PROBLEM SET (1); A calorimeter is to be used to compare the energy content of some fuels. In the calibration of the calorimeter, an electrical resistance heater supplies 100.0 J of heat and a temperature increase of 0.850°C is observed. Then 0.245 g of a particular fuel is burned in this same calorimeter, and the temperature increases by 5.23°C. What is the heat capacity of the calorimeter? O 117.65 J/°C 2.51 kJ/g 615 J -615 J QUESTION 2 1.1 Based from PROBLEM SET (1), what is the heat evolved by fuel, qfuel? O 117.65 J/°C 615 J -615 J 2.51 kJ/g QUESTION 3 1.2 Based from PROBLEM SET (1), what is the energy density (amount of energy liberated per gram of fuel burned) of this fuel? 118 J/g 117.65 J/°C 615 J/g 2.51 kJ/g

PROBLEM SET (1); A calorimeter is to be used to compare the energy content of some fuels. In the calibration of the calorimeter, an electrical resistance heater supplies 100.0 J of heat and a temperature increase of 0.850°C is observed. Then 0.245 g of a particular fuel is burned in this same calorimeter, and the temperature increases by 5.23°C. What is the heat capacity of the calorimeter? O 117.65 J/°C 2.51 kJ/g 615 J -615 J QUESTION 2 1.1 Based from PROBLEM SET (1), what is the heat evolved by fuel, qfuel? O 117.65 J/°C 615 J -615 J 2.51 kJ/g QUESTION 3 1.2 Based from PROBLEM SET (1), what is the energy density (amount of energy liberated per gram of fuel burned) of this fuel? 118 J/g 117.65 J/°C 615 J/g 2.51 kJ/g

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Ignition wires heat sample Thermometer Stirrer A bomb calorimeter, or a constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of foods. In an experiment, a 0.4059 g sample of 9,10-anthracenedione (C14H30,) is burned completely in a bomb calorimeter. The calorimeter is surounded by 1.116x10³ g of water. During the combustion the temperature increases from 22.76 to 25.09 °C. The heat capacity of water is 4.184 Jgl°c-!. Water The heat capacity of the calorimeter was determined in a previous experiment to be 965.5 J/°C. Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of 9,10-anthracenedione based on these data. C14HgO2(s) - 1502(g) 4 H20(1) + 14 CO,(g) - Energy Molar Heat of Combustion = kJ/mol Sample dish Burning sample Steel Insulated outside chamber bomb Combustion (bomb) calorimeter.
Thermochemistry and Stoichiometry
A 21.42g sample of an unknown metal was heated to 99.5ºC, and the added to 50.00g of water contained in a foam coffee cup. The initial temperature of the water was 20.5ºC, and the final temperature of the metal and water was 25.1ºC. The calorimeter constant for the coffee-cup calorimeter was 13.5 J/ºC. What was the specific heat of the metal? * the answer is 0.64 J/gºC, but I need to know how to get there
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The standard heat of formation, AH, is defined as the enthalpy change for the formation of one mole of substance from its constituent elements in their standard states. Thus, elements in their standard states have AH = 0. Heat of formation values can be used to calculate the enthalpy change of any reaction. Consider, for example, the reaction 2NO(g) + O2(g) = 2NO₂(g) with heat of formation values given by the following table: Substance ΔΗ (kJ/mol) 90.2 0 33.2 NO(g) O₂(g) NO₂(g) Then the standard heat of reaction for the overall reaction is AH AH (products) AH; (reactants) [2(90.2) +0] = 2(33.2) = -114 kJ Part A For which of the following reactions is AHn equal to AH; of the product(s)? You do not need to look up any values to answer this question. Check all that apply. ► View Available Hint(s) Li(s) + Cl₂(g) →LiCl(s) SO(g) + O₂(g) →SO2(g) S(s) + O₂(g) →SO₂ (g) SO3(g) → O₂(g) + SO2(g) Li(s) + Cl₂(1)→LiCl(s) 2Li(s) + Cl₂ (g)→2LiCl(s) Submit Constants I Periodic Table Part B
A 1.435g of Naphthalene (C10H8) was burned in Constant Volume Bomb Calorimeter. Consequently, temperature of the water rose from 20.17°C to 25.84°C. If the mass of water surrounding the calorimeter was exactly 2.0 X 103 kg and the heat capacity of the bob calorimeter was 1.80 Kj/°C, Calculate the molar heat of reaction (combustion) in KJ of Naphthalene.
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Phenol undergoes combustion in oxygen to produce carbon dioxide gas and liquid water. The standard heat of combustion of phenol, CH,OH(s), is -3054 kJ/mol. Given that AHÇ [CO2(g)] = -393.5 kJ/mol and AHS [H,O(1)] = -285.8 kJ/mol, what is the standard %3D enthalpy of formation of phenol? +164.4 kj/mol +328.8 kj/mol -164.4 kj/mol -328.8 kj/mol
In the laboratory a "coffee cup" calorimeter, or constant pressure calorimeter, is frequently used to determine the specific heat of a solid, or to measure the energy of a solution phase reaction.A chunk of lead weighing 19.61 grams and originally at 97.01 °C is dropped into an insulated cup containing 82.14 grams of water at 21.79 °C.The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.61 J/°C.Using the accepted value for the specific heat of lead (See the References tool), calculate the final temperature of the water. Assume that no heat is lost to the surroundings.
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You're tasked with verifying whether or not a platinum ring bought from an online store is indeed made of platinum. After checking that the ring is not plated, but a solid piece of metal, you test the specific heat using a calorimeter. You heat up the 15.00 g ring in a water bath which is brought to a boil for 15 minutes. Then, you quickly transfer the ring into your calorimeter which has 100.0 g of water initially at 21.00 degrees Celsius. The ring and the calorimeter equilibriate at a final temperature of 21.69 degrees Celsius. According to your calorimetric test and table 2, what is the identity of the metal in the ring? The specific heat of water is 4.184 J/ (g*C).
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