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.

An 80.0 g sample of metal, initially at 96.0 °C, is placed into 150.0 g of water initially at 26.0 °C in a calorimeter. The final temperature of the water is 28.1 °C. What is the identity of the metal? (The specific heat of water is 4.18 J/g°C.)

Consider the dissolution of CaCl2: CaCl2(s) -> Ca²⁺(aq) + 2Cl⁻(aq), ΔH = -81.5 kJ. An 11.6 g sample of CaCl2 is dissolved in 126 g water, with both substances at 24.3°C. Calculate the final temperature of the solution assuming no heat loss to the surroundings. What is the final temperature of the solution?

Given 352 mL of water at 26 °C in a perfectly heat-insulating container, how much ice at 0 °C (in grams) would have to be added to this water so that after the ice has melted, the overall temperature of the system has been lowered to 5 °C?

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 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?