Calculate the standard entropy of formation of liquid ethanol at 25°C. [S°(Cgraphite) = 160.70J/K•mol, S°(02) = 205.14 J/K•mol, S°(H2) = 130.68 J/K•mol, S°(C2H5OH) = 130.68 J/K•mol] 1. %3!
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![Assessment 2.2
Calculate the standard entropy of formation of
liquid ethanol at 25°C. [S°(Cgraphite) = 160.70J/K•mol,
S°(02) = 205.14 J/K•mol, S°(H2) = 130.68 J/K•mol,
S°(C2H5OH) = 130.68 J/K•mol]
1.
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- At constant pressure and 25°C, what is ΔH° for the following reaction2C2H6(g) + 7O2(g) → 4CO2(g) + H2O(l)if the complete consumption of 38.2 g of C2H6 liberates 1981 kJ of heat energy?a. 3120 kJb. 1560 kJc. 5030 kJd. 2510 kJe. 784.05 kJCalculate the change in entropy in (J/K) when 340g of methanol (32 g/mol) is heated from 40 ⁰C to 50 ⁰C at constant pressure. Specific heat capacity of methanol at constant pressure is 81 J/mol-K. Answer Format: [2 decimals]The combustion of ethanol used as a fuel has the ff reaction: C2H5OH(g) + O2 (g) -> CO2(g) +H2O with heating values of HHV=-2960 kJ/kg and LHV =-20760 kJ/kg. What is the vaporization of H2O in kj/kg a. 2260 b. 6780 c. 2970 d.8910
- The standard heat of formation for AgCN(s) is 146 kJ/mol at 298 K. Write the formation equation for AgCN(s) that goes with this value of ΔH°.Enter carbon as C(s). Be sure to specify states. Write fractions with a slash, such as 1/2 for one half.The value of AH° for the reaction below is -6535 kJ. ob kJ of heat are released in the combustion of 16.0 g of C6H6 (1)? MM C6H6 = 78.12 g/mol 2C6H6 (1) + 1502 (g) → 12CO2 (g) + 6H₂O (1) 1 A) 669 SHAHB)-6535 C) 1.34 x 103 D) 5.23 x 104 E) 2.68 x 103 Only typed solution.The vaporisation of a certain element at 24.0 oC has the following enthalpy and entropy values: Hvap = 3.40 kJ mol-1 and Svap = 246 J K-1 mol-1. What is the total entropy change (Stot) for the vaporisation of this element, in J K-1mol-1? (Enter your answer as a number only, with the correct number of significant figures!)
- Automobiles and trucks pollute the air with NO. At 2000.0°C, Kc for the reactionN2(g)+O2(g)2NO(g)At 2000.0°C Kc = 4.100 × 10–4 and ΔH° = 180.6 kJ. What is the value of Kc at 41.00°C?Given the following reaction: 4 Fe(s) + 3 O2 (g) → 2 Fe2O3 (s) ΔH = -1648 kJ 52.0 g of Fe (MM = 55.845 g/mol) are reacted as above in 1.000 x 103 g of water (MM = 18.02, ΔHFUSION = 6.01 kJ/mol, ΔHVAP = 40.65 kJ/mol, specific heat = 4.18 J/(g C) that is at 20.0 °C. What will the final temperature of the water be? Select one: 100 367 91.8 112 20.1Calculate the value of ΔGo in kJ for the combustion of 1 mole of methane to form carbon dioxide and gaseous water at 298 K.(value ± 2) So given below in J/mol K S° (CH4(g)) = 186. S° (O2(g)) = 209. S° (CO2(g)) = 217. S° (H2O(g)) = 188. ΔHfo given in kJ/mol ΔHfo (CH4(g)) = -74. ΔHfo (CO2(g)) = -399. ΔHfo (H2O(g)) = -231.
- Given the following reaction:4 Fe(s) + 3 O2 (g) → 2 Fe2O3 (s) ΔH = -1648 kJ52.0 g of Fe (MM = 55.845 g/mol) are reacted as above in 1.000 x 103 g of water (MM = 18.02, ΔHFUSION = 6.01 kJ/mol, ΔHVAP = 40.65 kJ/mol, specific heat = 4.18 J/(g C) that is at 20.0 °C. What will the final temperature of the water be?Select one:367 112 20.1 91.8 100The vaporisation of a certain element at 23.0 oC has the following enthalpy and entropy values: Hvap = 7.00 kJ mol-1 and Svap = 246 J K mol-1. What is the total entropy change (Stot) for the vaporisation of this element, in J K-1 mol-1? (Enter your answer as a number only, with the correct number of significant figures!)Calculate the change in entropy (in J/K) when 400 mL of water at 33.8 ⁰C is heated to 55 ⁰C at constant pressure. Specific heat capacity of water at constant pressure is 4.183 J/g-K. Density of water at different temperature is presented (use this table only). Answer Format: [2 decimals