Propane, C 3 H 8 , is a hydrocarbon that is commonly used as a fuel. (a) Write a balanced equation for the complete combustion of propane gas. (b) Calculate the volume of air at 25 °C and 1.00 atmosphere that is needed to completely combust 25.0 grams of propane. Assume that air is 21.0 percent O 2 by volume. (Hint: we will see how to do this calculation in a later chapter on gases−for now use the information that 1.00 L of air at 25 °C and 1.00 atm contains 0.275 g of °2 per liter.) (c) The heat of combustion of propane is −2,219.2 kJ/mol. Calculate the heat of formation, Δ H f ° of propane given that Δ H f ° of H 2 O ( l ) = − 285.8 kJ/mol and Δ H f ° of CO 2 ( g ) = − 393.5 kJ/mol. (d) Assuming that all of the heat released in burning 25.0 grams of propane is transferred to 4.00 kilograms of water, calculate the increase in temperature of the water.
Propane, C 3 H 8 , is a hydrocarbon that is commonly used as a fuel. (a) Write a balanced equation for the complete combustion of propane gas. (b) Calculate the volume of air at 25 °C and 1.00 atmosphere that is needed to completely combust 25.0 grams of propane. Assume that air is 21.0 percent O 2 by volume. (Hint: we will see how to do this calculation in a later chapter on gases−for now use the information that 1.00 L of air at 25 °C and 1.00 atm contains 0.275 g of °2 per liter.) (c) The heat of combustion of propane is −2,219.2 kJ/mol. Calculate the heat of formation, Δ H f ° of propane given that Δ H f ° of H 2 O ( l ) = − 285.8 kJ/mol and Δ H f ° of CO 2 ( g ) = − 393.5 kJ/mol. (d) Assuming that all of the heat released in burning 25.0 grams of propane is transferred to 4.00 kilograms of water, calculate the increase in temperature of the water.
Propane,
C
3
H
8
, is a hydrocarbon that is commonly used as a fuel.
(a) Write a balanced equation for the complete combustion of propane gas.
(b) Calculate the volume of air at 25 °C and 1.00 atmosphere that is needed to completely combust 25.0 grams of propane. Assume that air is 21.0 percent O2 by volume. (Hint: we will see how to do this calculation in a later chapter on gases−for now use the information that 1.00 L of air at 25 °C and 1.00 atm contains 0.275 g of °2 per liter.)
(c) The heat of combustion of propane is −2,219.2 kJ/mol. Calculate the heat of formation,
Δ
H
f
°
of propane given that
Δ
H
f
°
of
H
2
O
(
l
)
=
−
285.8
kJ/mol and
Δ
H
f
°
of
CO
2
(
g
)
=
−
393.5
kJ/mol.
(d) Assuming that all of the heat released in burning 25.0 grams of propane is transferred to 4.00 kilograms of water, calculate the increase in temperature of the water.
A sample of a hydrocarbon is completely combusted in presence in O2(g) to produce 21.83 g carbon dioxide, 4.47 g H2O, and 311 KJ of heat.
What is the mass of hydrocarbon sample that was combusted?
What is the empirical formula of the hydrocarbon?
Calculate the value of Ho per empirical-formula unit of the hydrocarbon.
Do you think that the hydrocarbon is one of those listed in appendix C? Explain your answer.
A large sport utility vehicle has a mass of 2500 kg.Calculate the mass of CO2 emitted into the atmosphere upon accelerating the SUV from 0.0 mph to 65.0 mph. Assume that the required energy comes from the combustion of octane (C8H18) with 30% efficiency. (Hint: Use KE = ½ mv2 to calculate the kinetic energy required for the acceleration and pay attention to units).
(a) The atomic weight of carbon is 12, hydrogen is 1 and oxygen is 16, and the
formula for the combustion of methane (CH4) is given by :
CH4 + 2 O2 –→ CO2 + 2 H2O + energy
A mole of methane releases 810 KJ of energy on burning.
Calculate the weight of carbon dioxide produced by burning 5kg of methane.
Identify an alternative gas for combustion that produces less carbon dioxide
than methane and state how it is generated.
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Calorimetry Concept, Examples and Thermochemistry | How to Pass Chemistry; Author: Melissa Maribel;https://www.youtube.com/watch?v=nSh29lUGj00;License: Standard YouTube License, CC-BY