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1:11 File Details CHEM 120 - Fund of Col Chem #3765 - Spring 2022 2. Use the calculated value from #1 (above) and the mass of ice to calculate the heat of fusion per gram. (answer: 83.2 calories/g) 3. If the accepted value for the heat of fusion of ice is 80.0 calories-per- gram, calculate a) the error (the difference) = b) the % error: [(difference) + 80.0] (100) = % error 4. Convert calories-per-gram (#2, above) into kilocalories-per-mole. (recall: 1 kilocalorie - 1000 calories, 1 mole ice-18 grams) (answer: 1.50 kcal/mole) 5. Using the accepted value for the heat of fusion, 80.0 calories-per-gram, calculate the heat energy needed to melt a 24.0 gram ice cube. (answer: 1920 calories) 6. On a hot summer day, you might like to cool down a hot beverage with ice. The mass of a beverage is 355 grams and the temperature is 34.0°C. (Assume the beverage is primarily water.) a) How many calories of heat must be removed to bring the temperature down to 0.0°C? (answer: 12,070 12,100 cal.) b) How many grams of ice will be needed to cool the beverage to 0°C? (use 80.0 calories-per-gram) (answer: 151 grams) * Previous Next > 13 Dashboard Inbox Calendar To Do Notifications 64