2.5 X Bb Quiz 8- Blackbox XYa SOLUTION: A per Xeploymentid=5735112480241329813180832311&eISBN=9781305862883&id=1774598910&snapshot!...Use the References to access important values if needed for this question.A bomb calorimeter, or a constant volume calorimeter, is a device often usedto determine the heat of combustion of fuels and the energy content of foods.In an experiment, a 0.3163 g sample of azulene (C1₁0Hg) is burnedcompletely in a bomb calorimeter. The calorimeter is surrounded by1.061x10³ g of water. During the combustion the temperature increases from23.18 to 25.79 °C. The heat capacity of water is 4.184 J g-¹°C-1.MindTap - Cenga XReferencesThe heat capacity of the calorimeter was determined in a previous experimentto be 797.7 J/°C.Molar Heat of Combustion =Submit AnswerAssuming that no energy is lost to the surroundings, calculate the molar heatof combustion of azulene based on these data.C10Hg(s) + 1202(9) 4 H₂O(1) + 10 CO₂(g) + Energyab Calorimeter Calculations: This is group attempt 1 of 10kJ/molMacBook AirAutosaved at 10:21 PMSpecific HeatsIgnitionwiresheatsampleWaterStirrerXQThermometerInsulated Sample Burningoutside dishsamplechamber.CA samp✩SteelbombCombustion (bomb) calorimeter.

Mass of compound = 0.3163 g Molar mass = 128.17 g/mol Mole(n) = 0.3163/128.17 = 0.002468 mol…

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 0.3163 g sample of azulene (C₁0H8) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.061x10³ g of water. During the combustion the temperature increases from 23.18 to 25.79 °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 797.7 3/°C. Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of azulene based on these data. C10Hg(s) + 120₂(9) 4 H₂O(1) + 10 CO₂(g) + Energy Molar Heat of Combustion = kJ/mol Ignition wires heat sample Water Stirrer Thermometer Sample Burning Steel sample bomb dish Insulated outside chamber Combustion (bomb) calorimeter.

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 0.3163 g sample of azulene (C₁0H8) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.061x10³ g of water. During the combustion the temperature increases from 23.18 to 25.79 °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 797.7 3/°C. Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of azulene based on these data. C10Hg(s) + 120₂(9) 4 H₂O(1) + 10 CO₂(g) + Energy Molar Heat of Combustion = kJ/mol Ignition wires heat sample Water Stirrer Thermometer Sample Burning Steel sample bomb dish Insulated outside chamber Combustion (bomb) 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...

See similar textbooks

Similar questions

In the laboratory a "coffee cup" calorimeter, or constant pressure calorimeter, is frequently used to determine the specific heat capacity of a solid, or to measure the enthalpy change of a solution phase reaction. A student heats 66.56 g iron to 99.38 °C and carefully lowers it into a cup containing 84.64 g water at 21.17 °C. She measures the final temperature to be 26.99 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.81 J/°C. Assuming that there is no heating of the surroundings calculate the specific heat capacity of iron. Specific Heat (Fe) = 0.451 J g-1 °C-1. Water Thermometer Metal- sample 2003 Thomson-Brooks/Cole Stirring rod
A sample of 35.41 g of Cus at 96.73 degrees celcius was added to a calorimeter containing 148.3 g of H2O l at 25.20 degrees C. The final temperature of the system was 26.66 degrees C. Assuming no heat heat loss to the surroundings, what is the calorimeter constant?
At constant volume, the heat of combustion of a particular compound, compound A, is −3520.0 kJ/mol.−3520.0 kJ/mol. When 1.439 g1.439 g of compound A (molar mass =112.71 g/mol)=112.71 g/mol) is burned in a bomb calorimeter, the temperature of the calorimeter (including its contents) rose by 6.391 ∘C.6.391 ∘C. What is the heat capacity (calorimeter constant) of the calorimeter?
When a solid dissolves in water, heat may be evolved or absorbed. The heat of dissolution (dissolving) can be determined using a coffee cup calorimeter.In the laboratory a general chemistry student finds that when 0.77 g of KOH(s) are dissolved in 108.00 g of water, the temperature of the solution increases from 23.34 to 25.12 °C.The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.83 J/°C.Based on the student's observation, calculate the enthalpy of dissolution of KOH(s) in kJ/mol.Assume the specific heat of the solution is equal to the specific heat of water.ΔHdissolution = ______kJ/mol
Having just invented a new type of calorimeter, Dr. Cox needs to determine the heat capacity of the calorimeter. She carries out the following experiment to do this: Her empty calorimeter is at a temperature of 25.0ºC. She adds 32.502 grams of water at a temperature of 72.5ºC to the empty calorimeter and the final temperature of the calorimeter and the water is 39.5ºC. Based on this experiment, what is the heat capacity of her calorimeter assuming units of J/ºC? Enter your answer with at least 3 sig figs.
A bomb calorimeter has a heat capacity of 2.47 kJ/?. When a 1.00 mol sample of a certain hydrocarbon was burned in this calorimeter, the temperature increased by 2.14?. Calculate the heat of combustion per mole of the hydrocarbon.
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 69.43 grams of nickel to 97.93 °C and then drops it into a cup containing 75.96 grams of water at 20.90 °C. She measures the final temperature to be 27.45 °C.The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.71 J/°C.Assuming that no heat is lost to the surroundings calculate the specific heat of nickel.Specific Heat (Ni) = J/g°C.
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 65.54 grams of copper to 98.08 °C and then drops it into a cup containing 78.67 grams of water at 23.78 °C. She measures the final temperature to be 29.26 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.57 J/°C. Assuming that no heat is lost to the surroundings calculate the specific heat of copper. Specific Heat (Cu) = J/g°C.
A 1.200 g sample of ZnCO3 (s) dissolved in 40.0 mL of a dilute HCl solution (density = 1.10 g/mL) in a coffee cup calorimeter, producing CO2 (g), liquid water and ZnCl2 (aq). The temperature of the solution changes from 24.32 oC to 25.49 oC. The resulting solution has a specific heat of 4.18 J/goC. What would be the # of heat released by the reaction and Is the reaction endothermic?
A serving of Chocobits cereal is 122 g.A 1.00-g sample of the cereal is burned in a bomb calorimeter that has a heat capacity, C, of 8.50 kJ K-1, causing the temperature to increase from 25.0°C to 25.8°C. Calculate the energy of Chocobits in Calories per serving to three significant figures. 1 Cal = 4.184 kJ
A 77.5g piece of brass is heated so that its temperature is 98.7◦C. Next,it is quickly placed in a calorimeter containing 102.76 g of water at 18.5◦C.Knowing that the final temperature is 23.5◦C, what is the specific heat of this alloy?Note: Brass is an alloy of copper and zinc. From 98.7 to 23.5◦C, this alloy does not changeno phase, it remains in solid form.
When 1.42 g of iron reacts with 1.80 g of chlorine, 3.22 g of iron(II) chloride (FeCl2, molar mass = 126.75 g/mol) and 6.8 kJ of heat is produced. What is the enthalpy change for the reaction when 1 mole of iron(II) chloride is produced? round to sig figs