How much energy is needed to raise the temperature of 5.0 grams of lead from 25°C to 35°C? [specific heat (c) = 0.129 J/(g°C)]

A 60 g piece of zinc is initially at 20°C. It is then dropped into 200 g of water, which is at 100°C. Assuming no heat loss to the surroundings, what is the final temperature of the system? (The specific heat capacity of zinc is 0.389 J/g°C and the specific heat capacity of water is 4.18 J/g°C.)

What is the equivalent temperature in Celsius when 89°F is converted?

Determine the temperature change that occurs when 10.6 g of potassium perchlorate (KClO4) is dissolved in enough water to make 104.8 mL of solution, given that the enthalpy of dissolution is -55.5 kJ/mol.

How many grams of ice at -6.3 °C can be completely converted to liquid at 9.9 °C if the available heat for this process is 5.20 x 10^3 kJ? For ice, use a specific heat of 2.01 J/(g·°C) and ΔHfus=6.01 kJ/mol. Express your answer to three significant figures.

If 55.0 mL of ethanol (density = 0.789 g/mL) initially at 8.0 °C is mixed with 55.0 mL of water (density = 1.0 g/mL) initially at 28.0 °C in an insulated beaker, what is the final temperature of the mixture, assuming that no heat is lost to the surroundings?

Suppose that to a mug containing 125 mL of water at a temperature of 90.0 °C we add 165 mL of water at an unknown temperature and mix the contents well. What is that unknown temperature if the final temperature of water in the mug is 58.3 °C?

The temperature of a room is 19.1 °C. What is this temperature expressed in Kelvin (K)?

What volume of water (in mL), initially at 75.6 °C, needs to be mixed with 229 mL of water, initially at 20.7 °C, so that the final temperature of the water is 41.8 °C? Assume that the density of water remains constant over the above temperature range.