Question

Propane (C3H8) burns in oxygen to form carbon dioxide and water. A 0.5000 g sample of...

Propane (C3H8) burns in oxygen to form carbon dioxide and water. A 0.5000 g sample of propane was burned in a bomb calorimeter whose total heat capacity is 17.15 kJ/K. The temperature of the calorimeter apparatus increased by 2.591 K. Calculate the heat of combustion per mole of propane.

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Propane gas, C3H8, undergoes combustion with oxygen gas to produce carbon dioxide and water gases. Propane...
Propane gas, C3H8, undergoes combustion with oxygen gas to produce carbon dioxide and water gases. Propane has a density of 2.02 g/L at room temperature. Write the balanced chemical equation. How many grams of H2O form when 5.50 L of C3H8 reacts? How many grams of H2O can be produced from the reaction of 170. g of C3H8 ?
Suppose you burned 0.414 g of solid carbon in an excess of oxygen gas in a...
Suppose you burned 0.414 g of solid carbon in an excess of oxygen gas in a constant-volume calorimeter to give carbon dioxide gas. C(s) + O2(g) → CO2(g) The temperature of the calorimeter, which contained 770. g of water, increased from 23.02°C to 26.31°C. The heat capacity of the bomb is 901. J/K. Calculate ΔU per mole of carbon.
The combustion of titanium with oxygen produces titanium dioxide: Ti (s) + O2(g) → TiO2 (s)...
The combustion of titanium with oxygen produces titanium dioxide: Ti (s) + O2(g) → TiO2 (s) When 2.060 g of titanium is combusted in a bomb calorimeter, the temperature of the calorimeter increases from 25.00 °C to 91.60 °C. In a separate experiment, the heat capacity of the calorimeter is measured to be 9.84 kJ/K. The heat of reaction for the combustion of a mole of Ti in this calorimeter is ________ kJ/mol.
A sample of 1.05 moles of propane (C3H8) is completely burned in 2.25 moles of oxygen....
A sample of 1.05 moles of propane (C3H8) is completely burned in 2.25 moles of oxygen. The products are carbon dioxide and water.
When propane (C3H8) is combusted with excess oxygen, carbon dioxide and water vapor are produced. a....
When propane (C3H8) is combusted with excess oxygen, carbon dioxide and water vapor are produced. a. Determine how many grams of each reactant are required to produce 50.0 g of carbon dioxide. b. If you combined the number of grams of both reactants determined in part a and produced 47.31 grams of carbon dioxide, what would the percent error for the experiment be?
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.
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
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).
The next three questions are based on the combustion of propane gas (C3H8) with oxygen to...
The next three questions are based on the combustion of propane gas (C3H8) with oxygen to produce carbon dioxide and water vapor. C3H8(g) + 5 O2(g) → 3 CO2(g) + 4 H2O(g) Stu Dent measures exactly 5.10 g of C3H8 and burns it with excess oxygen gas. What is his theoretical yield of carbon dioxide gas?  What is his theoretical yield of water vapor?  (Both answers should have 3 significant digits and units of g) Stu measures his experimental products. He finds...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT