Chapter 5: Problem 19
(a) What is work? (b) How do we determine the amount of work done, given the force associated with the work?
Chapter 5: Problem 19
(a) What is work? (b) How do we determine the amount of work done, given the force associated with the work?
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Get started for freeThe two common sugars, glucose \(\left(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\right)\) and sucrose \(\left(\mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}\right)\), are both carbohydrates. Their standard enthalpies of formation are given in Table \(5.3\). Using these data, (a) calculate the molar enthalpy of combustion to \(\mathrm{CO}_{2}(g)\) and \(\mathrm{H}_{2} \mathrm{O}(l)\) for the two sugars; (b) calculate the enthalpy of combustion per gram of each sugar; (c) determine how your answers to part (b) compare to the average fuel value of carbohydrates discussed in Section \(5.8\).
Ammonia \(\left(\mathrm{NH}_{3}\right)\) boils at \(-33^{\circ} \mathrm{C} ;\) at this temperature it has a density of \(0.81 \mathrm{~g} / \mathrm{cm}^{3}\). The enthalpy of formation of \(\mathrm{NH}_{3}(g)\) is \(-46.2 \mathrm{~kJ} / \mathrm{mol}\), and the enthalpy of vaporization of \(\mathrm{NH}_{3}(l)\) is \(23.2 \mathrm{~kJ} / \mathrm{mol}\). Calculate the enthalpy change when \(1 \mathrm{~L}\) of liquid \(\mathrm{NH}_{3}\) is burned in air to give \(\mathrm{N}_{2}(g)\) and \(\mathrm{H}_{2} \mathrm{O}(g)\). How does this compare with \(\Delta H\) for the complete combustion of \(1 \mathrm{~L}\) of liquid methanol \(\mathrm{CH}_{3} \mathrm{OH}(l) ?\) For \(\mathrm{CH}_{3} \mathrm{OH}(\mathrm{l})\), the density at \(25^{\circ} \mathrm{C}\) is \(0.792 \mathrm{~g} / \mathrm{cm}^{3}\), and \(\Delta H_{f}^{\circ}\) equals \(-239 \mathrm{~kJ} / \mathrm{mol}\).
Naphthalene \(\left(\mathrm{C}_{10} \mathrm{H}_{8}\right)\) is a solid aromatic compound often sold as mothballs. The complete combustion of this substance to yield \(\mathrm{CO}_{2}(g)\) and \(\mathrm{H}_{2} \mathrm{O}(l)\) at \(25^{\circ} \mathrm{C}\) yields \(5154 \mathrm{~kJ} / \mathrm{mol}\). (a) Write balanced equations for the formation of naphthalene from the elements and for its combustion. (b) Calculate the standard enthalpy of formation of naphthalene.
A coffee-cup calorimeter of the type shown in Figure \(5.17\) contains \(150.0 \mathrm{~g}\) of water at \(25.1^{\circ} \mathrm{C}\). A \(121.0\) -g block of copper metal is heated to \(100.4^{\circ} \mathrm{C}\) by putting it in a beaker of boiling water. The specific heat of \(\mathrm{Cu}(s)\) is \(0.385 \mathrm{~J} / \mathrm{g}-\mathrm{K} .\) The \(\mathrm{Cu}\) is added to the calorimeter, and after a time the contents of the cup reach a constant temperature of \(30.1^{\circ} \mathrm{C}\). (a) Determine the amount of heat, in \(J\), lost by the copper block. (b) Determine the amount of heat gained by the water. The specific heat of water is \(4.18 \mathrm{~J} / \mathrm{g}-\mathrm{K} .\) (c) The difference between your answers for (a) and (b) is due to heat loss through the Styrofoam \(^{8}\) cups and the heat necessary to raise the temperature of the inner wall of the apparatus. The heat capacity of the calorimeter is the amount of heat necessary to raise the temperature of the apparatus (the cups and the stopper) by \(1 \mathrm{~K}\). Calculate the heat capacity of the calorimeter in J/K. (d) What would be the final temperature of the system if all the heat lost by the copper block were absorbed by the water in the calorimeter?
Methanol \(\left(\mathrm{CH}_{3} \mathrm{OH}\right)\) is used as a fuel in race cars. (a) Write a balanced equation for the combustion of liquid methanol in air. (b) Calculate the standard enthalpy change for the reaction, assuming \(\mathrm{H}_{2} \mathrm{O}(g)\) as a product. (c) Calculate the heat produced by combustion per liter of methanol. Methanol has a density of \(0.791 \mathrm{~g} / \mathrm{mL}\) (d) Calculate the mass of \(\mathrm{CO}_{2}\) produced per \(\mathrm{kJ}\) of heat emitted.
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