Chapter 6: Problem 18
Explain why oceanfront areas generally have smaller temperature fluctuations than inland areas.
Chapter 6: Problem 18
Explain why oceanfront areas generally have smaller temperature fluctuations than inland areas.
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Get started for freeThe equation for the fermentation of glucose to alcohol and carbon dioxide is: $$ \mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}(a q) \longrightarrow 2 \mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}(a q)+2 \mathrm{CO}_{2}(g) $$ The enthalpy change for the reaction is \(-67 \mathrm{kJ} .\) Is this reaction exothermic or endothermic? Is energy, in the form of heat, absorbed or evolved as the reaction occurs?
A 30.0 -g sample of water at \(280 . \mathrm{K}\) is mixed with 50.0 g water at \(330 . \mathrm{K}\) . Calculate the final temperature of the mixture assuming no heat loss to the surroundings.
A sample of nickel is heated to \(99.8^{\circ} \mathrm{C}\) and placed in a coffeecup calorimeter containing 150.0 \(\mathrm{g}\) water at \(23.5^{\circ} \mathrm{C}\) . After the metal cools, the final temperature of metal and water mixture is \(25.0^{\circ} \mathrm{C}\) . If the specific heat capacity of nickel is 0.444 \(\mathrm{J} /^{\prime} \mathrm{C} \cdot \mathrm{g}\) what mass of nickel was originally heated? Assume no heat loss to the surroundings.
Calculate \(q, w, \Delta E,\) and \(\Delta H\) for the process in which 88.0 g of nitrous oxide (laughing gas, \(\mathrm{N}_{2} \mathrm{O} )\) is cooled from \(165^{\circ} \mathrm{C}\) to \(55^{\circ} \mathrm{C}\) at a constant pressure of 5.00 \(\mathrm{atm} .\) The molar heat capacity for \(\mathrm{N}_{2} \mathrm{O}(g)\) is 38.7 \(\mathrm{J} /^{\prime} \mathrm{C} \cdot\) mol.
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?
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