LO A. Specific Heat of a Metal = 4184 x mass H2O Desk No. Unknown No. 1. Mass of metal (g) Trial 1 Trial 2 24.857 24, 2. Temperature of metal (boiling water) (°C) 3. Mass of calorimeter (g) 100 4. Mass of calorimeter + water (g) d2s.4749 231.027g 5. Mass of water (g) ne ol noh 6. Temperature of water in calorimeter (°C) HC) as0 7 Maximum temperature of metal and water from graph (°C) 30 8. Instructor's approval of graph Calculations for Specific Heat of a Metal 1. Temperature change of water, AT (°C) t 81A 5°C 2. Heat gained by water (J) 3. Temperature change of metal, AT (°C) Specific heat of metal, equation 25.5 (J/g •°C) Data Analysis, B Average specific heat of metal (J/g •°C) now calculations for Trial 1 using the correct number of significant figures. TO VAC Comancor ou Experiment 25 301 155

LO A. Specific Heat of a Metal = 4184 x mass H2O Desk No. Unknown No. 1. Mass of metal (g) Trial 1 Trial 2 24.857 24, 2. Temperature of metal (boiling water) (°C) 3. Mass of calorimeter (g) 100 4. Mass of calorimeter + water (g) d2s.4749 231.027g 5. Mass of water (g) ne ol noh 6. Temperature of water in calorimeter (°C) HC) as0 7 Maximum temperature of metal and water from graph (°C) 30 8. Instructor's approval of graph Calculations for Specific Heat of a Metal 1. Temperature change of water, AT (°C) t 81A 5°C 2. Heat gained by water (J) 3. Temperature change of metal, AT (°C) Specific heat of metal, equation 25.5 (J/g •°C) Data Analysis, B Average specific heat of metal (J/g •°C) now calculations for Trial 1 using the correct number of significant figures. TO VAC Comancor ou Experiment 25 301 155

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter7: Chemical Energy

Section: Chapter Questions

Problem 61E: A coffee-cup calorimeter initially contains 125 g water at 24.2C. Potassium bromide (10.5 g), also...

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When 50.0 g of 0.200 M NaCl(aq) at 24.1 C is added to 100.0 g of 0.100 M AgNO3(aq) at 24.1 C in a calorimeter, the temperature increases to 25.2 C as AgCl(s) forms. Assuming the specific heat of the solution and products is 4.20 J/g C, calculate the approximate amount of heat in joules produced.
Microwave ovens convert radiation to energy. A microwave oven uses radiation with a wavelength of 12.5 cm. Assuming that all the energy from the radiation is converted to heat without loss, how many moles of photons are required to raise the temperature of a cup of water (350.0 g, specific heat =4.18J/gC) from 23.0C to 99.0C?
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.
9.63 Reactions of hydrocarhons are often studied in the petroleum industry. One example is 2C3H8(g)C6H6(l)+5H2(g) , with H = 698 kJ. If 35 L of propane at 25C and 0.97 atm is to be reacted, how much heat must he supplied?
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?
9.37 A calorimeter contained 75.0 g of water at 16.95°C. A 93.3-g sample of iron at 65.58°C was placed in it, giving a final temperature of 19.68°C for the system. Calculate the heat capacity of the calorimeter. Specific heats are 4.184Jg1C1 for H2O and 0.444Jg1C1 for Fe.
In a coffee-cup calorimeter, 100.0 mL of 1.0 M NaOH and 100.0 mL of 1.0 M HCI are mixed. Both solutions were originally at 24.6C. After the reaction, the final temperature is 31.3C. Assuming that all the solutions have a density of 1.0 g/cm3 and a specific heat capacity of 4.18 J/Cg, calculate the enthalpy change for the neutralization of HCl by NaOH. Assume that no heat is lost to the surroundings or to the calorimeter.
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.
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)
A 237-g piece of molybdenum, initially at 100.0 C, is dropped into 244 g of water at 10.0 C. When the system comes to thermal equilibrium, the temperature is 15.3 C. What is the specific heat capacity of molybdenum?
Chlorine trifluoride is a toxic, intensely reactive gas. It was used in World War II to make incendiary bombs. It reacts with ammonia and forms nitrogen, chlorine, and hydrogen fluoride gases. When two moles of chlorine trifluoride react, 1196 kJ of heat are evolved. (a) Write a thermochemical equation for the reaction. (b) What is Hf for ClF3?
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?