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

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.

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)]

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?

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.

What will be the final temperature in °C if a 5.00-g silver ring at 37.0 °C gives off 25.0 J of heat to its surroundings? (specific heat = 0.235 J g^-1 °C^-1)

A 125 ml sample of water at 293.2 K was heated for 8 minutes 25 seconds with a constant temperature increase of 3 degrees Fahrenheit per minute. What is the final temperature of the water in degrees Celsius?

How many calories are needed to raise the temperature of 32g of water from 12 degrees Celsius to 54 degrees Celsius?