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The fluorocarbon compound C_2CI_3F_3 has a normal boding point of 47.6 degree C The specific heats...
The fluorocarbon compound C2Cl3F3 has a normal boiling point of 47.6 ∘C. The specific heats of...
The fluorocarbon compound C2Cl3F3 has a normal boiling point of 47.6 ∘C. The specific heats of C2Cl3F3(l) and C2Cl3F3(g) are 0.91 J/g⋅K and 0.67 J/g⋅K, respectively. The heat of vaporization for the compound is 27.49 kJ/mol. Calculate the heat required to convert 45.5 g of C2Cl3F3 from a liquid at 14.10 ∘C to a gas at 78.40 ∘C. Express your answer using two significant figures.
The flourocarbon compound C2Cl3F3 has a normal boiling point of 47.6oC. The specific heats of C2Cl3F3(l)...
The flourocarbon compound C2Cl3F3 has a normal boiling point of 47.6oC. The specific heats of C2Cl3F3(l) and C2Cl3F3(g) are 0.91 J/g-K and 0.67 J/g-K, respectively. The heat of vaporization for the compound is 27.49 kJ/mol. Calculate the heat required to convert 50.0 grams of C2Cl3F3 from a liquid at 10 degrees Celcius to a gas at 85 degrees celcius.
Question 11 (1 point) The solubility of nitrogen gas in water at 25 °C is 6.8x104...
Question 11 (1 point) The solubility of nitrogen gas in water at 25 °C is 6.8x104 mol / (L'atm). If the partial pressure of nitrogen gas is (1.60x10*0) atm, what is the concentration (molarity) of dissolved nitrogen? Report to 3 significant figures. Note: Your answer is assumed to be reduced to the highest power possible. Your Answer: x10 Answer Save Question 12 (1 point) The fluorocarbon C2CI3F3 has a normal boiling point of 476 °C The specific heats of C2C13F3D...
ID: 10. Identify the place which has the highest boiling point of water, a Death Valley,...
ID: 10. Identify the place which has the highest boiling point of water, a Death Valley, 282 feet below sea level b. A pressurized passenger jet, 39,000 feet C. Panama City, Florida, sea level d. Mt. Everest, 29,035 feet c. Denver, Colorado, 5,280 feet d. Minha City, Florcnger jet. c. Der Everest, 29 onda, sea le 39,000 feet 11. The heat of vaporization of water at 100°C is 40.66 kJ/mol Calculate the quantity of heat that is absorbed released when...
5. (4 pts) The compound C2C13F3 has been used as a cooling agent in refrigerants and...
5. (4 pts) The compound C2C13F3 has been used as a cooling agent in refrigerants and air conditioners. It has a boiling point of 47.6 °C. The specific heats of C2Cl3F3 (l) and C2C13F3 (g) are 0.91 Jg-2 K-2 and 0.67 Jg-1K-2, respectively. The heat of vaporization for the compound is 27.49 kJ/mol. Calculate the heat absorbed by 35.0 g of C2C13F3 while going from a liquid at 10.00 °C to a gas at 105.00 °C.
How much heat energy is required to convert 82.0 g of solid ethanol at -114.5 degree...
How much heat energy is required to convert 82.0 g of solid ethanol at -114.5 degree C to gaseous ethanol at 167.4 degree C? The molar heat of fusion of ethanol is 4.60 kJ/mol and its molar heat of vaporization is 38.56 kJ/mol. Ethanol has a normal melting point of -114.5 degree C and a normal boiling point of 78.4 degree C. The specific heat capacity of liquid ethanol is 2.45 J/g middot degree C and that of gaseous ethanol...
Can you show the work for these problems? Ethanol has an enthalpy of vaporization of 42.3...
Can you show the work for these problems?
Ethanol has an enthalpy of vaporization of 42.3 kJ/mol. The compound has a vapor pressure of 1.00 atm at 78.3 degree C. At what temperature is the vapor pressure equal to 0.800 atm? (R = 8.314 J/K middot mol) -83.8 degree C -24.4 degree C 62.6 degree C 73.0 degree C 78.0 degree C A liquid has an enthalpy of vaporization of 30.4 kJ/mol. At 269 K is has a vapor pressure...
