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Chapter 5: Q43 E (page 271)

Calculate the enthalpy of solution (鈭咹 for the dissolution) per mole of CaCl2(refer to Exercise 5.25).

Short Answer

Expert verified

The enthalpy of a solution (鈭咹 for the dissolution) per mole of CaCl2 is 81 kJ/mol.

Step by step solution

01

Given data

The molar mass of CaCl2 = 110.98 g/mol.

Mass of CaCl2 = 3.0g.

\begin{aligned}{\rm{NumberofmolesofCaC}}{{\rm{l}}_{\rm{2}}}{\rm{=}}\frac{{{\rm{givenmass\;}}}}{{{\rm{molarmass}}}}{\rm{\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;}}\\{\rm{=}}\frac{{{\rm{3}}{\rm{.0g}}}}{{{\rm{110}}{\rm{.98g/mol}}}}{\rm{\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;}}\\\end{aligned}

\begin{aligned}{\rm{=0}}{\rm{.0270 mol}}\end{aligned}

02

Enthalpy of a solution

The formula for finding the enthalpy of a solution is given below:

\[{\bf{Enthalpy=}}\frac{{{\bf{Heat of the solution}}}}{{{\bf{Number of moles}}}}\]

The known values are substituted:

\begin{aligned}{\rm{Enthalpy=}}\frac{{{\rm{2}}{\rm{.2kJ}}}}{{{\rm{0}}{\rm{.0270mol}}}}{\rm{\;}}\\{\rm{=81kJ/mol}}\end{aligned}

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Most popular questions from this chapter

Calculate \[{\bf{\Delta H}}_{{\bf{298 }}}^{\bf{^\circ }}\] for the process \[{\bf{C}}{{\bf{o}}_{\bf{3}}}{{\bf{O}}_{\bf{4}}}\left( {\bf{s}} \right) \to {\bf{3Co}}\left( {\bf{s}} \right){\bf{ + 2}}{{\bf{O}}_{\bf{2}}}\left( {\bf{g}} \right)\]

from the following information:

\[\begin{array}{c}{\bf{Co(s) + }}\frac{{\bf{1}}}{{\bf{2}}}{{\bf{O}}_{\bf{2}}}{\bf{(g)}} \to {\bf{CoO(s) \Delta H}}_{{\bf{298}}}^{\bf{^\circ }}{\bf{ = - 237}}{\bf{.9kJ}}\\{\bf{3CoO(s) + }}\frac{{\bf{1}}}{{\bf{2}}}{{\bf{O}}_{\bf{2}}}{\bf{(g)}} \to {\bf{C}}{{\bf{o}}_{\bf{3}}}{{\bf{O}}_{\bf{4}}}{\bf{(s) \Delta H}}_{{\bf{298}}}^{\bf{^\circ }}{\bf{ = - 177}}{\bf{.5kJ}}\end{array}\]

When 2.50 g of methane burns in oxygen, 125 kJ of heat is produced. What is the enthalpy of combustion per mole of methane under these conditions?

Using the data in Appendix G, calculate the standard enthalpy change for each of the following reactions:

(a) N2(g) + O2(驳)鉄�2狈翱(驳)

(b) Si(s) + 2Cl2(驳)鉄禨颈颁濒4(g)

(c) Fe2O3(s) + 3H2(g)鉄�2Fe(s) + 3H2O(l)

(d) 2LiOH(s) + CO2(驳)鉄禠颈2CO3(s) + H2O(g)

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 螖H掳 for reaction(i):

\(\begin{array}{*{20}{l}}{\left( {{\bf{ii}}} \right){\rm{ }}{\bf{HCl(g)}} \to {\bf{HCl(aq) \Delta H^\circ (ii) = - 74}}{\bf{.8 kJ}}}\\{\left( {{\bf{iii}}} \right){\rm{ }}{{\bf{H}}_{\bf{2}}}{\bf{(g) + C}}{{\bf{l}}_{\bf{2}}}{\bf{(g)}} \to {\bf{2HCl(g) \Delta H^\circ (iii) = - 185 kJ}}}\\{\left( {{\bf{iv}}} \right){\rm{ }}{\bf{AlC}}{{\bf{l}}_{\bf{3}}}{\bf{(aq)}} \to {\bf{AlC}}{{\bf{l}}_{\bf{3}}}{\bf{(s) \Delta H^\circ (iv) = + 323 kJ}}}\\{\left( {\bf{v}} \right){\rm{ }}{\bf{2Al(s) + 6HCl(aq)}} \to {\bf{2AlC}}{{\bf{l}}_{\bf{3}}}{\bf{(aq) + 3}}{{\bf{H}}_{\bf{2}}}{\bf{(g) \Delta H^\circ (v) = - 1049 kJ}}}\end{array}\)

Water gas, a mixture of \({{\bf{H}}_{\bf{2}}}\) and CO, is an important industrial fuel produced by the reaction of steam with red hot coke, essentially pure carbon:\({\bf{C}}\left( {\bf{s}} \right){\bf{ + }}{{\bf{H}}_{\bf{2}}}{\bf{O}}\left( {\bf{g}} \right) \to {\bf{CO}}\left( {\bf{g}} \right){\bf{ + }}{{\bf{H}}_{\bf{2}}}\left( {\bf{g}} \right)\).

(a) Assuming that coke has the same enthalpy of formation as graphite, calculate \({\bf{\Delta H}}_{{\bf{298}}}^{\bf{0}}\)for this reaction.

(b) Methanol, a liquid fuel that could possibly replace gasoline, can be prepared from water gas and additional hydrogen at high temperature and pressure in the presence of a suitable catalyst:\({\bf{2}}{{\bf{H}}_{\bf{2}}}\left( {\bf{g}} \right){\bf{ + CO}}\left( {\bf{g}} \right) \to {\bf{C}}{{\bf{H}}_{\bf{3}}}{\bf{OH}}\left( {\bf{g}} \right)\).

Under the conditions of the reaction, methanol forms as a gas. Calculate \({\bf{\Delta H}}_{{\bf{298}}}^{\bf{0}}\)for this reaction and for the condensation of gaseous methanol to liquid methanol.

(c) Calculate the heat of combustion of 1 mole of liquid methanol to H2O(g) and CO2(g).
See all solutions

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