115.4 g of water, H2O, (molar mass is 18.02 g/mol) was heated from -11.54 °C to 135.72 °C. The freezing and boiling point of water is 0.0 °C and 100. °C, respectively. The specific heat capacities of solid, liquid, and gaseous water is 2.03 J/(g*K), 4.18 J/(g*K), and 1.84 J/(g*K), respectively. The heat of fusion and vaporization of water is 6.01 kJ/mol and 40.67 kJ/mol, respectively. How much heat, in kJ, is required?

A gold coin whose mass is 8.47 g is heated to 138.9oC and then quickly dropped into an ice calorimeter. What mass of ice melts? (The amount of heat in an ice calorimeter is determined from the quantity of ice the melts, knowing that it takes 6.01 kJ of heat to melt exactly one mole of ice. Molar heat capacity of gold is 25.418 J/mol/K)

4

Ethylene glycol (specific heat 2.42 J/g°C) is used as a coolant in automotive engines. Calculate the energy released (q) when 3.65 kg of ethylene glycol is cooled from 132 °C to 85 °C.

The temperature of a sample of iron increased by 22.0 °C22.0 °C when 269 J269 J of heat was applied. What is the mass of the sample?   Substance Specific heat J/(g · °C) lead 0.128 silver 0.235 copper 0.385 iron 0.449 aluminum 0.903

4. Aluminum metal melts at 658.5°C. What would be the final temperature if 28.0 grams of solid aluminum at this temperature were placed into 520 grams of liquid aluminum at 1000.0°C? The heat of fusion for aluminum is 396 J/ -1 -1 g, and the specific heat of liquid aluminum is 0.481 J-g`¹deg-¹. (Note: this is the aluminum analog to the process you just did in lab!)

A 4.70-g sample of aluminum pellets (specific heat capacity = 0.89 J °C- g) and a 10.00-g sample of iron pellets (specific heat capacity = 0.45 J °C- g) are heated to 115.0°C. The mixture of hot iron and aluminum is then dropped into 98.3 g of water at 22.0°C. Calculate the final temperature of the metal and water mixture, assuming no heat loss to the surroundings. The specific heat capacity of water is 4.18 J °C¯'g¬! °C

Calculate the heat required  to raise the temperature of a 50.0 g of water from 25.0 °C to 39.0 °C. (The specific heat capacity of water is 4.184 J·g–1·°C–1). A) 2.93 kJ B) 4.18 kJ C) 5.23 kJ D) 8.16 kJ         0.163 kJ

A soft drink (290 mL of mostly water) initially at 18.0 C is cooled by adding 197 g of ice cubes at 0 C. What mass of ice remains when the temperature of the drink reaches equilibrium (water and ice at 0 C)? The enthalpy of fusion of water (i.e., the heat required to melt ice) is 6.007 kJ/mol. The density of the water is 1.0 g/mL. Assume the specific heat capacity of water is constant and equal to 4.184 J/g/C.