1) energy in the amount of 420 J is added to a 35 g sample of water at a temperature of 10.0degrees celsiuswhat is the final temperature of the water? (specific heat of water is 4.18 j/gk)2) If 980000 J of energy as heat is transfered into 6200 grams of water at 291 K, what will the final temperature of the water be? Specific heat of water is 4.18 j/gk3) how much energy as heat must be transferred to raise the temperature of a 55 gram sample of aluminum from 22.4 degrees celsius to 94.6 degrees celsius? the specific heat of aluminum is 0.897 j/gknote that a temperature change of 1 degree celsius is the same temperature change of 1 k because the sizes of the degree divisions on both scales are equal
1) energy in the amount of 420 J is added to a 35 g sample of water at a temperature of 10.0degrees celsiuswhat is the final temperature of the water? (specific heat of water is 4.18 j/gk) dH m C dT 420J (35 g) (4.18)(dT) dT 2.9 c rise final temp 12.9C 2) If 980000 J of energy as heat is transfered into 6200 grams of water at 291 K, what will the final temperature of the water be? Specific heat of water is 4.18 j/gk dH m C dT 980,000J (6200 g) (4.18)(dT) dT 37.8 K rise final temp 12.9C + 291 your answer, rounded to 1 degree Kelvin 329 Kelvin 3) how much energy as heat must be transferred to raise the temperature of a 55 gram sample of aluminum from 22.4 degrees celsius to 94.6 degrees celsius? the specific heat of aluminum is 0.897 j/gk dH m C dT dH 55g (0.897) (72.2K) dH 3562 Joules you may be expected to round off
