O THERMOCHEMISTRYSolving a basic calorimetry problemthermometerA sample of polystyrene, which has a specific heat capacity of 1.880 J'g .°c', is put into a calorimeter (see sketch at right) thatcontains 300.0 g of water. The polystyrene sample starts off at 96.4 °C and the temperature of the water starts off at 16.0 °CinsulatedcontainerWhen the temperature of the water stops changing it's 22.2 °C. The pressure remains constant at 1 atm.waterCalculate the mass of the polystyrene sample. Be sure your answer is rounded to the correct number of significant digits.samplea calorimeterII

Answered: Image /qna-images/answer/01c0c475-30e0-47aa-9575-0b98deb6c3f7.jpg

thermometer -1.°c A sample of polystyrene, which has a specific heat capacity of 1.880 J'g contains 300.0 g of water. The polystyrene sample starts off at 96.4 °C and the temperature of the water starts off at 16.0 °C. When the temperature of the water stops changing it's 22.2 °C. The pressure remains constant at 1 atm. is put into a calorimeter (see sketch at right) that insulated container water Calculate the mass of the polystyrene sample. Be sure your answer is rounded to the correct number of significant digits. sample a calorimeter

thermometer -1.°c A sample of polystyrene, which has a specific heat capacity of 1.880 J'g contains 300.0 g of water. The polystyrene sample starts off at 96.4 °C and the temperature of the water starts off at 16.0 °C. When the temperature of the water stops changing it's 22.2 °C. The pressure remains constant at 1 atm. is put into a calorimeter (see sketch at right) that insulated container water Calculate the mass of the polystyrene sample. Be sure your answer is rounded to the correct number of significant digits. 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 61E: A 5.00-g sample of aluminum pellets (specific heat capacity = 0.89 J/C g) and a 10.00-g sample of...

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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.
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?
Nitrogen gas is confined in a cylinder with a movable piston under a constant pressure of 9.95 104 Pa. When 695 J of energy in the form of heat is transferred from the gas to the surroundings, its volume decreases by 1.88 L. What is the change in internal energy of the gas?
When 1.0 g of fructose, C6H12O6(s), a sugar commonly found in fruits, is burned in oxygen in a bomb calorimeter, the temperature of the calorimeter increases by 1.58 C. If the heat capacity of the calorimeter and its contents is 9.90 kJ/C, what is q for this combustion?
9.47 If 14.8 kJ of heat is given off when 1.6 g of HCl condenses from vapor to liquid, what is Hcond for this substance?
A 250-g sample of water at 20.0C is placed in a freezer that is held at a constant temperature of 20.0C. Considering the water as the system, answer the following questions: a What is the sign of qsys for the water after it is placed in the freezer? b After a few hours, what will be the state of the water? c How will the initial enthalpy for the water compare with the final enthalpy of the water after it has spent several hours in the freezer? d What will the temperature of the water be after several hours in the freezer?
9.57 The heat of combustion of butane is —2877 kJ/mol. Use this value to find the heat of formation of butane. (You may also need to use additional thermochemical data found in Appendix E.)
9.50 When a 13.0-g sample of NaOH(s) dissolves in 400.0 mL of water in a coffee cup calorimeter, the temperature of the water changes from 22.6°C to 30.7C Assuming that the specific heat capacity of the solution is the same as for water, calculate (a) the heat transfer from system to surroundings and (b) H for the reaction NaOH(s)Na+(aq)+OH(aq)
In earlier times, ethyl ether was commonly used as an anesthetic. It is, however, highly flammable. When five milliliters of ethyl ether, C4H10O(l)(d=0.714g/mL), are burned in a bomb calorimeter, the temperature rises from 23.5C to 39.7C. The calorimeter contains 1.200 kg of water and has a heat capacity of 5.32 kJ/C. (a) What is qH2o? (b) What is qcal? (c) What is q for the combustion of 5.00 mL of ethyl ether? (d) What is q for the combustion of one mole of ethyl ether?
When hydrazine reacts with oxygen, nitrogen gas and steam are formed. (a) Write a thermochemical equation for the reaction. (b) How much heat is evolved or absorbed if 1.683 L of steam at 125C and 772 mm Hg are obtained?
9.104 An engineer is using sodium metal as a cooling agent in a design because it has useful thermal properties. Looting up the heat capacity, the engineer finds a value of 28.2 J mol-l °C-l. Carelessly, he wrote this number down without units. As a result, it was later taken as specific heat. (a) What would he the difference between these two values? (b) Would the engineer overestimate the ability of sodium to remove heat from the system or underestimate it because of this error? Be sure to explain your reasoning.
Ammonium nitrate is an oxidizing agent and can give rise to explosive mixtures. A mixture of 2.00 mol of powdered aluminum and 3.00 mol of ammonium nitrate crystals reacts exothermically yielding nitrogen gas, water vapor, and aluminum oxide. How many grams of the mixture are required to provide 245 kJ of heat? See Appendix C for data.

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