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Chapter 6: Problem 33
A gas absorbs 45 kJ of heat and does 29 kJ of work. Calculate \(\Delta E .\)
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The enthalpy of combustion of \(\mathrm{CH}_{4}(g)\) when $\mathrm{H}_{2} \mathrm{O}(l)$ is formed is \(-891 \mathrm{kJ} / \mathrm{mol}\) and the enthalpy of combustion of \(\mathrm{CH}_{4}(g)\) when \(\mathrm{H}_{2} \mathrm{O}(g)\) is formed is $-803 \mathrm{kJ} / \mathrm{mol}$ . Use these data and Hess's law to determine the enthalpy of vaporization for water.
For each of the following situations a-c, use choices i-iii to complete the statement: "The final temperature of the water should be.." i. between \(50^{\circ} \mathrm{C}\) and \(90^{\circ} \mathrm{C}\) . ii. \(50^{\circ} \mathrm{C}\) . iii. between \(10^{\circ} \mathrm{C}\) and \(50^{\circ} \mathrm{C}\) . a. 100.0 -g sample of water at \(90^{\circ} \mathrm{C}\) is added to a 100.0 -g sample of water at \(10^{\circ} \mathrm{C}\) . b. A 100.0 -g sample of water at \(90^{\circ} \mathrm{C}\) is added to a $500.0 . \mathrm{g}\( sample of water at \)10^{\circ} \mathrm{C} .$ c. You have a Styrofoam cup with 50.0 \(\mathrm{g}\) of water at $10^{\circ} \mathrm{C}\( . You add a 50.0 -g iron ball at \)90^{\circ} \mathrm{C}$ to the water.
A coffee-cup calorimeter initially contains 125 \(\mathrm{g}\) water at \(24.2^{\circ} \mathrm{C} .\) Potassium bromide \((10.5 \mathrm{g}),\) also at \(24.2^{\circ} \mathrm{C},\) is added to the water, and after the KBr dissolves, the final temperature is \(21.1^{\circ} \mathrm{C}\) . Calculate the enthalpy change for dissolving the salt in \(\mathrm{J} / \mathrm{g}\) and $\mathrm{kJ} / \mathrm{mol}$ . Assume that the specific heat capacity of the solution is 4.18 \(\mathrm{J} / \mathrm{C} \cdot \mathrm{g}\) and that no heat is transferred to the surroundings or to the calorimeter.
Explain why aluminum cans are good storage containers for soft drinks. Styrofoam cups can be used to keep coffee hot and cola cold. Why is this?
Hydrogen gives off \(120 . \mathrm{J} / \mathrm{g}\) of energy when burned in oxygen, and methane gives off \(50 . \mathrm{J} / \mathrm{g}\) under the same circumstances. If a mixture of 5.0 \(\mathrm{g}\) hydrogen and \(10 . \mathrm{g}\) methane is burned, and the heat released is transferred to 50.0 \(\mathrm{g}\) water at \(25.0^{\circ} \mathrm{C},\) what final temperature will be reached by the water?
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