Practice ProblemATTEMPT
Calculate the standard entropy change for the following reactions at
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- Find ∆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_forwardBe sure to answer all parts. Consider the combustion of butane gas: C4H10(g) + 13/2 O2(g) → 4CO2(g) + 5H2O(g) (a) Predict the signs of ΔS and ΔH (b) Calculate ΔG at 298 K.arrow_forwardSOLVE 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_forward
- 5). Calculate the standard entropy change for the following two reactions. Consult the last page of the exam for data and equations. a) 2 CO(g) + O2(g) à 2 CO2(g) b) 2 NaHCO3(s) à Na2CO3(s) + H2O(l) + CO2(g)arrow_forwardWhat is ΔH, ΔS and ΔG° at 1000 °C for the following reaction? CaCO3 (s) = CaO (s) + CO2 (g) ΔHf° (KJ) S° (J/K CaCO3 -1206.9 92.9 CaO -635.1 38.2 CO2 -393.5 213.7 ΔHAnswerKJ ΔSAnswerJ/K ΔGoAnswerKJ (b) Is the reaction spontaneous at 1000 °C and 1 atm? Answer (c) What is the value of Kp at 1000 °C for this reaction given that (R = 8.314 J/K mol) KpAnswer (d) What is the partial pressure of CO2 (g)?Answeratmarrow_forwardCalculate the entropy change for each of these processes. thereby verifying the predictions made in Conceptual Exercise 16.4. (a) 2 CO2(g) 2 CO(g) + O2(g) (b) NaCl(s) NaCl(aq) (c) MgCO3(s) MgO(s) + CO2(g)arrow_forward
- Predict the sign of S for each of the following and explain. a. the evaporation of alcohol b. the freezing of water c. compressing an ideal gas at constant temperature d. dissolving NaCl in waterarrow_forwardEstimate the sign of the entropy change for the reaction: CaCO3 (s) → CaO (s) + CO2 (g) Select one: a. is zero b. negative c. not possible to determine the sign d. none of these e. positivearrow_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_forward
- Calculate the temperature at which the following reaction becomes spontaneous. Compound ΔHof (kJmol)ΔHfo (kJmol) ΔSo (JK ⋅ mol)ΔSo (JK ⋅ mol) Cl2(g) 0.0 +223.1 ClNO2(g) +12.6 +272.2 NO(g) +91.3 +210.8 NO2(g) +33.2 +240.1 NOCl(g) +51.7 +261.7 PCl3(g) −287.2 +311.8 PCl5(g) −374.9 +364.6 PCl5(g) ↔ PCl3(g) + Cl2(g) (Answer with K unit )arrow_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_forwardOut atmosphere is composed primarily of nitrogen and oxygen, which coexist at 25°C without reacting to any significant extent. However, the two gases can react to form nitrogen monoxide according to the following reaction: N2(g) + O2(g) ⇌ 2NO(g) Calculate delta G° at 1940K. (Express answer using four significant figures.) Does the reaction become spontaneous with increasing temperature?arrow_forward
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