Review I Constants I Periodic TablePart AIn the following experiment, a coffee-cup calorimeter containing 100 mL of H, 0 is used. The initial temperature of thecalorimeter is 23.0 °C. If 3.50 g of CaCl, is added to the calorimeter, what will be the final temperature of the solution inthe calorimeter? The heat of solution AHoln of CaCl, is -82.8 kJ/mol.Assume that the specific heat of the solution formed in the calorimeter is the same as that for pure water: C, = 4.184J/g °C.Express your answer with the appropriate units.> View Available Hint(s)HAValueUnitsSubmit< Return to AssignmentProvide Feedback

Answer:- This question is answered by suing the simple concept of calorimetry which states that heat…

Part A In the following experiment, a coffee-cup calorimeter containing 100 mL of H20 is used. The initial temperature of the calorimeter is 23.0 °C. If 3.50 g of CaCl, is added to the calorimeter, what will be the final temperature of the solution im the calorimeter? The heat of solution AH,oln of CaCl, is-82.8 kJ/mol. Assume that the specific heat of the solution formed in the calorimeter is the same as that for pure water: C, = 4.184 J/g °C. Express your answer with the appropriate units. > View Availlable Hint(s)

Part A In the following experiment, a coffee-cup calorimeter containing 100 mL of H20 is used. The initial temperature of the calorimeter is 23.0 °C. If 3.50 g of CaCl, is added to the calorimeter, what will be the final temperature of the solution im the calorimeter? The heat of solution AH,oln of CaCl, is-82.8 kJ/mol. Assume that the specific heat of the solution formed in the calorimeter is the same as that for pure water: C, = 4.184 J/g °C. Express your answer with the appropriate units. > View Availlable Hint(s)

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter4: Energy And Chemical Reactions

Section4.8: Measuring Reaction Enthalpies: Calorimetry

Problem 4.10PSP

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Small amounts of oxygen gas can be prepared in the laboratory by decomposing potassium chlorate with heat. A by-product of the decomposition is potassium chloride. When one mole of potassium chlorate decomposes, 44.7 kJ are evolved. (a) Write a balanced thermochemical equation for the decomposition of one mole of potassium chlorate. (b) Is the reaction exothermic? (c) Draw an energy diagram showing the path of this reaction. (Figure 8.6 is an example of such an energy diagram.) (d) What is H when 3.00 g of potassium chlorate decompose? (e) How many grams of potassium chlorate need to be decomposed to liberate fifteen kilojoules of heat?
When one mole of nitroglycerine, C3H5(NO3)3(l) decomposes, nitrogen, oxygen, carbon dioxide, and liquid water are formed. The decomposition liberates 5725 kJ of heat. (a) Write a balanced thermochemical equation for the reaction. (b) Using Table 8.3, calculate Hf for nitroglycerine.
Hydrogen cyanide is used in the manufacture of clear plastics such as Lucite and Plexiglas. It is prepared from ammonia and natural gas (CH4). 2NH3(g)+3O2(g)+2CH4(g)2HCN(g)+6H2O(g) The reaction evolves 469 kJ of heat per mol of HCN formed. Is the reaction endothermic or exothermic? What is the value of q when 2 mol HCN forms?
When one mole of calcium carbonate reacts with ammonia, solid calcium cyanamide, CaCN2, and liquid water are formed. The reaction absorbs 90.1 kJ of heat. (a) Write a balanced thermochemical equation for the reaction. (b) Using Table 8.3, calculate Hf for calcium cyanamide.
Given the following data 2ClF(g)+O2(g)Cl2O(g)+F2O(g)H=167.4KJ2ClF3(g)+2O2(g)Cl2O(g)+3F2O(g)H=341.4KJ2F2(g)+O2(g)2F2O(g)H=43.4KJ Calculate H for the reaction ClF(g)+F2(g)ClF3(g)
9.55 Hydrogen gas will react with either acetylene or ethylene gas. The thermochemical equations for these reactions are provided below. Write the thermochemical equation for the conversion of acetylene into ethylene by hydrogen gas. C2H2(g)+2H2(g)C2H6 H= -311 kJ C2H4(g)+H2(g)C2H6 H = -136 kJ
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.)
The bomb calorimeter in Exercise 102 is filled with 987 g water. The initial temperature of the calorimeter contents is 23.32C. A 1.056-g sample of benzoic acid (Ecomb = 26.42 kJ/g) is combusted in the calorimeter. What is the final temperature of the calorimeter contents?
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.
Nitroglycerin, C3H5(NO3)3(l), is an explosive most often used in mine or quarry blasting. It is a powerful explosive because four gases (N2, O2, CO2, and steam) are formed when nitroglycerin is detonated. In addition, 6.26 kJ of heat are given off per gram of nitroglycerin detonated. (a) Write a balanced thermochemical equation for the reaction. (b) What is H when 4.65 mol of products are formed?
Examine the experimental data below: 1st type of unknown metal Mass of cup and water: 170.54 g Mass of cup: 6.83 g Initial temperature of water: 24.0OC Final temperature of water: 26. 0OC Mass of unknown metal: 21.95g Initial temperature of unknown metal: 100.0OC Final temperature of unknown metal: 26.0OC Questions: 1. Calculate the heat gained by the water in the calorimeter. Note that the temperature of the cup did not change. 2. Calculate the specific heat of the unknown metal, using the heat gained=-heat lost equation. 3. Look up for the list of specific heat values of some metals in the internet. Compare your experimental specific heat value to other metals’ specific heat. What do you think is the name of the unknown metal?
Hydrogen gas and oxygen gas release 482.6 kJ of heat when they combine to form steam. Is this reaction endothermic or exothermic? In which direction does heat transfer (between system and the surroundings) for this reaction? Is ΔH for this reaction positive or negative? topic: enthalphy of reaction