The team performed a bomb calorimetry experiment on a sample of the liquid. A 1.0740 g sample of jojane was put into the bomb calorimeter with a high pressure of O2 gas. Upon combustion, the temperature of the calorime was seen to rise from 24.7109 to 28.5557 °C. The heat capacity of the calorimeter was previously determined to be 10.044 kJ °C-1 and in a separate experiment the molar mass of the substance was determined to be 74.1216 mol1. Determine AcombU for the substance. O 2670.0 kJ mol1 O 2670.0 kJ mol1 O 2665.2 kJ mol-1 O 2665.2 kJ mol-1

The team performed a bomb calorimetry experiment on a sample of the liquid. A 1.0740 g sample of jojane was put into the bomb calorimeter with a high pressure of O2 gas. Upon combustion, the temperature of the calorime was seen to rise from 24.7109 to 28.5557 °C. The heat capacity of the calorimeter was previously determined to be 10.044 kJ °C-1 and in a separate experiment the molar mass of the substance was determined to be 74.1216 mol1. Determine AcombU for the substance. O 2670.0 kJ mol1 O 2670.0 kJ mol1 O 2665.2 kJ mol-1 O 2665.2 kJ mol-1

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

A piece of metal weighing 8.00 g at a temperature of 46.0 oCo was placed in a calorimeter in 38.10 mL of water at 24.3 oC. The final equilibrium temperature was found to be 25.7 oC . What is the specific heat of the metal?
A 3.971 g sample of a new organic material is combusted in a bomb calorimeter. The temperature of the calorimeter and its contents increase from 24.87 ∘C to 28.06 ∘C. The heat capacity (calorimeter constant) of the calorimeter is 36.35 kJ/ ∘C, what is the heat of combustion per gram of the material?
14.00 g of Compound X with molecular formula C,H, are burned in a constant-pressure calorimeter containing 50.00 kg of water at 25 °C. The temperature of the water is observed to rise by 3.098 °C. (You may assume all the heat released by the reaction is absorbed by the water, and none by the calorimeter itself.) Calculate the standard heat of formation of Compound X at 25 °C. Be sure your answer has a unit symbol, if necessary, and round it to 3 significant digits. Ox10 ?
Part B 2.0000 g of the unknown compound is burned in a bomb calorimeter. During the combustion, the temperature of the calorimeter increases from 23.125°C to 28.997 °C. During calibration, the heat capacity of the calorimeter was found to be 9.9897kJ °C-1. In the previous experiment, the molar mass of the substance was found to be 148.16 gmol-1. What is AcombU for the unknown compound? να ΑΣφ ? kJ mol1 Submit Request Answer
In this experiment you will place a sample of your salt in water in a constant pressure calorimeter. You will determine the enthalpy change for the dissociation of your salt, Delta Hdiss. A sample of 4.368 grams of the salt SrCl2 was placed in 35.5 g water, the initial temperature was 20.00℃ and the final temperature was 27.086365℃. What is the number of moles of SrCl2? 4.368 g SrCl2 x ( 1 mol SrCl2 / 123.073 g SrCl2 ) = 0.035491131 mol SrCl2 a. 0.035491 mol SrCl2 b. none of these c. 0.035 mol SrCl2 d. 0.03 mol SrCl2 e. 0.0355 mol SrCl2 f. 0.04 mol SrCl2 g. 0.035491131 mol SrCl2 h. 0.03549 mol SrCl2
A piece of metal of mass 15 g at 99◦C is placed in a calorimeter containing 41.3 g of water at 19◦C. The final temperature of the mixture is 40.2◦C. What is the specific heat capacity of the metal? Assume that there is no energy lost to the surroundings. Answer in units ofJg·◦C.
Fructose, C6H12O6(s), is a sugar closely related to glucose. A 0.755 g sample of fructose was combusted with excess oxygen in a bomb calorimeter, containing 500.0 g of water. The heat capacity of the empty calorimeter was 208 J/K. The temperature of the calorimeter and the water rose from 22.00°C to 27.12°C due to the combustion reaction, which formed CO₂(g) and liquid water. What is the energy change, AU (in kJ), for the combustion of one mole of fructose under these conditions? O +254 O-15600 -2810 +520 -804
Fructose, C6H12O6(s), is a sugar closely related to glucose.. A 0.755 g sample of fructose was combusted with excess oxygen in a bomb calorimeter, containing 500.0 g of water. The heat capacity of the empty calorimeter was 208 J/K. The temperature of the calorimeter and the water rose from 22.00°C to 27.12°C due to the combustion reaction, which formed CO2(g) and liquid water. What is the energy change, AU (in kJ), for the combustion of one mole of fructose under these conditions? -15600 -2810 +520 +254 -804
A 57.1 g sample of polystyrene, which has a specific heat capacity of 1.880 J-g¹C, is put into a calorimeter (see sketch at right) that contains 100.0 g of water. The temperature of the water starts off at 23.0 °C. When the temperature of the water stops changing it's 38.3 °C. The pressure remains constant at 1 atm. Calculate the initial temperature of the polystyrene sample. Be sure your answer is rounded to 3 significant digits. 0°C 0...º X
A 25.0 mL portion of dilute HCl (aq) is combined with a 25.0 mL portion of dilute NaOH in a coffee-cup calorimeter. Both solutions are initially at a temperature of 23.3 ºC. The reaction produces enough heat to raise the final temperature of the 50.0 mL of liquid in the calorimeter to 25.3 ºC . What is qrxn in J? Assume the density of the reaction mixture is 1.0 g/mL and the specific heat of the solution is 4.184 J/g· ºC