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5. (14 pts) Calculate the entropy change As for the follow ate the entropy change AS...
8) Find the molar entropy change when H20 (1) at 1.00 atm and 300 K is...
8) Find the molar entropy change when H20 (1) at 1.00 atm and 300 K is changed to H2O (g) at 1.00 atm and 500 K. The enthalpy of vaporization of H2O is 40.66 kJ mol"! Cp [H2O(1)]=[12.16-1.943 x 10-2T +3.042 x 10-ST?]R Cpm[H,0(8)]=[3.633–1.195 x 10-T +1.34 x 10-?T?]R
Calculate the change in entropy that occurs when 18.02 g of ice at –17.5°C is placed...
Calculate the change in entropy that occurs when 18.02 g of ice at –17.5°C is placed in 90.08 g of water at 100.0°C in a perfectly insulated vessel. Assume that the molar heat capacities for H2O(s) and H2O(l) are 37.5 J K^-1 mol^-1 and 75.3 J K^-1 mol^-1, respectively, and the molar enthalpy of fusion for ice is 6.01 kJ/mol. Change in entropy = ______J/K
References Calculate the change in entropy that occurs when 18.02 g of ice at -12.5C is...
References Calculate the change in entropy that occurs when 18.02 g of ice at -12.5C is placed in 45,04 g of water at 100.0°C in a perfectly insulated vessel. Assume that the molar heat capacities for H2O(s) and H2O(l) are 37.5 JK-mol-and 753 JK mol", respectively, and the molar enthalpy of fusion for ice is 6.01 kJ/mol. Change in entropy - JK Submit Answer T ry Another Version 3tem attempts remaining
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...
17.51 Calculate the entropy change for the following processes. (a) 1.00 mol H,O(s) melts at 0...
17.51 Calculate the entropy change for the following processes. (a) 1.00 mol H,O(s) melts at 0 °C. AH = 6.01 kJ/mol. (b) 2.00 mol CH.() vaporizes at 80.0 °C. AH vap = 30.7 kJ/mol. 17.52 - Calculate the entropy change for the following processes. (a) 2.00 mol NH3(e) vaporizes at -33.0 °C. AHvap = 23.35 kJ/mol. (b) 1.00 mol C,H,OH(s) melts at -114 °C. AHjus = 5.0 kJ/mol. 17.53 Use data from Appendix G to calculate the standard entropy change...
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
1. a) Calculate the change in entropy (AS) when one mole of diamond is heated from...
1. a) Calculate the change in entropy (AS) when one mole of diamond is heated from a temperature of 0 K to 400 K at a constant pressure of 1 bar. The temperature-dependent heat capacity of diamond is C 2.9x10 T J/(mol K), where T is the absolute temperature in K. b) Given that the entropy of diamond is zero at 0 K, calculate its absolute molar entropy (S) at 400 K from the above result.
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.
3. Calculate the change in entropy when 50.0 g of ethanol at 50.0 °C is poured into 70.0 g of ethanol at 10.0°C in...
3. Calculate the change in entropy when 50.0 g of ethanol at 50.0 °C is poured into 70.0 g of ethanol at 10.0°C in an isolated vessel given that Cp.m is 111.5 J/mol K. a) Determine the final temperature of the system. (ANS: 299.9 K) b) Calculate the entropy change for the process (ANS: AS = 273.8 kJ/mole)
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:
8) Find the molar entropy change when H20 (1) at 1.00 atm and 300 K is changed to H2O (g) at 1.00 atm and 500 K. The enthalpy of vaporization of H2O is 40.66 kJ mol"! Cp [H2O(1)]=[12.16-1.943 x 10-2T +3.042 x 10-ST?]R Cpm[H,0(8)]=[3.633–1.195 x 10-T +1.34 x 10-?T?]R
References Calculate the change in entropy that occurs when 18.02 g of ice at -12.5C is placed in 45,04 g of water at 100.0°C in a perfectly insulated vessel. Assume that the molar heat capacities for H2O(s) and H2O(l) are 37.5 JK-mol-and 753 JK mol", respectively, and the molar enthalpy of fusion for ice is 6.01 kJ/mol. Change in entropy - JK Submit Answer T ry Another Version 3tem attempts remaining
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...
17.51 Calculate the entropy change for the following processes. (a) 1.00 mol H,O(s) melts at 0 °C. AH = 6.01 kJ/mol. (b) 2.00 mol CH.() vaporizes at 80.0 °C. AH vap = 30.7 kJ/mol. 17.52 - Calculate the entropy change for the following processes. (a) 2.00 mol NH3(e) vaporizes at -33.0 °C. AHvap = 23.35 kJ/mol. (b) 1.00 mol C,H,OH(s) melts at -114 °C. AHjus = 5.0 kJ/mol. 17.53 Use data from Appendix G to calculate the standard entropy change...
1. a) Calculate the change in entropy (AS) when one mole of diamond is heated from a temperature of 0 K to 400 K at a constant pressure of 1 bar. The temperature-dependent heat capacity of diamond is C 2.9x10 T J/(mol K), where T is the absolute temperature in K. b) Given that the entropy of diamond is zero at 0 K, calculate its absolute molar entropy (S) at 400 K from the above result.
3. Calculate the change in entropy when 50.0 g of ethanol at 50.0 °C is poured into 70.0 g of ethanol at 10.0°C in an isolated vessel given that Cp.m is 111.5 J/mol K. a) Determine the final temperature of the system. (ANS: 299.9 K) b) Calculate the entropy change for the process (ANS: AS = 273.8 kJ/mole)
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:
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