Learning Materials
Features
Discover
Chapter 5: Q5.3-78E (page 274)
From the data in Table 5.2, determine which of the following fuels produces the greatest amount of heat per gram when burned under standard conditions: CO(g), CH4(g), or C2H2(g).
The greatest amount of heat per gram is produced by CO(g).
Over 30 million students worldwide already upgrade their learning with Vaia!
All the tools & learning materials you need for study success - in one app.
Get started for free
Propane, \({{\bf{C}}_{\bf{3}}}{{\bf{H}}_{\bf{8}}}\), 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 O2 per liter.)
(c) The heat of combustion of propane is −2,219.2 kJ/mol. Calculate the heat of formation,ΔHf °of propane given thatΔHf °of H2O(l) = −285.8 kJ/mol andΔHf °of CO2(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.
From the molar heats of formation in Appendix G, determine how much heat is required to evaporate one mole of water:\({{\bf{H}}_{\bf{2}}}{\bf{O}}\left( {\bf{l}} \right) \to {{\bf{H}}_{\bf{2}}}{\bf{O}}\left( {\bf{g}} \right)\)
The white pigment \({\bf{Ti}}{{\bf{O}}_{\bf{2}}}\)is prepared by the reaction of titanium tetrachloride, \({\bf{TiC}}{{\bf{l}}_{\bf{4}}}\), with water vapor in the gas phase:
\({\bf{TiC}}{{\bf{l}}_{\bf{4}}}\left( {\bf{g}} \right){\bf{ + 2}}{{\bf{H}}_{\bf{2}}}{\bf{O}}\left( {\bf{g}} \right) \to {\bf{Ti}}{{\bf{O}}_{\bf{2}}}\left( {\bf{s}} \right){\bf{ + 4HCl}}\left( {\bf{g}} \right)\)
How much heat is evolved in the production of exactly 1 mole of \({\bf{Ti}}{{\bf{O}}_{\bf{2}}}\)(s) under standard state conditions?
Calculate the enthalpy of combustion of butane, C4H10(g) for the formation of H2O(g) and CO2(g). The enthalpy of formation of butane is -126 kJ/mol.
When a 3.00-g sample of KCl was added to 3.00×102 g of water in a coffee cup calorimeter, the temperature decreased by 1.05 °C. How much heat is involved in the dissolution of the KCl? What assumptions did you make?
What do you think about this solution?
We value your feedback to improve our textbook solutions.
Explanations 
Textbooks 
Exams 
GCSE 
IGCSE 
AS 
A Level 
International A Level 
University Admissions Tests 
Flashcards 
Vaia AI 
Notes 
Study Plans 
Study Sets 
Find a job 
Find a degree 
Student Deals 
Magazine 
Mobile App