Calculate the change in heat when 18.50 g of water vapor (steam) at 100.0°C condenses to liquid water and then cools to 18.50 °C.

A 33.6-g piece of silver initially at 46.5 °C is submerged into 162.4 g of water at 12.3 °C. What is the final temperature of the metal once the metal and water reaches thermal equilibrium? The specific heats of silver and water are 0.235 J/g·°C and 4.18 J/g·°C, respectively. 29.4 °C 10.4 °C 11.0 °C 12.7 °C 21.0 °C

A particular sample of cold graphite at 10.20 °C was added to 988.5 g of water at 25.31 °C in a constant pressure calorimeter. If the final temperature of the graphite and water was 25.17 °C, what was the mass of the graphite sample? Assume no heat was lost to the surroundings. The specific heat for water is 4.184 J/g•°C and the specific heat for this graphite is 0.7069 J/g•°C.

A 0.870-g piece of lithium metal is dropped into a mixture of 50.0 g water and 50.0 g ice, both at 0°C. The reaction is 2 Li(s) + 2 H₂O(l) → 2 LiOH(aq) + H₂(g) ∆H = 446 kJ/mol Assuming no heat is lost to the surroundings, and that the final mixture has a specific heat capacity of 4.18 J/g･°C, calculate the final temperature in °C. The enthalpy of fusion for ice is 6.02 kJ/mol.

The molar heat of solution of a substance is found to be +21.38 kJ/mol. The addition of 0.100 mol of this substance to 1.000L of water initially at 40.0 degrees celsius results in a temperature decrease. Assume the specific heat of the resulting solution to be equal to that of pure water. Find the final temperature of the solution (Also assume that the heat capacity of the calorimeter is negligible).

4. 30.0 g of a substance (molar mass: 46 g/mo) required 262 J of heat to raise its temperature from 32.0°C to 37.4°C. What is the specific heat per gram and per mole of this substance?

The specific heat of substance C is 0.93 J/(g K) and that of substance D is 1.8 J/(g K). You are given an unknown that could be pure substance C, pure substance D, or a homogeneous mixture of C and D. In the lab you determine that it requires 23.3 J of heat energy to raise the temperature of a 25.0 g sample of the unknown by 1.0 K. What conclusions can you make about the identity of your unknown, from this data?

A 35.19 g sample of a substance is initially at 27.1 °C. After absorbing 1533 J of heat, the temperature of the substance is 186.9 °C. What is the specific heat (?) of the substance?

A chemical reaction takes place inside a flask submerged in a water bath. The water bath contains 6.30 kg of water at 21.7 °C. During the reaction 143. kJ of heat flows out of the bath and into the flask. Calculate the new temperature of the water bath. You can assume the specific heat capacity of water under these conditions iS 4.18 J·g¯¹·K¯¹. Round your answer to 3 significant digits.

To treat a burn on his hand, a person decides to place an ice cube on the burned skin. The mass of the ice cube is 15.2 g, and its initial temperature is −13.9 ∘C. The water resulting from the melted ice reaches the temperature of his skin, 29.9⁢ ∘C. How much heat is absorbed by the ice cube and resulting water? Assume that all of the water remains in the hand. Constants for water can be found in this table.   Enthalpy of fusion 333.6 J/g 6010. J/mol Enthalpy of vaporization 2257 J/g 40660 J/mol Specific heat of solid H 2 O (ice) 2.087 J/(g·°C) * 37.60 J/(mol·°C) *  Specific heat of liquid H 2 O (water) 4.184 J/(g·°C) * 75.37 J/(mol·°C) *  Specific heat of gaseous H 2 O (steam) 2.000 J/(g·°C) * 36.03 J/(mol·°C) *