3.0 g of cream at 12.7 °C are added to an insulated cup containing 100.0 g of coffee at 80.3 °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 the correct number of significant digits. °C X S

3.0 g of cream at 12.7 °C are added to an insulated cup containing 100.0 g of coffee at 80.3 °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 the correct number of significant digits. °C X S

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

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 chemist carefully measures the amount of heat needed to raise the temperature of a 1.10kg sample of a pure substance from −6.3°C to 10.7°C . The experiment shows that 8.40kJ of heat are needed. What can the chemist report for the specific heat capacity of the substance? Be sure your answer has the correct number of significant digits.
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?
14.0 g of cream at 20.3 °C are added to an insulated cup containing 100.0 g of coffee at 78.8 °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 S
The temperature of the cooling water as it leaves the hot engine of an automobile is 240 °F. After it passes through the radiator it has a temperature of 175 °F. Calculate the amount of heat transferred from the engine to the surroundings by 10 grams of water with a specific heat of 4.184 J/g °C.
Expressing amounts of energy in different energy units is necessary to solve many chemistry problems. For practice, complete the following table. The Joule (J) is the SI unit of energy. 1 calorie (cal) = 4.184 J J cal kJ 549 197 0.806
A chemical reaction takes place inside a flask submerged in a water bath. The water bath contains 8.40 kg of water at 25.0 °C. During the reaction 97.5 kJ of heat flows out of the flask and into the bath. - 1 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 ·K'. Round your answer to 3 significant digits. x10 ?
A chemical reaction takes place inside a flask submerged in a water bath. The water bath contains 9.80kg of water at 34.0°C . During the reaction 139.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−1K−1 . Be sure your answer has the correct number of significant digits. °C