7.0 g of cream at 13.3 °C are added to an insulated cup containing 100.0 g of coffee at 84.0 °C. Calculate the equilibrium temperature of the coffee. You may assume no heat is lost to the cup or surroundings, and that any physical properties of cream and coffee you need are the same as those of water. Be sure your answer has 3 significant digits. °C x10 X

12.0 g of cream at 23.0 °C are added to an insulated cup containing 100.0 g of coffee at 78.1 °C. Calculate the equilibrium temperature of the coffee. You may assume no heat is lost to the cup or surroundings, and that any physical properties of cream and coffee you need are the same as those of water. Be sure your answer has 3 significant digits. 0 °C 0 x10 X

Which statement best defines specific heat? The amount of heat required to increase the temperature of 1 mol of a substance by 1 °C. The amount of heat required to increase the temperature of a specific object, such as a calorimeter, by 1 °C. The amount of heat required to increase the temperature of 1 g of a substance by 1 °C. The amount of heat required to increase the temperature of 1 L of a substance by 1 °C.

A 50.5 g sample of quartz is put into a calorimeter (see sketch at right) that contains 150.0 g of water. The quartz sample starts off at 98.8 °C and the temperature of the water starts off at 15.0 °C. When the temperature of the water stops changing it's 19.5 °C. The pressure remains constant at 1 atm. Calculate the specific heat capacity of quartz according to this experiment. Be sure your answer is rounded to 2 significant digits. J g. °C x10 X S thermometer. insulated container water sample a calorimeter ? ola

If you combine 370.0 mL of water at 25.00 °C and 130.0 mL of water at 95.00 °C, what is the final temperature of the mixture? Use 1.00 g/mL as the density of water.

A chemical reaction takes place inside a flask submerged in a water bath. The water bath contains 9.80kg of water at 27.4°C . During the reaction 140.kJ of heat flows out of the flask and into the bath. Calculate the new temperature of the water bath. You can assume the specific heat capacity of water under these conditions is 4.18J·g−1·K−1 . Be sure your answer has the correct number of significant digits.

13.0 g of cream at 22.4 °C are added to an insulated cup containing 150.0 g of coffee at 81.3 °C. Calculate the equilibrium temperature of the coffee. You may assume no heat is lost to the cup or surroundings, and that any physical properties of cream and coffee you need are the same as those of water. Be sure your answer has 3 significant digits. °C Xx10 X

A 47.0-g sample of copper at 99.3 °C is dropped into a beaker containing 158 g of water at 18.2 °C. What is the final temperature when thermal equilibrium is reached? (The specific heat capacities of liquid water and copper are 4.184 J/g ⋅ K and 0.385 J/g ⋅ K, respectively.)

If 30.5 g of LiBr are dissolved 350.0 g of water at 20.0 °C in an insulated container, a temperature change is observed. The Δ H of solution of LiBr is -48.8 kJ/mol. Assuming that the specific heat of the solution is 4.184 J/(g C) and that no heat is gained or lost by the container, what will be the final temperature of the solution?

A total of 2.00 mol of a compound is allowed to react with water in a foam coffee cup and the reaction produces 156 g of solution. The reaction caused the temperature of the solution to rise from 21.00 to 24.70 degrees Celsius. What is the enthalpy of this reaction? Assume that no heat is lost to the surroundings or to the coffee cup itself and that the specific heat of the solution is the same as that of pure water. Enter your answer in kilojoules per mole of compound to three significant figures.