Calculate the entropy change (J/K) for the vaporization of 14.4 g of a hydrocarbon (88 g/mole]),...
Calculate the entropy change (J/K) for the vaporization of 14.4 g of a hydrocarbon (88 g/mole]), at its boiling point of 86.8°C. The enthalpy of vaporization of this hydrocarbon is 25.1 kJ/mol. Enter to 2 decimal places.
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Calculate the entropy change (J/K) for the vaporization of 14.4
g of a hydrocarbon (88 g/mole]),...
Entropy and Change of State The standard enthalpy of vaporization for CHFCI2 is 242.17 J/g at...
Entropy and Change of State The standard enthalpy of vaporization for CHFCI2 is 242.17 J/g at its normal boiling point of 8.92°C. Calculate the standard entropy of vaporization (AS°vap) of CHFC12(1). Answer to the nearest 0.1 J K-1 mol-1. cf Zumdahl Chemical Principles 8th ed. sec. 10.4 pp 362-5. Submit Answer Tries 0/5
The heat of vaporization of CH_2CI_2 is 28.0 kJ/mol. Calculate the entropy the entropy change when...
The heat of vaporization of CH_2CI_2 is 28.0 kJ/mol. Calculate the entropy the entropy change when 42 g of CH_2CI_2 boils at its boiling point of 39.8degreeC. 17 J/K 44J/K 59J/K 350J/K 700J/K
Calculate the change in entropy that occurs in the system when 3.90 mole of diethyl ether...
Calculate the change in entropy that occurs in the system when 3.90 mole of diethyl ether (C4H6O) condenses from a gas to a liquid at its normal boiling point (34.6∘C). ΔHvap = 26.5 kJ/mol. Answer in J/K
Calculate the change in entropy (in J/K) that occurs when a sample containing 2.00 moles of...
Calculate the change in entropy (in J/K) that occurs when a sample containing 2.00 moles of water is heated from 10.00°C to 300.0 °C at 1 atm pressure. Molar Heat Capacity H2O(1) = 75.3 JK' moi? H2O(g) = 36.4 JK' mol Enthalpy of Vaporization at 100 °C = 40.7 kJ mol .-1 -1 Answer:
boiling point (BP) of n-pentane, given that the entropy 67 I/mol x °K and the change...
boiling point (BP) of n-pentane, given that the entropy 67 I/mol x °K and the change in enthalpy is 26.8 kJ/mole 14) (6 Points) Calculate the boil change at the BP is 86.7 J/mol v
3. The normal boiling point for the chloro-fluoro- hydrocarbon C,C1,F3 is 47.6°C: C C1,F3(1) C_C1zFz (g)...
3. The normal boiling point for the chloro-fluoro- hydrocarbon C,C1,F3 is 47.6°C: C C1,F3(1) C_C1zFz (g) We have []Hºvap = 27.49 kJ/mol. What is [Sºvap for the vaporization of C ClzFz at its normal boiling point? a) b) c) d) 33.1 J/K mole 5.2 J/K mole 71.2 J/K mole 85.7 J/K mole 4. For the following chemical reaction: H2(g) + CO(g) CH,Og) we have [H°(298) = 1.9 kJ/mole and [S°(298) = -109.6 J/Kmole. What is []Gº(298) for this reaction? a)...
3. A liquid compound has an enthalpy of vaporization equal to 65.0 kJ and an entropy...
3. A liquid compound has an enthalpy of vaporization equal to 65.0 kJ and an entropy of equal to 98 J/K at its boiling point. Calculate the boiling point of the compound. AH = 65 kJ AS - 987
Physical Chemistry Calculate the change in entropy when one mole of metallic aluminum is heated at...
Physical Chemistry
Calculate the change in entropy when one mole of metallic aluminum is heated at one bar pressure from an initial temperature of 25 °C to a final temperature of 750 °C. The molar heat capacities of solid and liquid aluminum at one bar pressure are 29.2 J mol K1 and 31.75 J mol K, respectively. The specific enthalpy of fusion of aluminum at its melting point (660.46 °C) is 396.57 J g1. The molar mass of aluminum is...
Calculate the change in entropy when one mole of metallic aluminum is heated at one bar...
