Question

1. A bomb calorimeter, or a constant volume calorimeter, is a device often used to determine...

1.

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 0.4137 g sample of bianthracene (C28H18) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.361×103 g of water. During the combustion the temperature increases from 24.82 to 27.25 °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 760.2 J/°C.

Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of bianthracene based on these data.

C28H18(s) + (65/2) O2(g) > 9 H2O(l) + 28 CO2(g) + Energy

Molar Heat of Combustion =    kJ/mol

2.

A bomb calorimeter, or constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of foods.

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.

In the laboratory a student burns a 0.831-g sample of glutaric acid (C5H8O4) in a bomb calorimeter containing 1110. g of water. The temperature increases from 25.40 °C to 27.90 °C. The heat capacity of water is 4.184 J g-1°C-1.

The molar heat of combustion is −2151 kJ per mole of glutaric acid.

C5H8O4(s) + 5 O2(g) >5 CO2(g) + 4 H2O(l) + Energy

Calculate the heat capacity of the calorimeter.

heat capacity of calorimeter =  J/°C

3.

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 0.7263 g sample of para-benzoquinone (C6H4O2) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.225×103 g of water. During the combustion the temperature increases from 28.02 to 30.95 °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 884.1 J/°C.

Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of para-benzoquinone based on these data.

C6H4O2(s) + 6O2(g) > 2 H2O(l) + 6 CO2(g) + Energy

Molar Heat of Combustion =    kJ/mol

Homework Answers

Answer #1

mass of water = 1.361×103 g

dT = T2 -T1 = 27.25 - 24.82 = 2.43

dT = 17.9 oC

Q = ( m Cp dT ) solution + ( Cp dT ) calorimeter

Q = 1.361 x 10^3 x 4.184 x 2.43 + 760.2 x 2.43

Q = 15684.7 J

Q = 15.685 kJ

moles of bianthracene = 0.4137 / 354 = 1.168 x 10^-3

deltaHrxn = - Q / n

             = - 15.685 / 1.168 x 10^-3

             = -13421.5 kJ / mol

Molar Heat of Combustion = -13421.5 kJ / mol

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
A bomb calorimeter, or a constant volume calorimeter, is a device often used to determine the...
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 0.3833 g sample of phenanthrene (C14H10) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.284×103 g of water. During the combustion the temperature increases from 22.04 to 24.54 °C. The heat capacity of water is 4.184 J g-1°C-1. The heat capacity of the calorimeter was...
A bomb calorimeter, or a constant volume calorimeter, is a device often used to determine the...
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 0.5265 g sample of bisphenol A (C15H16O2) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.377×103 g of water. During the combustion the temperature increases from 21.79 to 24.65 °C. The heat capacity of water is 4.184 J g-1°C-1. The heat capacity of the calorimeter...
A bomb calorimeter, or a constant volume calorimeter, is a device often used to determine the...
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 1.4170 g sample of L-ascorbic acid (C6H8O6) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.354×103 g of water. During the combustion the temperature increases from 24.92 to 27.68 °C. The heat capacity of water is 4.184 J g-1°C-1. The heat capacity of the calorimeter...
A 0.553-g sample of diphenyl phthalate (C20H14O4) is burned in a bomb calorimeter and the temperature...
A 0.553-g sample of diphenyl phthalate (C20H14O4) is burned in a bomb calorimeter and the temperature increases from 24.40 °C to 27.57 °C. The calorimeter contains 1.08×103 g of water and the bomb has a heat capacity of 877 J/°C. The heat capacity of water is 4.184 J g-1°C-1. Based on this experiment, calculate ΔE for the combustion reaction per mole of diphenyl phthalate burned. ______ kJ/mol
In the laboratory a student burns a 1.17-g sample of dimethyl oxalate (C4H6O4) in a bomb...
In the laboratory a student burns a 1.17-g sample of dimethyl oxalate (C4H6O4) in a bomb calorimeter containing 1070. g water. The temperature increases from 24.60 °C to 27.70 °C. The specific heat capacity of water is 4.184 J g-1 °C-1. The combustion enthalpy is −1675 kJ/mol dimethyl oxalate. C4H6O4(s) + 7/2 O2(g) 4 CO2(g) + 3 H2O(l) ΔrH o = -1675 kJ/mol Calculate the heat capacity of the calorimeter. heat capacity of calorimeter = J/°C
