Learning Materials
Features
Discover
Chapter 5: Q39 E (page 271)
Explain how the heat measured in example 5.5 differs from the enthalpy change for the endothermic reaction described by the following equation
HCl(aq)+NaOH(aq) → NaCl(aq)+H2O(I)
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
Before the introduction of chlorofluorocarbons, sulfur dioxide (enthalpy of vaporization, 6.00 kcal/mol) was used in household refrigerators. What mass of \({\bf{S}}{{\bf{O}}_{\bf{2}}}\)must be evaporated to remove as much heat as evaporation of 1.00 kg of \({\bf{CC}}{{\bf{l}}_{\bf{2}}}{{\bf{F}}_{\bf{2}}}\) (enthalpy of vaporization is 17.4 kJ/mol)?
The vaporization reactions for \({\bf{S}}{{\bf{O}}_{\bf{2}}}\)and \({\bf{CC}}{{\bf{l}}_{\bf{2}}}{{\bf{F}}_{\bf{2}}}\)are\({\bf{S}}{{\bf{O}}_{\bf{2}}}{\bf{(l)}} \to {\bf{S}}{{\bf{O}}_{\bf{2}}}{\bf{(g) and CC}}{{\bf{l}}_{\bf{2}}}{\bf{F(l) }} \to {\bf{CC}}{{\bf{l}}_{\bf{2}}}{{\bf{F}}_{\bf{2}}}{\bf{(g)}}\), respectively.
Calculate the enthalpy of solution (∆H) for the dissolution) per mole of NH4NO3 under the conditions described in example 5.6.
Aluminum chloride can be formed from its elements:
(i)\({\bf{2Al(s) + 3C}}{{\bf{l}}_{\bf{2}}}{\bf{(g)}} \to {\bf{2AlC}}{{\bf{l}}_{\bf{3}}}{\bf{(s) \Delta H^\circ = ?}}\)
Use the reactions here to determine the ΔH° for reaction(i):
\(\begin{array}{*{20}{l}}{\left( {{\bf{ii}}} \right){\rm{ }}{\bf{HCl(g)}} \to {\bf{HCl(aq) \Delta H^\circ (ii) = - 74}}{\bf{.8 kJ}}}\\{\left( {{\bf{iii}}} \right){\rm{ }}{{\bf{H}}_{\bf{2}}}{\bf{(g) + C}}{{\bf{l}}_{\bf{2}}}{\bf{(g)}} \to {\bf{2HCl(g) \Delta H^\circ (iii) = - 185 kJ}}}\\{\left( {{\bf{iv}}} \right){\rm{ }}{\bf{AlC}}{{\bf{l}}_{\bf{3}}}{\bf{(aq)}} \to {\bf{AlC}}{{\bf{l}}_{\bf{3}}}{\bf{(s) \Delta H^\circ (iv) = + 323 kJ}}}\\{\left( {\bf{v}} \right){\rm{ }}{\bf{2Al(s) + 6HCl(aq)}} \to {\bf{2AlC}}{{\bf{l}}_{\bf{3}}}{\bf{(aq) + 3}}{{\bf{H}}_{\bf{2}}}{\bf{(g) \Delta H^\circ (v) = - 1049 kJ}}}\end{array}\)
When 1.42 g of iron reacts with 1.80 g of chlorine, 3.22 g of \({\bf{FeC}}{{\bf{l}}_{\bf{2}}}\)(s) and 8.60 kJ of heat is produced. What is the enthalpy change for the reaction when 1 mole of \({\bf{FeC}}{{\bf{l}}_{\bf{2}}}\)(s) is produced?
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).
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