It is observed that 3.23 kcal of energy are released when a 40.5 g sample of an unknown liquid condenses.
What is the heat of vaporization of the unknown liquid in cal/g?
Heat of vaporization = ? cal/g
It is observed that 3.23 kcal of energy are released when a 40.5 g sample of...
An amount 10.24 kcal of heat is added to a 35.0 g sample of a liquid at 25.0°C. The final temperature is 87.4°C. What is the specific heat of the substance in cal/g°C?
How much energy (in kilojoules) is released when 12.6 g of steam at 110.5 ∘C is condensed to give liquid water at 67.0 ∘C? The heat of vaporization of liquid water is 40.67 kJ/mol, and the molar heat capacity is 75.3 J/(K⋅mol) for the liquid and 33.6 J/(K⋅mol) for the vapor.
9) How much energy in Kcal is needed to take 340 g of water at 6.0 degrees Celsius to steam at 127.0 degrees Celsius? ALSO indicate this process as a heating curve on the axes below. [the specific heat of ice, water and steam are 0.47, 1.00, and 0.48 cal/g oC respectively, Also the Heat of Fusion and Heat of vaporization of water are 80, and 540 cal/g respectively] You may or may not need all of these numbers. hny...
1. How much energy (in kilojoules) is released when 16.4 g of steam at 116.5 ∘C is condensed to give liquid water at 60.5 ∘C? The heat of vaporization of liquid water is 40.67 kJ/mol, and the molar heat capacity is 75.3 J/(K⋅mol) for the liquid and 33.6 J/(K⋅mol) for the vapor. 2.What is the entropy of fusion, ΔSfusion [in J/(K⋅mol)] for sodium? The necessary data are the following: mp = 97.8 ∘C,bp = 883 ∘C, ΔHvap = 89.6kJ/mol, and...
Calculate the energy released when 50.0g of steam condenses at 100℃.Use the cooling curve to show what happens when 50.0g steam condenses at 100℃ and then cools to 20℃. Then calculate this energy change.6. Use the below cooling curve for water for the following questions. A. Label the melting/freezing point. B. Label the boiling/evaporation point. C. At what state is water when the temperature is 80 °c? D. At what state is water when the temperature is -20 °C? E. What happens to the temperature...
the heat of vaporization of water at 100C is 2.26kj/g. calculate the quantity of heat and specify if heat is absorbed or released when 9.00 g of steam condenses to liquid water at 100C
Calculate the heat that is absorbed/released when 9.00 g of steam condenses to liquid water at 100°C. DHvap(water) = 40.66 kJ/mol.
8. Use the data in the Introduction calculate the total amount of heat in kcal required to turn 100 g of ice at -20°C to steam at 120°C? liq gas equilibrium (heat goes into phase change) Steam - Water and steam allas (heat goes into temperature change) Temperature (°C) all liquid (heat goes into temperature change) -Water Ice and water all solid Nice solid/liq equilibrium (heat goes into phase change) - Time Heat On the 5 sections of the graph...
15. When gasoline burns in a car engine, the heat released causes the products CO2 and H20 to expand, which pushes the pistons outward. Excess heat is removed by the car's radiator. If the expanding gases do 478.9 J of work on the pistons and the system releases 846.8 J to the surroundings as heat, calculate the change in energy (AE) in J, KJ, and kcal. (4.0 pts) Energy change Your solutions (AE-+ w) (1 cal = 4.184 J, 1...
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A 272.3 gram sample of an unknown substance (MM = 189.50 g/mol) is cooled from 233.0 °C to 147.6 °C. (heat capacity of liquid = 1.62 J/g. °C; heat capacity of gas = 1.04 J/g. °C; AHvap = 78.11 kJ/mol; Tb = 160.3 °C) How much energy (in kJ) is absorbed/released to cool the gas? pple A 272.3 gram sample of an unknown substance (MM = 189.50 g/mol) is cooled from 233.0 °C to 147.6 °C. (heat capacity...