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Chapter 6: Problem 78

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, \(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{Cl}(\mathrm{g})\). e. the enthalpy of combustion of liquid benzene, \(\mathrm{C}_{6} \mathrm{H}_{6}(l)\). f. the enthalpy of solution of solid ammonium bromide.

Short Answer

Expert verified
a. \(4 Al(s) + 3 O_2(g) \rightarrow 2 Al_2O_3(s)\) b. \(C_2H_5OH(l) + 3 O_2(g) \rightarrow 2 CO_2(g) + 3 H_2O(l)\) c. \(NaOH(aq) + HCl(aq) \rightarrow NaCl(aq) + H_2O(l)\) d. \(2 C(s) + 3 H_2(g) + Cl_2(g) \rightarrow C_2H_3Cl(g)\) e. \(C_6H_6(l) + \frac{15}{2}O_2(g) \rightarrow 6 CO_2(g) + 3 H_2O(l)\) f. \(NH_4Br(s) \rightarrow NH_4^+(aq) + Br^-(aq)\)

Step by step solution

01

Reaction

The formation of solid aluminum oxide from its elements, aluminum and oxygen, can be represented by the following balanced equation: \(4 Al(s) + 3 O_2(g) \rightarrow 2 Al_2O_3(s)\) b. Enthalpy of Combustion of Ethanol:
02

Reaction

The combustion of liquid ethanol, in the presence of oxygen gas, results in the formation of carbon dioxide and water. The balanced equation is: \(C_2H_5OH(l) + 3 O_2(g) \rightarrow 2 CO_2(g) + 3 H_2O(l)\) c. Enthalpy of Neutralization of Sodium Hydroxide and Hydrochloric Acid:
03

Reaction

The neutralization reaction between sodium hydroxide and hydrochloric acid forms salt (sodium chloride) and water. The balanced equation is: \(NaOH(aq) + HCl(aq) \rightarrow NaCl(aq) + H_2O(l)\) d. Formation Enthalpy of Vinyl Chloride:
04

Reaction

The formation of gaseous vinyl chloride from its elements, carbon, hydrogen, and chlorine, can be represented by the following balanced equation: \(2 C(s) + 3 H_2(g) + Cl_2(g) \rightarrow C_2H_3Cl(g)\) e. Enthalpy of Combustion of Benzene:
05

Reaction

The combustion of liquid benzene in the presence of oxygen gas results in the formation of carbon dioxide and water. The balanced equation for this reaction is: \(C_6H_6(l) + \frac{15}{2}O_2(g) \rightarrow 6 CO_2(g) + 3 H_2O(l)\) f. Enthalpy of Solution of Ammonium Bromide:
06

Reaction

The dissolution of solid ammonium bromide in water can be represented by the following equation: \(NH_4Br(s) \rightarrow NH_4^+(aq) + Br^-(aq)\)

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Most popular questions from this chapter

Consider the following cyclic process carried out in two steps on a gas: Step 1: \(45 \mathrm{~J}\) of heat is added to the gas, and \(10 . \mathrm{J}\) of expansion work is performed. Step \(2: 60 . \mathrm{J}\) of heat is removed from the gas as the gas is compressed back to the initial state. Calculate the work for the gas compression in Step \(2 .\)

Consider the reaction \(\mathrm{B}_{2} \mathrm{H}_{6}(g)+3 \mathrm{O}_{2}(g) \longrightarrow \mathrm{B}_{2} \mathrm{O}_{3}(s)+3 \mathrm{H}_{2} \mathrm{O}(g) \quad \Delta H=-2035 \mathrm{~kJ}\) Calculate the amount of heat released when \(54.0 \mathrm{~g}\) of diborane is combusted.

Are the following processes exothermic or endothermic? a. When solid \(\mathrm{KBr}\) is dissolved in water, the solution gets colder. b. Natural gas \(\left(\mathrm{CH}_{4}\right)\) is burned in a furnace. c. When concentrated \(\mathrm{H}_{2} \mathrm{SO}_{4}\) is added to water, the solution gets very hot. d. Water is boiled in a teakettle.

A biology experiment requires the preparation of a water bath at \(37.0^{\circ} \mathrm{C}\) (body temperature). The temperature of the cold tap water is \(22.0^{\circ} \mathrm{C}\), and the temperature of the hot tap water is \(55.0^{\circ} \mathrm{C}\). If a student starts with \(90.0 \mathrm{~g}\) cold water, what mass of hot water must be added to reach \(37.0^{\circ} \mathrm{C}\) ?

A \(5.00-\mathrm{g}\) sample of aluminum pellets (specific heat capacity \(=\) \(0.89 \mathrm{~J} /{ }^{\circ} \mathrm{C} \cdot \mathrm{g}\) ) and a \(10.00-\mathrm{g}\) sample of iron pellets (specific heat capacity \(=0.45 \mathrm{~J} /{ }^{\circ} \mathrm{C} \cdot \mathrm{g}\) ) are heated to \(100.0^{\circ} \mathrm{C}\). The mixture of hot iron and aluminum is then dropped into \(97.3 \mathrm{~g}\) water at \(22.0^{\circ} \mathrm{C}\). Calculate the final temperature of the metal and water mixture, assuming no heat loss to the surroundings.
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