2Cl₂₍g₎ + 2H₂O₍g₎ S°(J/K•mol): HCl ₍g₎ = 186.8 O2₍g₎ = 205 Cl2₍g₎ = 223 H2O₍g₎ = 188.7 2. Predict whether the following reaction leads to an increase or a decrease in entropy. Explain Why. Ag+₍aq₎ + Cl-₍aq₎ → AgCl₍s₎ 3. Calculate ∆G° for the combustion of ethane 2C₂H₆₍g₎ + 7O₂₍g₎ → 4CO₂₍g₎ + 6H₂O₍ₗ₎ With the following ∆G°f: C₂H₆(g = -32.86 kJ/mol CO₂(g) = -394.4 kJ/mol H₂O(l) = -237.2 kJ/mol O₂(g) = 0 4. From the following ∆H and ∆S values, predict whether the reaction would be spontaneous. If not, at what temperature…arrow_forwardDetermine ΔG°rxn for the following reaction at 298 K. FeO(s) + CO(g) → Fe(s) + CO2(g) ΔH°= -11.0 kJ; ΔS°= -17.4 J/K Group of answer choices -193.0 kJ -5.8 kJ +5.8 kJ +16.8 kJ -16.8 kJarrow_forwardFor a reaction with ΔH = 5.2767 kJ/mol and ΔS = 18 J/K•mol, at 20°C, the reaction is: Spontaneous Not Spontaneous At equilibrium. Please type answer note write by hend.arrow_forward
- Chemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning