Ignition wires heat Thermometer A bomb calorimeter, or constant volume calorimeter, is a device often used to determine the heat of combustion of fuels Stirrer and the energy content of foods. sample Since the "bomb" itself can absorb energy, a separate experiment is needed to determine the heat capacity of the calorimeter. This is known as calibrating the calorimeter. Water In the laboratory a student burns a 0.520-g sample of 1,6- hexanediol (C,H1402) in a bomb calorimeter containing 1090. g of water. The temperature increases from 24.30 °C to 27.40 °C. The heat capacity of water is 4.184 J glºC¯!. The molar heat of combustion is –3792 kJ per mole of 1,6- hexanediol. C,H1402(s) + 17/2 O2(g) →6 CO2(g) + 7 H,O(1) + Insulated outside chamber Sample dish Burning sample Steel bomb Energy Calculate the heat capacity of the calorimeter. J/°C Combustion (bomb) calorimeter. heat capacity of calorimeter =

Ignition wires heat Thermometer A bomb calorimeter, or constant volume calorimeter, is a device often used to determine the heat of combustion of fuels Stirrer and the energy content of foods. sample Since the "bomb" itself can absorb energy, a separate experiment is needed to determine the heat capacity of the calorimeter. This is known as calibrating the calorimeter. Water In the laboratory a student burns a 0.520-g sample of 1,6- hexanediol (C,H1402) in a bomb calorimeter containing 1090. g of water. The temperature increases from 24.30 °C to 27.40 °C. The heat capacity of water is 4.184 J glºC¯!. The molar heat of combustion is –3792 kJ per mole of 1,6- hexanediol. C,H1402(s) + 17/2 O2(g) →6 CO2(g) + 7 H,O(1) + Insulated outside chamber Sample dish Burning sample Steel bomb Energy Calculate the heat capacity of the calorimeter. J/°C Combustion (bomb) calorimeter. heat capacity of calorimeter =

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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A 6.61g sample of an unknown salt (MM=116.82g//mol) is dissolved in 150.00g water in a coffee cup calorimeter. Before placing the sample in the water, the temperature of the salt and water is 23.72 C. After the salt has completely dissolved, the temperature of the solution is 28.54 C. Given that 156.61 g of solution increased in temperature by 4.82 °C, what quantity of heat, in J, was gained by the solution? Assume the specific heat of the solution is the same as water, 4.184 J/g• °C.
The heat released when one mole of water is formed from the elements is 1,198 kJ. An experiment was conducted that permitted water to form in this manner, and the heat was contained in 2.0 liters of water. The water temperature before the reaction was 34.5°C, and after the reaction it had risen to 52.0°C. How many moles of water were formed? (The specific heat of water is 4.184 J/g·°C.)Answer: 0.12 mole (Can you explain how?)
6. Determine the mass of a sample of water in a coffee cup calorimeter if the final temperature is 65.7 °C, the initial temperature is 22.3 °C, and 27.6 kJ of heat is added to the water (specific heat of water is 4.184 J/g•K).
3. A 74.5 g piece of metal at 86.0°C is placed in 133 g of water at 21.0°C contained in a calorimeter. The metal and water come to the same temperature at 24.2°C. How much heat (in J) did the metal give up to the water? (Assume the specific heat of water is 4.18 J/g·°C across the temperature range.) J What is the specific heat (in J/g·°C) of the metal? J/g·°C 4. A 0.528 g sample of KCl is added to 51.7 g of water in a calorimeter. If the temperature decreases by 1.07°C, what is the approximate amount of heat (in J) involved in the dissolution of the KCl, assuming the heat capacity of the resulting solution is 4.18 J/g°C? J Is the reaction exothermic or endothermic? exothermicendothermic 5. When 2.56 g of methane burns in oxygen, 128 kJ of heat is produced. What is the enthalpy of combustion (in kJ) per mole of methane under these conditions? kJ/mol methane 6. Joseph Priestly prepared oxygen in 1774 by heating red mercury(II) oxide with sunlight focused through a lens. How much…
1 A piece of metal with a specific heat of 1.011 J/gºC is heated to 123.1ºC and then placed in 111.031 g of water which is at a temperature of 3.6 ºC. After a minute, the temperature of the water has stopped changing and is now 55.8ºC. Assuming that there are no heat losses to the container or surroundings, what is the mass of the piece of metal in grams? Assume that water has a specific heat of 4.184 J/gºC. Enter your answer with at least 3 sig figs.
2 moles of lithium metal reacts with liquid water to produce solid lithium hydroxide, hydrogen gas, and 402.4 kJ/mol of heat energy. a) write a balanced thermochemical equation for the reaction b) how much heat would be produced by the reaction of 14 g of lithium with an excess of liquid water c) is the reaction endothermic or exothermic?
Alexia determined the mass of her empty Styrofoam cup calorimeter was 1.0698 g. She then added distilled water to the cup and weighed it again. The combined mass of the cup + water was 33.2191 g. What is the mass of water, in g, in Alexia's cup?
1. A thermometer placed in a solution undergoing a chemical reaction indicates an increase in temperature as the reaction proceeds. Is this reaction endothermic or exothermic? Describe if heat energy is lost or gained from the reaction (the system) to the surroundings. What is the sign of the enthalpy change (AH) of this reaction? 2. A student performs a reaction and determines the enthalpy change (AH) to be 31.4 kJ. Will the temperature of the surrounding solution increase or decrease as a result of this chemical process? 3. If you hold 3 grams of ice in your hand at room temperature, your hand will become cold. a) Is the reaction H,O(s) – H,O(1) endothermic or exothermic? b) In which direction does heat flow?
In order to break water into hydrogen and oxygen, water is heated to more than 500°C. Which kind of reaction is this and why? It is exothermic because heat needs to be released by the reactants to form the products. It is endothermic because heat needs to be released by the reactants to form the products It is exothermic because heat needs to be absorbed by the reactants to form the products. It is endothermic because heat needs to be absorbed by the reactants to form the products.
A 7.37 g sample of an unknown salt (MM = 116.82 g/mol) is dissolved in 150.00 g water in a coffee cup calorimeter. Before placing the sample in the water, the temperature of the salt and water is 23.72°C. After the salt has completely dissolved, the temperature of the solution is 28.54°C. What quantity in moles of the unknown salt were used in the reaction?
How much heat is released when 22.75 g oxygen gas is used in the reaction? (Pay close attention to the units your given is in! Maybe need a conversion first?) 4 Fe+ 3 O2 → 2 Fe2O3 ΔH = -1652 kJ