3✓ 14✓ 15✓ 16✓ 17✓ 18192021✓ 22✓ 23IIIReview Homework REQUIRED (NOT Pie Progress)Question 20 of 46 (2 points) | Question Attempt: 1 of UnlimitedCalculate the energy required to heat 173.0 g of graphite from -0.6 °C to 16.1 °C. Assume the specific heat capacity of graphite under these conditions is0.710 J.g K. Round your answer to 3 significant digits.ロ・ロμ号5

Step 1: We know that, q=mCdT T2=16.1+273=289.1KT1=−0.6+273=272.4K =>q=mC(T2−T1)…

Answered: 3 ✓ 14 ✓ 15 ✓ 16 ✓ 17 ✓ 18 19 20 21 ✓…

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter8: Thermochemistry

Section: Chapter Questions

Problem 65QAP: Natural gas companies in the United States use the therm as a unit of energy. One therm is 1105 BTU....

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Similar questions

Natural gas companies in the United States use the therm as a unit of energy. One therm is 1105 BTU. (a) How many joules are in one therm? (1J=9.48104BTU) (b) When propane gas, C3H8, is burned in oxygen, CO2 and steam are produced. How many therms of energy are given off by 1.00 mol of propane gas?
Ethyl alcohol, C2H5OH, is the intoxicating agent in liquor. Burning 1.00 g of ethyl alcohol in an excess of oxygen at 23.28C and constant volume releases 29.52 kJ of heat. When 7.40 g of ethyl alcohol is burned in oxygen under the same conditions in a bomb calorimeter, the temperature of the bomb and water rises from 23.28C to 48.04C. The bomb holds 0.750 kg of water. (a) What is q for the combustion of the ethyl alcohol in the bomb calorimeter? (b) What is qH2O? (c) What is qcal? (d) What is the heat capacity of the calorimeter?
A 45-g aluminum spoon (specific heat 0.88 J/g C) at 24 C is placed in 180 mL (180 g) of coffee at 85 C and the temperature of the two become equal. (a) What is the final temperature when the two become equal? Assume that coffee has the same specific heat as water. (b) The first time a student solved this problem she got an answer of 88 C. Explain why this is clearly an incorrect answer.
The complete combustion of acetylene, C2H2(g), produces 1300. kJ of energy per mole of acetylene consumed. How many grams of acetylene must be burned to produce enough heat to raise the temperature of 1.00 gal water by 10.0c if the process is 80.0% efficient? Assume the density of water is 1.00 g/cm3
The “Chemistry in Focus” segment Nature Has Hot Plants discusses thermogenic, or heat-producing, plants. For some plants, enough heat is generated to increase the temperature of the blossom by 15 °C. About how much heat is required to increase the temperature of 1 L of water by 15 °C?
Acetic acid, HC2H3O2, is responsible for the sour taste of vinegar. Combustion of acetic acid gives off 14.52 kJ/g of heat. When 15.00 g of acetic acid is burned in a bomb calorimeter (heatcapacity=2.166kJ/C) containing 0.800 kg of water, the final temperature in the calorimeter is 64.14C. What was the initial temperature of the calorimeter?
9.90 Many engineering designs must incorporate ways to dissipate energy in the form of heat. Water evaporators are common for this task. (a) What property of water makes it a good material for evaporators? {b} If an application could not use water, hut instead was forced to use a material with a value for the property in part (a) that was one half that of water, what changes would need to be made in the design?
In the 1880s, Frederick Trouton noted that the enthalpy of vaporization of 1 mol pure liquid is approximately 88 times the boiling point, Tb, of the liquid on the Kelvin scale. This relationship is called Troutons rule and is represented by the thermochemical equation liquid gas H = 88 Tb, joules Combined with an empirical formula from chemical analysis, Troutons rule can be used to find the molecular formula of a compound, as illustrated here. A compound that contains only carbon and hydrogen is 85.6% C and 14.4% H. Its enthalpy of vaporization is 389 J/g, and it boils at a temperature of 322 K. (a) What is the empirical formula of this compound? (b) Use Troutons rule to calculate the approximate enthalpy or vaporization or one mole of the compound. Combine the enthalpy of vaporization per mole with that same quantity per gram to obtain an approximate molar mass of the compound. (c) Use the results of parts (a) and (b) to find the molecular formula of this compound. Remember that the molecular mass must be exactly a whole-number multiple of the empirical formula mass, so considerable rounding may be needed.
In the “Chemistry in Focus” segment Firewalking: Magic or Science?, it is claimed that one reason people can walk on hot coals is that human tissue is mainly composed of water. Because of this, a large amount of heat must be transferred from the coals to change the temperature of the feet significantly. How much heat must be transferred to 100.0 g of water to change its temperature by 35 °C?
Consider the following statements: ''Heat is a form of energy, and energy is conserved. The heat lost by a system must be equal to the amount of heat gained by the surroundings. Therefore, heat is conserved." Indicate everything you think is correct in these statements. Indicate everything you think is incorrect. Correct the incorrect statements and explain.
A 244-g amount of coffee in an open plastic cup cools from 80.0C to 20.0C. Assuming no loss of mass and a heat capacity of liquid water, determine w, q, U, and H for the process. The densities of water are dH2O, 80.0C = 0.9718g/cm3 and dH2O, 20.0C =0.9982 g/cm3.
How much heat, in joules and in calories, must be added to a 75.0g iron block with a specific heat of 0.449 Jig C to increase its temperature from 25 C to its melting temperature of 1535 C?

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