thermometer-A 51.9 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 atinsulatedcontainer85.7 °C and the temperature of the water starts off at 15.0 °C. When the temperature of the water stops changing it's 16.7 °C. Thepressure remains constant at 1 atm.waterCalculate the specific heat capacity of iron according to this experiment. Be sure your answer is rounded to 2 significant digits.samplea calorimeterg.°CContinueSubmit AssignmentO 2021 McGraw Hill LLC. A Rights Reserved. Terms of UseI Privacy Center AccessibilityDELL

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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 100AE

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A 5.00-g sample of aluminum pellets (specific heat capacity = 0.89 J/C g) and a 10.00-g sample of iron pellets (specific heat capacity = 0.45 J/C g) are heated to 100.0C. The mixture of hot iron and aluminum is then dropped into 97.3 g water at 22.0C. Calculate the final temperature of the metal and water mixture, assuming no heat loss to the surroundings.
9.100 Two baking sheets are made of different metals. You purchase both and bake a dozen cookies on each sheet at the same time in your oven. You observe that after 9 minutes, the cookies on one sheet are slightly burned on the bottom, whereas those on the other sheet are fine. (You are curious and you vary the conditions so you know the result is not caused by the oven.) (a) How can you use this observation to infer something about the specific heat of the materials in the baking sheets? (b) What is themathematical reasoning (equation) that you need to support your conclusion?
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?
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?
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.
Indicate which state function is equal to heat, q, for each process described. a. The ignition of a sample in a bomb calorimeter, an unyielding, heavy metal chamberin which samples are burned for heat content analysis b.The melting of an icecube in a cup c.The cooling down ofthe inside of arefrigerator d.A fire in a fireplace
When a 0.740-g sample of trinitrotoluene (TNT), C7H5N2O6, is burned in a bomb calorimeter, the temperature increases from 23.4 C to 26.9 C. The heat capacity of the calorimeter is 534 J/C, and it contains 675 mL of water. How much heat was produced by the combustion of the TNT sample?
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.
A7.50-gpiece of iron at 100.0C is dropped into 25.0g of water at 22.0C. Assuming that the heat lost by the iron equals the heat gained by the water,determine thefinal temperature of the iron/watersystem. Assume a heat capacity of water at 4.18 J/g.K and of iron at 0.452J/g.K.

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