A 53.5 g sample of glass is put into a calorimeter (see sketch at right) that contains 200.0 g of water. The glass sample starts off at 89.2 °C and the temperature of the water starts off at 22.0 °C. When the temperature of the water stops changing it's 25.0 °C. The pressure remains constant at 1 atm. Calculate the specific heat capacity of glass according to this experiment. Be sure your answer is rounded to 2 significant digits. J 0,C g. °C insulated container water sample. a calorimeter

A 53.5 g sample of glass is put into a calorimeter (see sketch at right) that contains 200.0 g of water. The glass sample starts off at 89.2 °C and the temperature of the water starts off at 22.0 °C. When the temperature of the water stops changing it's 25.0 °C. The pressure remains constant at 1 atm. Calculate the specific heat capacity of glass according to this experiment. Be sure your answer is rounded to 2 significant digits. J 0,C g. °C insulated container water sample. a calorimeter

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

Chapter6: Thermochemistry

Section: Chapter Questions

Problem 63E: A 150.0-g sample of a metal at75.0C is added to 150.0 g H2O at 15.0C. The temperature of the water...

See similar textbooks

Similar questions

The specific heat capacity of copper is 0.385 J g1 C1, whereas it is 0.128 J g1 C1 for gold. Assume you place 100. g of each metal, originally at 25 C, in a boiling water bath at 100 C. If energy is transferred to each metal at the same rate, determine which piece of metal will reach 100 C first.
If 125 J of heat energy is applied to a block of silver weighing 29.3 g, by how many degrees will the temperature of the silver increase? (See Table 10.1.)
A sample of nickel is heated to 99.8C and placed in a coffee-cup calorimeter containing 150.0 g water at 23.5C. After the metal cools, the final temperature of metal and water mixture is 25.0C. If the specific heat capacity of nickel is 0.444 J/C g, what mass of nickel was originally heated? Assume no heat loss to the surroundings.
You drink 350 mL of diet soda that is at a temperature of 5 C. (a) How much energy will your body expend to raise the temperature of this liquid to body temperature (37 C)? Assume that the density and specific heat capacity of diet soda are the same as for water. (b) Compare the value in part (a) with the caloric content of the beverage. (The label says that it has a caloric content of 1 Calorie.) What is the net energy change in your body resulting from drinking this beverage? (1 Calorie = 1000 kcal = 4184 J.) (c) Carry out a comparison similar to that in part (b) for a nondiet beverage whose label indicates a caloric content of 240 Calories.
A 0.470-g sample of magnesium reacts with 200 g dilute HCl in a coffee-cup calorimeter to form MgCl2(aq) and H2(g). The temperature increases by 10.9 C as the magnesium reacts. Assume that the mixture has the same specific heat as water and a mass of 200 g. (a) Calculate the enthalpy change for the reaction. Is the process exothermic or endothermic? (b) Write the chemical equation and evaluate H.
A sample of 0.562 g of carbon is burned in oxygen in a bomb calorimeter, producing carbon dioxide. Assume both the reactants and products are under standard state conditions, and that the heat released is directly proportional to the enthalpy of combustion of graphite. The temperature of the calorimeter increases from 26.74 C to 27.93 C. What is the heat capacity of the calorimeter and its contents?
The internal energy of a gas decreases by 1.65 kJ when it transfers 1.87 kJ of energy in the form of heat to the surroundings. (a) Calculate the work done by the gas on the surroundings. (b) Does the volume of gas increase or decrease?
Which of the following substances have an enthalpy of formation equal to zero? a. Cl2(g) b. H2(g) c. N2(l) d. Cl(g)
Calculate Suppose that two pieces of iron, one with amass exactly twice the mass of the other, are placed in aninsulated calorimeter. If the original temperatures of thelarger piece and the smaller piece are 90.0°C and 50.0°C,respectively, what is the temperature of the two pieceswhen thermal equilibrium has been established? Referto Table R-9 on page 975 for the specific heat of iron.
A 150.0-g sample of a metal at75.0C is added to 150.0 g H2O at 15.0C. The temperature of the water rises to 18.3C. Calculate the specific heat capacity of the metal, assuming that all the heat lost by the metal is gained by the water.
When solid iron burns in oxygen gas (at constant pressure) to produce Fe2O3(s), 1651 kJ of heat is released for every 4 mol of iron burned. How much heat is released when 10.3 g Fe2O3(s) is produced (at constant pressure)? What additional information would you need to calculate the heat released to produce this much Fe2O3(s) if you burned iron in ozone gas, O3(g), instead of O2(g)?
Consider a mixture of air and gasoline vapor in a cylinder with a piston. The original volume is 40. cm3. If the combustion of this mixture releases 950. J of energy, to what volume will the gases expand against a constant pressure of 650. torr if all the energy of combustion is converted into work to push back the piston?