1. How much heat, in calories, is needed to raise the temperature of 415 grams of water from 25.5°C to 65.2°C? (3 points for set-up: 1 for the answer)

16475.5 calories.

Explanation:

The following data were obtained from the question:

Mass (M) = 415 g

Initial temperature (T1) = 25.5 °C

Final temperature (T2) = 65.2 °C

Specific heat capacity (C) = 1 cal/g°C

Heat (Q) required =?

Next, we shall determine the change in temperature of the water. This can be obtained as follow:

Initial temperature (T1) = 25.5 °C

Final temperature (T2) = 65.2 °C

Change in temperature (ΔT) =.?

Change in temperature (ΔT) = T2 – T1

Change in temperature (ΔT) = 65.2 – 25.5

Change in temperature (ΔT) = 39.7 °C

Finally, we shall determine the heat required to raise the temperature of the water as follow:

Mass (M) = 415 g

Specific heat capacity (C) = 1 cal/g°C

Change in temperature (ΔT) = 39.7 °C

Heat (Q) required =?

Q = MCΔT

Q = 415 × 1 × 39.7

Q = 16475.5 calories.

Therefore, the heat required to raise the temperature of the water is 16475.5 calories.

c is the answer because when something is left after something evaporates that shows the chemical change.

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