Calculate the change in entropy when one mole of metallic aluminum is heated at one bar pressure from an initial temperature of 25 °C to a final temperature of 750 °C. The molar heat capacities of solid and liquid aluminum at one bar pressure are 29.2 J mol' K and 31.75 J mol' K, respectively. The specific enthalpy of fusion of aluminum at its melting point (660.46 °C) is 396.57 J g! The molar mass of aluminum is 26.98 g...
The vaporization of compound A is described by the following chemical equation. A(1) A(8) A rap(72.39...
The vaporization of compound A is described by the following chemical equation. A(1) A(8) A rap(72.39 °C) = 38.21 kJ/mol Calculate the entropy of vaporization, Aswap, for A(l) at 25.0 °C given that the boiling point of A is 72.39 °C, and the molar heat capacity of A(l) is 119.09 J/mol K). Assume that the molar heat capacity of A(R) is 56.5% of that of A(1). ASP J. mol-K Calculate the standard enthalpy of vaporization. A Hap, for A(1) at...
Entropy and Change of State The standard enthalpy of vaporization for CHFCI2 is 242.17 J/g at its normal boiling point of 8.92°C. Calculate the standard entropy of vaporization (AS°vap) of CHFC12(1). Answer to the nearest 0.1 J K-1 mol-1. cf Zumdahl Chemical Principles 8th ed. sec. 10.4 pp 362-5. Submit Answer Tries 0/5
The heat of vaporization of CH_2CI_2 is 28.0 kJ/mol. Calculate the entropy the entropy change when 42 g of CH_2CI_2 boils at its boiling point of 39.8degreeC. 17 J/K 44J/K 59J/K 350J/K 700J/K
Calculate the change in entropy (in J/K) that occurs when a sample containing 2.00 moles of water is heated from 10.00°C to 300.0 °C at 1 atm pressure. Molar Heat Capacity H2O(1) = 75.3 JK' moi? H2O(g) = 36.4 JK' mol Enthalpy of Vaporization at 100 °C = 40.7 kJ mol .-1 -1 Answer:
boiling point (BP) of n-pentane, given that the entropy 67 I/mol x °K and the change in enthalpy is 26.8 kJ/mole 14) (6 Points) Calculate the boil change at the BP is 86.7 J/mol v
3. The normal boiling point for the chloro-fluoro- hydrocarbon C,C1,F3 is 47.6°C: C C1,F3(1) C_C1zFz (g) We have []Hºvap = 27.49 kJ/mol. What is [Sºvap for the vaporization of C ClzFz at its normal boiling point? a) b) c) d) 33.1 J/K mole 5.2 J/K mole 71.2 J/K mole 85.7 J/K mole 4. For the following chemical reaction: H2(g) + CO(g) CH,Og) we have [H°(298) = 1.9 kJ/mole and [S°(298) = -109.6 J/Kmole. What is []Gº(298) for this reaction? a)...
3. A liquid compound has an enthalpy of vaporization equal to 65.0 kJ and an entropy of equal to 98 J/K at its boiling point. Calculate the boiling point of the compound. AH = 65 kJ AS - 987
Physical Chemistry
Calculate the change in entropy when one mole of metallic aluminum is heated at one bar pressure from an initial temperature of 25 °C to a final temperature of 750 °C. The molar heat capacities of solid and liquid aluminum at one bar pressure are 29.2 J mol K1 and 31.75 J mol K, respectively. The specific enthalpy of fusion of aluminum at its melting point (660.46 °C) is 396.57 J g1. The molar mass of aluminum is...
Calculate the change in entropy when one mole of metallic aluminum is heated at one bar pressure from an initial temperature of 25 °C to a final temperature of 750 °C. The molar heat capacities of solid and liquid aluminum at one bar pressure are 29.2 J mol' K and 31.75 J mol' K, respectively. The specific enthalpy of fusion of aluminum at its melting point (660.46 °C) is 396.57 J g! The molar mass of aluminum is 26.98 g...
The vaporization of compound A is described by the following chemical equation. A(1) A(8) A rap(72.39 °C) = 38.21 kJ/mol Calculate the entropy of vaporization, Aswap, for A(l) at 25.0 °C given that the boiling point of A is 72.39 °C, and the molar heat capacity of A(l) is 119.09 J/mol K). Assume that the molar heat capacity of A(R) is 56.5% of that of A(1). ASP J. mol-K Calculate the standard enthalpy of vaporization. A Hap, for A(1) at...
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