8. Thermochemistry

How much energy is needed to vaporize 75.0 g of diethyl ether (C4H10O) at its boiling point (34.6 °C), given that ΔHvap of diethyl ether = 26.5 kJ/mol?

How much energy must be removed from a 125 g sample of benzene (molar mass = 78.11 g/mol) at 425.0 K to liquify the sample and lower the temperature to 335.0 K? The following physical data may be useful: ΔHvap = 33.9 kJ/mol, ΔHfus = 9.8 kJ/mol, Cliq = 1.74 J/g·K.

How much heat is released when 125.0 g of steam at 100.0°C is cooled to ice at -15.0°C? The enthalpy of vaporization of water is 40.67 kJ/mol, the enthalpy of fusion for water is 6.01 kJ/mol, the molar heat capacity of liquid water is 75.4 J/(mol·°C).

How much ice (in grams) at 0°C would have to melt to lower the temperature of 355 mL of water from 26°C to 5°C? (Assume the density of water is 1.0 g/mL and the specific heat capacity of water is 4.18 J/g°C, and the heat of fusion of ice is 334 J/g.)

If 45.0 mL of ethanol (density = 0.789 g/mL) initially at 9.0 °C is mixed with 45.0 mL of water (density = 1.0 g/mL) initially at 28.2 °C in an insulated beaker, what is the final temperature of the mixture, assuming that no heat is lost?

If 55.0 mL of ethanol (density = 0.789 g/mL) initially at 9.0 °C is mixed with 55.0 mL of water (density = 1.0 g/mL) initially at 28.7 °C in an insulated beaker, what is the final temperature of the mixture, assuming that no heat is lost and the specific heat capacities are 2.44 J/g°C for ethanol and 4.18 J/g°C for water?

If you combine 350.0 mL of water at 25.00°C and 100.0 mL of water at 95.00°C, what is the final temperature of the mixture, assuming no heat is lost to the surroundings?

An aluminum block initially at 25°C loses 2.89 x 10^3 J of heat. If the specific heat capacity of aluminum is 0.897 J/g°C and the mass of the block is 150 g, what is the final temperature of the aluminum?

A 101 g piece of aluminum (c_aluminum = 0.900 J/g°C) is heated to 128.1 °C and added to 62.6 g of water at an initial temperature of 24.2 °C. Assuming no heat is lost to the surroundings, what will the final temperature of the mixture be?

Ice cubes at exactly 0°C with a total mass of 54.0 g are combined with 140 g of water at 75°C in an insulated container. Given that the heat of fusion (ΔH_fus) is 6.02 kJ/mol and the specific heat capacity of water (c_water) is 4.18 J/g°C, what is the final temperature of the system if no heat is lost to the surroundings?