A quantity of 1.922 g of methanol (CH3OH) was burned in a constant-volume bomb calorimeter. Consequently,...
A quantity of 1.922 g of methanol (CH3OH) was burned in a constant-volume bomb calorimeter. Consequently, the temperature rose by 5.56°C. If the heat capacity of the bomb plus water was 8.09 kJ / °C, calculate the molar heat of combustion of methanol.
1. 0.1964 g sample of the solid quinone (C6H4O2) is combusted in a bomb calorimeter in...
1. 0.1964 g sample of the solid quinone (C6H4O2) is combusted in a bomb calorimeter in the presence of excess oxygen. The total heat capacity of the calorimeter including water is 1.560 kJ/°C. The temperature of the calorimeter increases initially from 22.000˚C to 25.200˚C. Write the balanced combustion reaction: (diff=3) a. Calculate the enthalpy of combustion of quinone in kJ/mol. b. Determine the enthalpy of formation of quinone (in kJ/mol). Use Appendix C from your textbook as needed. Hint: Write...
an alternative approach to bomb calorimeters is to establish the heat capacity of the calorimeter,, exclusive...
an alternative approach to bomb calorimeters is to establish the heat capacity of the calorimeter,, exclusive (without the presence of) the water it contains. the heat absorbed by the water and by the rest of the calorimeter must be calculated separately and then added together. a bomb calorimeter assembly containing 983.5g of water is calibrated by the combustion of 1.354g anthracene (C14H10(s)) . the temperature rises from 24.87 to 35.63 degrees C in this reaction. once calibrated, when 1.053g of...
A 1.000 g sample of octane (C8H18) is burned in a bomb calorimeter containing 1200 grams...
A 1.000 g sample of octane (C8H18) is burned in a bomb calorimeter containing 1200 grams of water at an initial temperature of 25.00ºC. After the reaction, the final temperature of the water is 33.20ºC. The heat capacity of the calorimeter (also known as the “calorimeter constant”) is 837 J/ºC. The specific heat of water is 4.184 J/g ºC. Calculate the heat of combustion of octane in kJ/mol.
When 86.6 g of a compound was burned in a bomb calorimeter that contained 0.184 kg...
When 86.6 g of a compound was burned in a bomb calorimeter that contained 0.184 kg of water the temperature rise of the water in the calorimeter was 57.0C. If the heat of combustion of the compound is 1,396 kJ/mol, what is the molar mass of the compound? Specific heat of water is 4.184 J/gC. Answer to 0 decimal places and enter the units.
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT
Active Questions
  • Determine whether each of the following scenarios is a regression, classification, or clustering problem. We run...
    asked 4 minutes ago
  • A car makes a trip along a straight line without changing direction. The average speed of...
    asked 9 minutes ago
  • What were the major differences during the reconstruction era between the northern and southern parts of...
    asked 14 minutes ago
  • A group of researchers want to determine whether the order in which items are presented influences...
    asked 16 minutes ago
  • A scientist wishes to perform the Stern-Gerlach experiment to separate silver atoms at least 1cm (greater...
    asked 19 minutes ago
  • You are conducting a study to see if the mean doctor's salary (in thousands of dollars)...
    asked 26 minutes ago
  • 70% of the students applying to a university are accepted. Assume the requirements for a binomial...
    asked 37 minutes ago
  • Problem 9-24 Comprehensive Variance Analysis [LO9-4, LO9-5, LO9-6] Marvel Parts, Inc., manufactures auto accessories. One of...
    asked 41 minutes ago
  • please answer the following question: Debate the two approaches from business and technology perspective. A “keep...
    asked 44 minutes ago
  • I need a solution of this structural dynamics problem? A mass with mass 1 is attached...
    asked 44 minutes ago
  • According to a recent study1, it takes between 5.6 and 10.2 million joules of energy to...
    asked 50 minutes ago
  • A regression analysis has been conducted between the annual income (in 1000 euros) and the work...
    asked 58 minutes ago