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Chapter 5: QCYL (page 227)

Write the heat of formation reaction equations for:

(a) \({{\bf{C}}_{\bf{2}}}{{\bf{H}}_{\bf{5}}}{\bf{O}}{{\bf{C}}_{\bf{2}}}{{\bf{H}}_{\bf{5}}}\)(l)

(b) \({\bf{N}}{{\bf{a}}_{\bf{2}}}{\bf{C}}{{\bf{O}}_{\bf{3}}}\)(s)

Short Answer

Expert verified

(a) \({\rm{\;4C }}\left( {{\rm{s, graphite}}} \right){\rm{ + 5}}{{\rm{H}}_{\rm{2}}}\left( {\rm{g}} \right){\rm{ + 1/2}}{{\rm{O}}_{\rm{2}}}{\rm{(g)}} \to {{\rm{C}}_{\rm{2}}}{{\rm{H}}_{\rm{5}}}{\rm{O}}{{\rm{C}}_{\rm{2}}}{{\rm{H}}_{\rm{5}}}{\rm{(l)}}\)

(b) \({\rm{Na}}\left( {\rm{s}} \right){\rm{ + C }}\left( {{\rm{s, graphite}}} \right){\rm{ + 3/2 }}{{\rm{O}}_{\rm{2}}}{\rm{(g) }} \to {\rm{ N}}{{\rm{a}}_{\rm{2}}}{\rm{C}}{{\rm{O}}_{\rm{3}}}{\rm{(s)}}\)

Step by step solution

01

Heat of formation

The heat of formation represented as 螖Hf掳 is used to form one mole of compound from its constituents鈥� elements under standard conditions.

It provides information on the enthalpy change happening during the formation of compounds.

02

Heat of formation of (a)

\({{\rm{C}}_{\rm{2}}}{{\rm{H}}_{\rm{5}}}{\rm{O}}{{\rm{C}}_{\rm{2}}}{{\rm{H}}_{\rm{5}}}\)(l)

As the standard state of carbon is graphite, hence

\({\rm{\;4C }}\left( {{\rm{s, graphite}}} \right){\rm{ + 5}}{{\rm{H}}_{\rm{2}}}\left( {\rm{g}} \right){\rm{ + 1/2}}{{\rm{O}}_{\rm{2}}}{\rm{(g)}} \to {{\rm{C}}_{\rm{2}}}{{\rm{H}}_{\rm{5}}}{\rm{O}}{{\rm{C}}_{\rm{2}}}{{\rm{H}}_{\rm{5}}}{\rm{(l)}}\)

03

Heat of formation of (b)

\({\rm{N}}{{\rm{a}}_{\rm{2}}}{\rm{C}}{{\rm{O}}_{\rm{3}}}\)(s)

As the standard state of carbon is graphite, hence

\({\rm{Na}}\left( {\rm{s}} \right){\rm{ + C }}\left( {{\rm{s, graphite}}} \right){\rm{ + 3/2 }}{{\rm{O}}_{\rm{2}}}{\rm{(g) }} \to {\rm{ N}}{{\rm{a}}_{\rm{2}}}{\rm{C}}{{\rm{O}}_{\rm{3}}}{\rm{(s)}}\)

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Most popular questions from this chapter

How much heat is produced by burning 4.00 moles of acetylene under standard conditions?

Both propane and butane are used as gaseous fuels. Which compound produces more heat per gram when burned?

Question: Calculate the heat capacity, in joules and in calories per degree, of the following:

(a) 28.4 g of water

(b) 1.00 oz of lead

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).

Calculate the heat capacity, in joules and in calories per degree, of the following:

(a) 45.8 g of nitrogen gas

(b) 1.00 pound of aluminum metal
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