Ignition wires heat sample Water Stirrer Thermometer Insulated Sample Burning Steel outside dish sample bomb chamber Combustion (bomb) calorimeter. In an experiment, a 0.7264 g sample of isophthalic acid (C8H6O4) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.333 x 10³ g of water. During the combustion the temperature increases from 27.65 to 29.88 °C. The heat capacity of water is 4.184 J.g-¹. °C-¹. The heat capacity of the calorimeter was determined in a previous experiment to be 972.6 J. °C-¹. Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of isophthalic acid based on these data. C8 H6O4(s) + (15/2) O₂(g) → 3H₂O(l) + 8CO2 (g) + Energy kJ/mol Molar Heat of Combustion = Previous Next

Ignition wires heat sample Water Stirrer Thermometer Insulated Sample Burning Steel outside dish sample bomb chamber Combustion (bomb) calorimeter. In an experiment, a 0.7264 g sample of isophthalic acid (C8H6O4) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.333 x 10³ g of water. During the combustion the temperature increases from 27.65 to 29.88 °C. The heat capacity of water is 4.184 J.g-¹. °C-¹. The heat capacity of the calorimeter was determined in a previous experiment to be 972.6 J. °C-¹. Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of isophthalic acid based on these data. C8 H6O4(s) + (15/2) O₂(g) → 3H₂O(l) + 8CO2 (g) + Energy kJ/mol Molar Heat of Combustion = Previous Next

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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In the laboratory a "coffee cup" calorimeter, or constant pressure calorimeter, is frequently used to determine the specific heat of a solid, or to Thermometer measure the energy of a solution phase reaction. Stirring rod A student heats 65.13 grams of copper to 98.95 °C and then drops it into a cup containing 84.76 grams of water at 23.02 °C. She measures the final temperature to be 27.86 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.60 J/°C. Water- Assuming that no heat is lost to the surroundings calculate the specific heat of copper. Metal sample Specific Heat (Cu) = J/g°C. 2000 Thomson-BrooksCole
Ignition wires heat Thermometer Stirrer sample 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 1.0580 g sample of B-D-fructose (C6H12O6) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.284x103 g of water. During the combustion the temperature increases from 26.32 to 29.03 °C. The heat capacity of water is 4.184 J g °C. Water The heat capacity of the calorimeter was determined in a previous experiment to be 991.6 J/oC Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of B-D-fructose based on these data 6 H2O(I)6 CO2(g) Energy CH12O6(s)6O2(g) Insulated Sample dish Burning sample Steel bomb kJ/mol Molar Heat of Combustion outside chamber Combustion (bomb) calorimeter.
thermometer. insulated container A sample of quartz, which has a specific heat capacity of 0.730 J-goC, is put into a calorimeter (see sketch at right) that contains 300.0 g of water. The quartz sample starts off at 90.0 °C and the temperature of the water starts off at 25.0 °C. When the temperature of the water stops changing it's 27.1 °C. The pressure remains constant at 1 atm. water Calculate the mass of the quartz sample. Be sure your answer is rounded to 2 significant digits. 0 x10 X ? a sample a calorimeter do F
The enthalpy of combustion of isooctane (C8H18), one of the many hydrocarbons in gasoline is 5.45 × 103 kJ/mol. Calculate the enthalpy change per gram of isooctane and per liter of isooctane (d = 0.688 g/mL).
▾ Part A For a hypothetical reaction X(g) → Y(g), you are told that the enthalpy of Y(g) is greater than that of X(g). Which of the following statements is false? O The enthalpies of X(g) and Y(g) could both have negative values. O AH for the reaction is positive. O The reaction is endothermic. O On an enthalpy diagram, the line for Y(g) is below the line for X(g). Submit Provide Feedback Request Answer Next >
A Chemistry 1A student drops 105.0 grams of copper with an initial temperature of 95.4 °C into a coffee cup calorimeter containing 100.0 grams of water. The water in the calorimeter was initially at 23.5 °C before the copper was added. Assuming no heat is lost to the environment, what will be the final temperature (°C) of the water?
(please type answer no write by hand)
A chemist burned a sample of coal in a bomb calorimeter. Her results are below. Calorimeter's Heat Capacity 7.264 kJ/°C Mass of Coal Initial Temperature Final Temperature 0.100 g 22.07°C 25.37°C The sample of coal that the chemist placed in the bomb was dry but when she finished the test there was a small amount of water in the bomb. Where did this water come from and how does it affect her result? The water came from the water surrounding the bomb so her measured heat of combustion is for a closed system. The water was a product of combustion so her measured heat of combustion is for an open system. The water came from the water surrounding the bomb so her measured heat of combustion is for an open system. The water was a product of combustion so her measured heat of combustion is for a closed system.
Consider the following chemical reaction which produces nitric oxide from its constituent elements: N2 (g) + O2(g) → 2 NO (g) AH = 182.6 kJ/mol If nitrogen and oxygen were mixed and allowed to react under constant pressure conditions, which of the following statements must be true? Select as many answers as applicable however points will be deducted for incorrect guesses. ΔΗ = q This is an endothermic reaction The temperature of the surroundings would decrease The temperature of the surroundings would increase AH = AU
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?
A 52.0 g sample of quartz is put into a calorimeter (see sketch at right) that contains 300.0 g of water. The quartz sample starts off at 98.2 °C and the temperature of the water starts off at 19.0 °C. When the temperature of the water stops changing it's 21.3 °C. The pressure remains constant at 1 atm. Calculate the specific heat capacity of quartz according to this experiment. Be sure your answer is rounded to the correct number of significant digits. g.°C ? O
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 student heats 62.45 grams of platinum to 99.18 °C and then drops it into a cup containing 84.71 grams of water at 23.23 °C. She measures the final temperature to be 25.02 °C.The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.66 J/°C.Assuming that no heat is lost to the surroundings calculate the specific heat of platinum.