Carbon disulfide burns in air, producing carbon dioxide and sulfur dioxide.CS2 (1) + 302 (9) CO2(g) + 2SO2(g); AH = -1.077 x 10° kJWhat is AH for the following equation?CO () + SO2 (9) → CS,(1) +02(9)ptptCS2pt1 ptΔΗkJ1 ptSubmit AnswerTry Another Version6 item attempts remaining1 pt1 pt1 pt1 pt1 pt1 pt1 pt1 pt1 pt1 pt

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Carbon disulfide burns in air, producing carbon dioxide and sulfur dioxide. CS2 (1) +302(g) CO2 (9) + 2SO2(g); AH = -1.077 x 10° kJ What is AH for the following equation? Co2(9) + SO2 (9) → CS (1) +02(9) CS2 AH kJ

Carbon disulfide burns in air, producing carbon dioxide and sulfur dioxide. CS2 (1) +302(g) CO2 (9) + 2SO2(g); AH = -1.077 x 10° kJ What is AH for the following equation? Co2(9) + SO2 (9) → CS (1) +02(9) CS2 AH kJ

EBK A SMALL SCALE APPROACH TO ORGANIC L

4th Edition

ISBN:9781305446021

Author:Lampman

Publisher:Lampman

Chapter26: Biodiesel

Section: Chapter Questions

Problem 2Q

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9.85 The figure below shows a "self-cooling" beverage can. The can is equipped with an outer jacket containing sodium carbonate (Na2CO3), which dissolves in water rapidly and endothermically: Na2CO3(s)2Na+(aq)+CO32(aq) H= 67.7 kJ The user adds water to the outer jacket, and the heat absorbed in the chemical reaction chills the drink. The can contains 200 g of drink, the jacket contains 55 g of Na2CO3, and 100 g of water is to be added. If the initial temperatures of the can and the water are both 32°C on a summer day, what is the coldest temperature that the drink can reach? The can itself has a heat capacity of 40 J/C Assume that the Na2CO3 solution and the drink both have the same heat capacity as pure water, 4.184 J g-l C-l, (HINT: Treat this like a calorimetry problem.)
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?
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.
You have the six pieces of metal listed below, plus a beaker of water containing 3.00 102 g of water. The water temperature is 21.00 C. (a) In your first experiment you select one piece of metal and heat it to 100 C, and then select a second piece of metal and cool it to 10 C. Both pieces of metal are then placed in the beaker of water and the temperatures equilibrated. You want to select two pieces of metal to use, such that the final temperature of the water is as high as possible. What piece of metal will you heat? What piece of metal will you cool? What is the final temperature of the water? (b) The second experiment is done in the same way as the first. However, your goal now is to cause the temperature to change the least, that is, the final temperature should be as near to 21.00 C as possible. What piece of metal will you heat? What piece of metal will you cool? What is the final temperature of the water?
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.
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