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Chapter 7: Problem 76

Write reactions for which the enthalpy change will be a. \(\Delta H_{\mathrm{f}}^{\circ}\) for solid aluminum oxide. b. the standard enthalpy of combustion of liquid ethanol, \(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}(l)\). c. the standard enthalpy of neutralization of sodium hydroxide solution by hydrochloric acid. d. \(\Delta H_{\mathrm{f}}^{\circ}\) for gaseous vinyl chloride, \(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{Cl}(g)\). e. the enthalpy of combustion of liquid benzene, \(C_{6} \mathrm{H}_{6}(l)\). f. the enthalpy of solution of solid ammonium bromide.

Short Answer

Expert verified
a. \(4 \mathrm{Al}(s) + 3 \mathrm{O}_2(g) \rightarrow 2 \mathrm{Al}_2 \mathrm{O}_3(s)\) b. \(\mathrm{C}_{2}\mathrm{H}_{5}\mathrm{OH}(l) + 3 \mathrm{O}_2(g) \rightarrow 2 \mathrm{CO}_2(g) + 3 \mathrm{H}_2 \mathrm{O}(l) \) c. \(\mathrm{NaOH}(aq) + \mathrm{HCl}(aq) \rightarrow \mathrm{H}_2 \mathrm{O}(l) + \mathrm{NaCl}(aq) \) d. \(\mathrm{C}(s) + \frac{3}{2} \mathrm{H}_2(g) + \frac{1}{2} \mathrm{Cl}_2(g) \rightarrow \mathrm{C}_{2}\mathrm{H}_{3}\mathrm{Cl}(g) \) e. \(\mathrm{C}_6 \mathrm{H}_6(l) + \frac{15}{2} \mathrm{O}_2(g) \rightarrow 6 \mathrm{CO}_2(g) + 3 \mathrm{H}_2 \mathrm{O}(l) \) f. \(\mathrm{NH}_4\mathrm{Br}(s) \rightarrow \mathrm{NH}_4^+(aq) + \mathrm{Br}^-(aq) \)

Step by step solution

01

Write the balanced equation for the formation of aluminum oxide

Aluminum oxide (Al₂O₃) is formed when aluminum (Al) reacts with oxygen (O₂). To balance the equation, we need to have 2 aluminum atoms and 3 oxygen atoms on each side: \[4 \mathrm{Al}(s) + 3 \mathrm{O}_2(g) \rightarrow 2 \mathrm{Al}_2 \mathrm{O}_3(s)\] b. Standard enthalpy of combustion of liquid ethanol
02

Write the balanced equation for the combustion of ethanol

In combustion reactions, the substance reacts with oxygen (O₂) to produce carbon dioxide (CO₂) and water (H₂O). Ethanol (C₂H₅OH) combusts to form carbon dioxide and water: \[ \mathrm{C}_{2}\mathrm{H}_{5}\mathrm{OH}(l) + 3 \mathrm{O}_2(g) \rightarrow 2 \mathrm{CO}_2(g) + 3 \mathrm{H}_2 \mathrm{O}(l) \] c. Standard enthalpy of neutralization of sodium hydroxide solution by hydrochloric acid
03

Write the balanced equation for the neutralization of sodium hydroxide by hydrochloric acid

In a neutralization reaction, sodium hydroxide (NaOH) and hydrochloric acid (HCl) react to form water (H₂O) and sodium chloride (NaCl): \[ \mathrm{NaOH}(aq) + \mathrm{HCl}(aq) \rightarrow \mathrm{H}_2 \mathrm{O}(l) + \mathrm{NaCl}(aq) \] d. Formation of gaseous vinyl chloride
04

Write the balanced equation for the formation of vinyl chloride

Vinyl chloride (C₂H₃Cl) is formed from the elements carbon (C), hydrogen (H₂), and chlorine (Cl₂): \[ \mathrm{C}(s) + \frac{3}{2} \mathrm{H}_2(g) + \frac{1}{2} \mathrm{Cl}_2(g) \rightarrow \mathrm{C}_{2}\mathrm{H}_{3}\mathrm{Cl}(g) \] e. Enthalpy of combustion of liquid benzene
05

Write the balanced equation for the combustion of benzene

Benzene (C₆H₆) combusts to form carbon dioxide (CO₂) and water (H₂O): \[ \mathrm{C}_6 \mathrm{H}_6(l) + \frac{15}{2} \mathrm{O}_2(g) \rightarrow 6 \mathrm{CO}_2(g) + 3 \mathrm{H}_2 \mathrm{O}(l) \] f. Enthalpy of solution of solid ammonium bromide
06

Write the balanced equation for the dissolution of ammonium bromide

Ammonium bromide (NH₄Br) dissolves in water (H₂O) to form ammonium ions (NH₄⁺) and bromide ions (Br⁻): \[ \mathrm{NH}_4\mathrm{Br}(s) \rightarrow \mathrm{NH}_4^+(aq) + \mathrm{Br}^-(aq) \]

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Most popular questions from this chapter

Explain the advantages and disadvantages of hydrogen as an alternative fuel.

Standard enthalpies of formation are relative values. What are \(\Delta H_{\mathrm{f}}^{\circ}\) values relative to?

It has been determined that the body can generate \(5500 \mathrm{kJ}\) of energy during one hour of strenuous exercise. Perspiration is the body's mechanism for eliminating this heat. What mass of water would have to be evaporated through perspiration to rid the body of the heat generated during 2 hours of exercise? (The heat of vaporization of water is \(40.6 \mathrm{kJ} / \mathrm{mol.}\))

In which of the following systems is(are) work done by the surroundings on the system? Assume pressure and temperature are constant. a. \(2 \mathrm{SO}_{2}(g)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{SO}_{3}(g)\) b. \(\mathrm{CO}_{2}(s) \longrightarrow \mathrm{CO}_{2}(g)\) c. \(4 \mathrm{NH}_{3}(g)+7 \mathrm{O}_{2}(g) \longrightarrow 4 \mathrm{NO}_{2}(g)+6 \mathrm{H}_{2} \mathrm{O}(g)\) d. \(\mathrm{N}_{2} \mathrm{O}_{4}(g) \longrightarrow 2 \mathrm{NO}_{2}(g)\) e. \(\mathrm{CaCO}_{3}(s) \longrightarrow \mathrm{CaCO}(s)+\mathrm{CO}_{2}(g)\)

The enthalpy change for the reaction $$\mathrm{CH}_{4}(g)+2 \mathrm{O}_{2}(g) \longrightarrow \mathrm{CO}_{2}(g)+2 \mathrm{H}_{2} \mathrm{O}(l)$$ is \(-891 \mathrm{kJ}\) for the reaction \(a s\) written. a. What quantity of heat is released for each mole of water formed? b. What quantity of heat is released for each mole of oxygen reacted?
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