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)...
Be sure to answer all parts. The molar heats of fusion and vaporization of a certain...
Be sure to answer all parts. The molar heats of fusion and vaporization of a certain substance are 2.89 kJ/mol and 8.84 kJ/mol, and its melting point and boiling point are -177°C and -141°C, respectively. Calculate the entropy changes for fusion (solid to liquid) and vaporization (liquid to gas). ASfus J/K mol AS vap = J/K mol
Be sure to answer all parts. The molar heats of fusion and vaporization of a certain...
Be sure to answer all parts. The molar heats of fusion and vaporization of a certain substance are 2.37 kJ/mol and 8.91 kJ/mol, and its melting point and boiling point are -165°C and -120°C, respectively. Calculate the entropy changes for fusion (solid to liquid) and vaporization (liquid to gas). AS fus J/K mol ASvap - J/K'mol
Question 11 (1 point) The solubility of nitrogen gas in water at 25 °C is 6.8x104 mol / (L'atm). If the partial pressure of nitrogen gas is (1.60x10*0) atm, what is the concentration (molarity) of dissolved nitrogen? Report to 3 significant figures. Note: Your answer is assumed to be reduced to the highest power possible. Your Answer: x10 Answer Save Question 12 (1 point) The fluorocarbon C2CI3F3 has a normal boiling point of 476 °C The specific heats of C2C13F3D...
ID: 10. Identify the place which has the highest boiling point of water, a Death Valley, 282 feet below sea level b. A pressurized passenger jet, 39,000 feet C. Panama City, Florida, sea level d. Mt. Everest, 29,035 feet c. Denver, Colorado, 5,280 feet d. Minha City, Florcnger jet. c. Der Everest, 29 onda, sea le 39,000 feet 11. The heat of vaporization of water at 100°C is 40.66 kJ/mol Calculate the quantity of heat that is absorbed released when...
5. (4 pts) The compound C2C13F3 has been used as a cooling agent in refrigerants and air conditioners. It has a boiling point of 47.6 °C. The specific heats of C2Cl3F3 (l) and C2C13F3 (g) are 0.91 Jg-2 K-2 and 0.67 Jg-1K-2, respectively. The heat of vaporization for the compound is 27.49 kJ/mol. Calculate the heat absorbed by 35.0 g of C2C13F3 while going from a liquid at 10.00 °C to a gas at 105.00 °C.
How much heat energy is required to convert 82.0 g of solid ethanol at -114.5 degree C to gaseous ethanol at 167.4 degree C? The molar heat of fusion of ethanol is 4.60 kJ/mol and its molar heat of vaporization is 38.56 kJ/mol. Ethanol has a normal melting point of -114.5 degree C and a normal boiling point of 78.4 degree C. The specific heat capacity of liquid ethanol is 2.45 J/g middot degree C and that of gaseous ethanol...
Can you show the work for these problems?
Ethanol has an enthalpy of vaporization of 42.3 kJ/mol. The compound has a vapor pressure of 1.00 atm at 78.3 degree C. At what temperature is the vapor pressure equal to 0.800 atm? (R = 8.314 J/K middot mol) -83.8 degree C -24.4 degree C 62.6 degree C 73.0 degree C 78.0 degree C A liquid has an enthalpy of vaporization of 30.4 kJ/mol. At 269 K is has a vapor pressure...
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)...
Be sure to answer all parts. The molar heats of fusion and vaporization of a certain substance are 2.89 kJ/mol and 8.84 kJ/mol, and its melting point and boiling point are -177°C and -141°C, respectively. Calculate the entropy changes for fusion (solid to liquid) and vaporization (liquid to gas). ASfus J/K mol AS vap = J/K mol
Be sure to answer all parts. The molar heats of fusion and vaporization of a certain substance are 2.37 kJ/mol and 8.91 kJ/mol, and its melting point and boiling point are -165°C and -120°C, respectively. Calculate the entropy changes for fusion (solid to liquid) and vaporization (liquid to gas). AS fus J/K mol ASvap - J/K'mol
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