A process at constant T and P can be described as spontaneous if ΔG < 0 and nonspontaneous if ΔG > 0. Over what range of temperatures is the following process spontaneous? Assume that gases are at a pressure of 1 atm. (Hint: Use the data below to calculate ΔH and ΔS [assumed independent of temperature and equal to ΔH° and ΔS°, respectively] and then use the definition of ΔG.) PCl3(g) + Cl2(g) → PCl5(g) ΔHf° (kJ mol-1) -287.0 -374.9 S° (J K-1 mol-1) 311.7 223.0 364.5 ΔH° = kJ ΔS° = J K-1 The calculated value of T at which ΔG° = 0 is K. Reaction is spontaneous . Submit Answer
A process at constant T and P can be described as spontaneous if ΔG < 0...
A process at constant T and P can be described as spontaneous if ΔG < 0 and nonspontaneous if ΔG > 0. Over what range of temperatures is the following process spontaneous? Assume that gases are at a pressure of 1 atm. (Hint: Use the data below to calculate ΔH and ΔS [assumed independent of temperature and equal to ΔH° and ΔS°, respectively] and then use the definition of ΔG.) 3 PbO2(s) → Pb3O4(s) + O2(g) ΔHf° (kJ mol-1) -277.0...
A process at constant T and P can be described as spontaneous if AG <0 and nonspontaneous if AG> 0. Over what range of temperatures is the following process spontaneous? Assume that gases are at a pressure of 1 atm. (Hint: Use the data below to calculate AH and AS [assumed independent of temperature and equal to AH° and AS°, respectively] and then use the definition of AG.) 2 MnO2(s) 02(g) 2 MnO(s) AH (kJ mol) -520.0 -385.2 s° (J...
A reaction has an equilibrium constant of Kp=0.061 at 27 ∘C. Part A Find ΔG∘rxn for the reaction at this temperature. Find for the reaction at this temperature. 6.98 kJ 0.839 kJ -6.98 kJ 0.628 kJ Part B Above what temperature does the following reaction become nonspontaneous? 2 H2S(g) + 3 O2(g) → 2 SO2(g) + 2 H2O(g) ΔH = -1036 kJ; ΔS = -153.2 J/K 298 K 158.7 K 6.762 × 103 K This reaction is nonspontaneous at all...
A) A reaction has an equilibrium constant of Kp=0.280 at 44 ∘C. Find ΔG∘rxn for the reaction at this temperature. Find for the reaction at this temperature. 3.35 kJ -3.35 kJ 0.404 kJ 0.466 kJ B) Above what temperature does the following reaction become nonspontaneous? FeO(s) + CO(g) → CO2(g) + Fe(s) ΔH= -11.0 kJ; ΔS = -17.4 J/K Above what temperature does the following reaction become nonspontaneous? FeO(s) + CO(g) → CO2(g) + Fe(s) = -11.0 kJ; = -17.4...
1a. ) Complete the table with signs and general values for K (ie: K<1 or K>1) Always spontaneous Always nonspontaneous Spontaneous at high temperatures ΔG ΔH ΔS K 2. Calculate the boiling point (in K) for the following: X2 (l) --) X2 (g) ΔH = +35 kJ ΔS = + 215 J/K (HINT: what does ΔG equal when a reaction switches from spontaneous to nonspontaneous?) 1b. ) Trick question (refer to the table in #1): at what temperature does the...
Consider the following reaction: CaCO3(s)→CaO(s)+CO2(g). Estimate ΔG∘ for this reaction at each of the following temperatures. (Assume that ΔH∘ and ΔS∘ do not change too much within the given temperature range.) Part A 315 K ΔG∘ Δ G ∘ = nothing kJ Part B 1085 K ΔG∘ Δ G ∘ = nothing kJ Part C 1465 K ΔG∘ Δ G ∘ = nothing kJ Part D Predict whether or not the reaction in part A will be spontaneous at 315...
Given the values of ΔH∘rxn , ΔS∘rxn , and T below, determine ΔSuniv . 1. ΔH∘rxn= 83 kJ , ΔSrxn= 152 J/K , T= 308K (spontaneous or nonspontaneous ) 2. ΔH∘rxn= 83 kJ , ΔSrxn= 152 J/K , T= 752 K (spontaneous or nonspontaneous ) 3. ΔH∘rxn= 83 kJ , ΔSrxn=− 152 J/K , T= 308 K (spontaneous or nonspontaneous ) 4. ΔH∘rxn=− 83 kJ , ΔSrxn= 152 J/K , T= 397 K (spontaneous or nonspontaneous )
Given the values of ΔH∘rxn, ΔS∘rxn, and T below, determine ΔSuniv and whether they are spontaneous or nonspontaneous: A. ΔH∘rxn= 80 kJ , ΔSrxn= 143 J/K , T= 290 K B. ΔH∘rxn= 80 kJ , ΔSrxn= 143 J/K , T= 764 K C. ΔH∘rxn= 80 kJ , ΔSrxn=− 143 J/K , T= 290 K D. ΔH∘rxn=− 80 kJ , ΔSrxn= 143 J/K , T= 396 K
Exercise 17.62 Consider the following reaction: CaCO3(s)→CaO(s)+CO2(g). Estimate ΔG∘ for this reaction at each of the following temperatures. (Assume that ΔH∘ and ΔS∘ do not change too much within the given temperature range.) Part A 285 K ΔG∘ = 134 kJ SubmitMy AnswersGive Up Correct Part B 1095 K ΔG∘ = kJ SubmitMy AnswersGive Up Part C 1475 K ΔG∘ = −50.9 kJ SubmitMy AnswersGive Up Incorrect; Try Again; 5 attempts remaining Part D Predict whether or not the reaction...
Use the table below to answer the question that follow. Thermodynamic Quantites for Selected Substances at 298.15 K (25°C) Substance ΔH°f (kJ/mol) ΔG°f (kJ/mol) S (J/K⋅mol) Calcium Ca (s) 0 0 41.4 CaCl2 (s) -795.8 -748.1 104.6 Ca2+ (aq) 226.7 209.2 200.8 Clorine Cl2 (g) 0 0 222.96 Cl- -167.2 -131.2 56.5 Oxygen O2 (g) 0 0 205.0 H2O (l) -285.83 -237.13 69.91 Phosphorus P2 144.3 103.7 218.1 PCl3 (g) -288.1 -269.6 311.7 POCl3 (g) -542.2 -502.5 325 Sulfur S...