Question

A bomb calorimeter is placed in a water bath, and a mixture of fueland oxygen is...

A bomb calorimeter is placed in a water bath, and a mixture of fueland oxygen is burned inside it.The temperature of the water isobserved to rise during the combustion reaction. Thecalorimeter ant the water remain at constant volume.

a. If the reaction products are the system, which thermodynamicsquantities - ΔU, Q or W- are positive and which arenegative?
b. If the water bath is the system, which thermodynamic quantities-- ΔU, Q -- are positive and which are negative?

Homework Answers

Answer #1

Assume

Q - W = dU is valid

so

a)

fuel + oxygen = system

the system is breaking its bonds to release energy

so they give off heat, dU = must be negative, since it is losing energy

Q = negative, as well, releasing heat

W =the system expands, thereofre system doing work on surroundings, W = +

b)

if bath system is surroundings then

dU = increases, since it is absorbing heat

Q = positive, since it is absorbing heat

W = negative, since it is getting compressed, i.e. the system is doing work on the surrouindings

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 0.727 g sample of D-ribose (C5H10O5) was placed in a bomb calorimeter (constant volume) and...
A 0.727 g sample of D-ribose (C5H10O5) was placed in a bomb calorimeter (constant volume) and ignited in the presence of excess oxygen. The temperature was observed to rise by 0.910 K. In a separate experiment, 0.825 g of benzoic acid (C6H5CO2H) is similarly ignited in the same calorimeter, and is observed to cause an increase of the temperature of 1.940 K. The internal energy of combustion of benzoic acid is -3251 kJ mol-1. (a) Calculate the heat capacity of...
Benzoic acid, C6H5COOH, is a common standard used in bomb calorimeters, which maintain a constant volume....
Benzoic acid, C6H5COOH, is a common standard used in bomb calorimeters, which maintain a constant volume. If 1.20 g of benzoic acid gives off 31,723 J of energy when burned in the presence of excess oxygen and in a water bath having a temperature of 24.6°C, calculate q, w, DH, and DU for the reaction.
If 4.40 g of glucose are burned in a bomb calorimeter, the temperature of the 800...
If 4.40 g of glucose are burned in a bomb calorimeter, the temperature of the 800 g of water in the calorimeter increases from 15.0∘C to 18.7∘C. If the heat capacity of the calorimeter is 550J∘C, what is the value of q for the combustion of the glucose sample?
1 g of α -D-glucose is burned in the adiabatic bomb calorimeter. The bomb is surrounded...
1 g of α -D-glucose is burned in the adiabatic bomb calorimeter. The bomb is surrounded by 2.500 L of H2O at 24.030°C. The bomb is made of steel and weighs 14.05 kg. Specific heats at constant pressure of water and steel at 24°C are 4.180 and 0.450 J/(g °C), respectively. The density of water at 24°C is 0.9973 g/cm3. Assuming the heat capacity of the chemicals in the bomb is negligible compared with the heat capacity of the bomb...
In order to calibrate a constant volume bomb calorimeter, the combustion of (7.450x10^-1) g of benzoic...
In order to calibrate a constant volume bomb calorimeter, the combustion of (7.450x10^-1) g of benzoic acid, C6H5COOH, was observed to cause the temperature in the calorimeter to rise from 25.000 to (2.87000x10^1) oC. The energy of combustion of benzoic acid, ΔU, is -3226.7 kJ mol-1. What is total heat capacity (C) of the calorimeter (including all its contents) in kJ oC-1?
A 0.373-g sample of naphthalene (C10H8) is burned in a bomb calorimeter and the temperature increases...
A 0.373-g sample of naphthalene (C10H8) is burned in a bomb calorimeter and the temperature increases from 24.90 °C to 27.80 °C. The calorimeter contains 1.05E3 g of water and the bomb has a heat capacity of 836 J/°C. Based on this experiment, calculate ΔE for the combustion reaction per mole of naphthalene burned (kJ/mol).
A 0.287-g sample of bianthracene (C28H18) is burned in a bomb calorimeter and the temperature increases...
A 0.287-g sample of bianthracene (C28H18) is burned in a bomb calorimeter and the temperature increases from 25.30 °C to 27.50 °C. The calorimeter contains 1.03E3 g of water and the bomb has a heat capacity of 856 J/°C. Based on this experiment, calculate ΔE for the combustion reaction per mole of bianthracene burned (kJ/mol).
A bomb calorimeter (C = 147 J/°C) contained 65 g of C4H4O (l) and excess O2...
A bomb calorimeter (C = 147 J/°C) contained 65 g of C4H4O (l) and excess O2 (g). The calorimeter was immersed in a 150. g water bath (Cwater = 4.19 J/g°C) and the calorimeter and the bath were equilibrated at 22.00 °C. The fuel was combusted, and the temperature of the calorimeter and the water bath were monitored independently. After 5 minutes, the calorimeter reached a maximum temperature of 25.04°C. At that time, the water bath had warmed to 22.62...
A 0.424 g sample of liquid C5H12 was combusted completely using excess oxygen inside a bomb...
A 0.424 g sample of liquid C5H12 was combusted completely using excess oxygen inside a bomb (constant volume) calorimeter, with the products being carbon dioxide and liquid water. The calorimeter's heat capacity is 4.782 kJ °C-1. If the temperature inside the calorimeter increased from 25.0 °C to 33.4 °C, determine ΔH for this reaction with respect to the system in kJ mol-1 at 298 K. Do not worry about how realistic the final answer is.
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...