Slide 1Slide 2Slide 3Slide 4Slide 5Slide 6Slide 7Slide 8•A 55.0 g piece of metal was heated in boiling water to a temperature of 99.8oC and dropped into an insulated beaker with 225 mL of water (d = 1.00 g/ml) at 21.0 oC. The final temperature of the metal and water is 23.1oC. Calculate the specific heat of the metal assuming that no heat was lost to the surroundings.•Octane, C8H18, a primary constituent of gasoline, burns in air. •C8H18(l) + 25/2 O2(g) 8 CO2(g) + 9 H2O(l)•Suppose that a 1.00 g sample of octane is burned in a calorimeter that contains 1.20 kg of water. The temperature of the water and the bomb rises from 25.00oC to 33.20oC. If the specific heat of the bomb, Cbomb, is known to be 837 J/oC, calculate the molar heat of reaction of C8H18.•Calculate the amount of heat required to convert 500 g of ice at 50oC to steam at 200oC.••specific heat of ice 2.06 J/goC •specific heat of water 4.184 J/goC •specific heat of steam 2.0 J/goC •heat of fusion 333 J/g•heat of vaporization 2226 J/g•A quantity of ice at 0oC is added to 90.0 g of water at 80oC. After the ice melted, the temperature of the water was 25oC. How much ice was added?•50.0 g of ice at -20.0 oC are added to 342.0 g of water at 86.0 oC. What will be the final temperature of the
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