s engine.html?ClassID=1653724337#Calculate the standard entropy change for thecombustion of propane, a common fuel.C3H3 (g) + 502(g) → 3CO2(g) + 4H2O(1)SubstanceS° (J/mol-K)C;H3(g)0,(g)Co,(g)H,O(1)27020521470AS° = [ ? ] J/mol KEnter either a + or - sign AND the magnitude inyour answer.Enter

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Calculate the standard entropy change for the combustion of propane, a common fuel. C3H8(g) + 502(g) → 3CO2(g) + 4H2O(1) -> Substance S° (J/mol-K) C3H3(g) 270 205 Co,(g) H,O(1) 214 70 AS° = [ ? ] J/mol K %3D Enter either a + or - sign AND the magnitude in your answer. Enter

Calculate the standard entropy change for the combustion of propane, a common fuel. C3H8(g) + 502(g) → 3CO2(g) + 4H2O(1) -> Substance S° (J/mol-K) C3H3(g) 270 205 Co,(g) H,O(1) 214 70 AS° = [ ? ] J/mol K %3D Enter either a + or - sign AND the magnitude in your answer. Enter

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...

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Consider the following reaction: 2 H2(g) + 2 NO(g) N2(g) + 2 H20(g) and the following table of standard enthalpies of formation and standard absolute entropies: compound AH (kJ mol-1) s° (J K-1 mol-1) H2(g) 130.8 NO(g) 91.3 210.8 N2(g) 191.6 H20(g) -241.8 188.8
2 NH3 (g) + 2 O2 (g) → N20 (g) + 3 H2O (g) Is this reaction spontaneous only at low temperatures, only at high temperatures, at all temperatures? AH°r, kJ/mol s°, J/mol·K NH3(g) -46.1 192.5 0:(g) 205.0 N 20 (g) 82.1 219.9 H2O(g) |-241.8 188.7 AH°i, kJ/mol s°, J/mol·K What is the lowest temperature at which the following reaction is spontaneous? H2O (g) + C (s) → H2 (g) + CO (g) Co(g) H2(g) C (s) -110.5 | 197.7 130.6 5.7 H2O(g) |-241.8 188.7
Consider the reaction 2NaOH(aq) + H2(g)—2Na(s) + 2H2O(l) for which AH° = 368.6 kJ and AS° = 15.30 J/K at 298.15 K. (1) Calculate the entropy change of the UNIVERSE when 1.759 moles of NaOH(aq) react under standard conditions at 298.15 K. ASuniverse= J/K (2) Is this reaction reactant or product favored under standard conditions? (3) If the reaction is product favored, is it enthalpy favored, entropy favored, or favored by both enthalpy and entropy? If the reaction is reactant favored, choose 'reactant favored'. Submit Answer
For the following reaction (the detonation of nitroglycerin), is it spontaneous under standard conditions and how can you tell? 4 C4H5N3O9(l) (arrow >) 12 CO2(g) + 10 H2O(g) + 6 N2(g) + O2(g) ΔH = -5678 kJ
Consider the reaction 6CO2(g) + 6H20((1) C,H12O6 + 602(g) for which AH° = 2.801×10° kJ and AS° = -259.0 J/K at 298.15 K. (1) Calculate the entropy change of the UNIVERSE when 1.722 moles of CO2(g) react under standard conditions at 298.15 K. ASuniverse J/K (2) Is this reaction reactant or product favored under standard conditions? (3) If the reaction is product favored, is it enthalpy favored, entropy favored, or favored by both enthalpy and entropy? If the reaction is reactant favored, choose 'reactant favored'.
The decomposition of copper (1) oxide to its elements does not occur spontaneously at 375°C (AG = 140.0 kJ): Cu₂0 (s) 2 Cu (s) + 1/2O₂(g). It can be made to occur spontaneously by being coupled to the oxidation of solid carbon to form carbon monoxide gas at this same temperature (AG = -143.8 kJ): C(s) + 1/2O₂(g) → CO (g) What product(s) is/are produced as a result of coupling the two reactions? CO (g) 2 Cu (s) and 1/2 O₂ (g) 2 Cu (s) and CO (g) 2 Cu (s), 1/2 O2 (g), and CO (g) 1/2 0₂ (g)
Under normal room conditions (standard pressure at about 20°C), vwater will not boil, so we do not observe H20(1) + 40.7 kJ → H20(g) . At this temperature, the process is [ Select ] O because [ Select ]
A mole of sodium met is added to water How much work is done on the atmosphere by the subsequent reaction if the temperature is 25 C°
"M" represents a metallic element. "X" represents a nonmetallic element. Calculate ΔH for the process M3X4(s) ⟶ 3M(s) + 2X2(g) from the following information: M(s) + ½X2(g) ⟶ MX(s) ΔH°= -286.2 kJ 3MX(s) + ½X2(g) ⟶ M3X4(s) ΔH°= -84.3 kJ
Using the values in the table below, calculate AGxn at 375 K for the reaction: 3 CO g) + 4 NH3(g) → 3 CH3OH(g) + 2 N2(g) AH°F, kJ/mol AG°, kJ/mol S°, J/mol K COg) CH3OH(g) CH3OH NH3(aq) NH3(g) N2(9) -111 -137 198 -201 -162 238 -239 -166 127 -80 -27 111 -46 -17 193 192 +55 +15 -7 +100,414 +150
O-234 kJ 234 kJ -150. kJ -117 kJ Given: -1835kJ AH°, AHᵒf (kJ/mol) -941 -840 QUESTION 12 Use the standard reaction enthalpies given below to determine AH°rxn for the following reaction: P4(g) + 10 Cl₂(g) → 4 PC|5(s) PC15(s) → PC13(g) + Cl₂(g) P4(g) + 6 Cl₂(g) → 4 PCl3(g) rxn IF7(g) IF 5(9) 2(g) 62.42 = ? ΔΗ° rxn AH°rxn = +157 kJ = -1207 KJ QUESTION 13 Use the AH°f and AH°rxn information provided to calculate AH°f for IF: IF7(9) + 12(g) → IF5(g) + 2 IF(g) AH°rxn = -89 kJ
For the reaction C(s,graphite) + 02(g) CO2(g) AG° = -394.3 kJ and AS° = 2.9 J/K at 290 K and 1 atm. This reaction is (reactant, product) favored under standard conditions at 290 K. The standard enthalpy change for the reaction of 2.38 moles of C(s,graphite) at this temperature would be kJ.