A 40.0 g sample of glass, which has a specific heat capacity of 0.670 J.g.°C', is dropped into an insulated container containing 200.0 g of water at 50.0 °C and a constant pressure of 1 atm. The initial temperature of the glass is 2.6 °C. Assuming no heat is absorbed from or by the container, or the surroundings, calculate the equilibrium temperature of the water. Be sure your answer has 3 significant digits.

A 40.0 g sample of glass, which has a specific heat capacity of 0.670 J.g.°C', is dropped into an insulated container containing 200.0 g of water at 50.0 °C and a constant pressure of 1 atm. The initial temperature of the glass is 2.6 °C. Assuming no heat is absorbed from or by the container, or the surroundings, calculate the equilibrium temperature of the water. Be sure your answer has 3 significant digits.

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

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
A 60.0 g sample of iron is put into a calorimeter (see sketch at right) that contains 300.0 g of water. The iron sample starts off at 98.3 °C and the temperature of the water starts off at 22.0 °C. When the temperature of the water stops changing it's 24.1 °C. The pressure remains constant at 1 atm. Calculate the specific heat capacity of iron according to this experiment. Be sure your answer is rounded to the correct number of significant digits. 0 J g. °C x10 X thermometer insulated container water sample. a calorimeter
A 56.2 g sample of aluminum, which has a specific heat capacity of 0.897 J-g¹C¹, is put into a calorimeter (see sketch at right) that contains 250.0 g of water. The temperature of the water starts off at 24.0 °C. When the temperature of the water stops changing it's 26.9 °C. The pressure remains constant at 1 atm. Calculate the initial temperature of the aluminum sample. Be sure your answer is rounded to the correct number of significant digits. °C X Ś thermometer- insulated. container water sample a calorimeter
thermometer- A 56.5 g sample of iron is put into a calorimeter (see sketch at right) that contains 250.0 g of water. The iron sample starts off at insulated container 89.3 °C and the temperature of the water starts off at 17.0 °C. When the temperature of the water stops changing it's 19.2 °C. The pressure remains constant at l atm. water Calculate the specific heat capacity of iron according to this experiment. Be sure your answer is rounded to the correct number of significant digits. sample a calorimeter
thermometer. insulated container A sample of quartz, which has a specific heat capacity of 0.730 J-goC, is put into a calorimeter (see sketch at right) that contains 300.0 g of water. The quartz sample starts off at 90.0 °C and the temperature of the water starts off at 25.0 °C. When the temperature of the water stops changing it's 27.1 °C. The pressure remains constant at 1 atm. water Calculate the mass of the quartz sample. Be sure your answer is rounded to 2 significant digits. 0 x10 X ? a sample a calorimeter do F
thermometer. A sample of aluminum, which has a specific heat capacity of 0.897 J·g *.°C*, is put into a calorimeter (see sketch at right) that insulated container contains 100.0 g of water. The aluminum sample starts off at 91.4 °C and the temperature of the water starts off at 19.0 °C. When the temperature of the water stops changing it's 26.9 °C. The pressure remains constant at 1 atm. water Calculate the mass of the aluminum sample. Be sure your answer is rounded to 2 significant digits. sample a calorimeter x10
A 56.5 g sample of iron is put into a calorimeter (see sketch at right) that contains 300.0 g of water. The iron sample starts off at 86.7 °C and the temperature of the water starts off at 21.0 °C. When the temperature of the water stops changing it's 22.8 °C. The pressure remains constant at 1 atm. Calculate the specific heat capacity of iron according to this experiment. Be sure your answer is rounded to 2 significant digits. J 0₂-C x10 x thermometer insulated container water sample a calorimeter
A 54.5 g sample of brass is put into a calorimeter (see sketch at right) that contains 300.0 g of water. The brass sample starts off at 95.8 °C and the temperature of the water starts off at 15.0 °C. When the temperature of the water stops changing it's 16.4 °C. The pressure remains constant at 1 atm. Calculate the specific heat capacity of brass according to this experiment. Be sure your answer is rounded to 2 significant digits. П J g.°C x10 X S thermometer insulated container water sample a calorimeter U!!! 0 C
In an experiment, a 0.5002 g sample of tridecanedioic acid ( C13 H24 O4) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.165 × 10³ g of water. During the combustion the temperature increases from 21.99 to 24.52 °C. The heat capacity of water is 4.184 J·g¯¹. °C-¹. The heat capacity of the calorimeter was determined in a previous experiment to be 904.0 J. °C¯¹. Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of tridecanedioic acid based on these data. C13H24 O4(s) + 17O2 (g) → 12H₂O(l) + 13CO2 (g) + Energy kJ/mol Molar Heat of Combustion =
Measurements show that the enthalpy of a mixture of gaseous reactants increases by 195.kJ during a certain chemical reaction, which is carried out at a constant pressure. Furthermore, by carefully monitoring the volume change it is determined that 69.kJ of work is done on the mixture during the reaction. Calculate the change in energy of the gas mixture during the reaction. Be sure your answer has the correct number of significant digits. Is the reaction exothermic or endothermic?
finding equilbrilium stion 12.0g of cream at 18.9°C are added to an insulated cup containing 100.0g of coffee at 90.7°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.
14.0 g of cream at 15.5 °C are added to an insulated cup containing 100.0 g of coffee at 70.1 °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. ?