Question

How much heat is required to raise the temperature of 65.8 grams of water from 31.5ºC to 46.9ºC?

Answer 1

Answer: 1,013.32 cal × 4.18 J/cal = 4,235.68 J

Step-by-step explanation:

1) Data:

Water ⇒ C = 1 cal/g°C

m = 65.8 g

Ti = 31.5°C

Tf = 36.9°C

Heat, Q = ?

2) Formula:

Q = mCΔT

3) Calculations:

Q = 65.8g × 1 cal/g°C × (46.9°C - 31.5°C) = 1,013.2 cal

4) You can convert from calories to Joules using the conversion factor:

1 cal = 4.18 J

⇒ 1,013.32 cal × 4.18 J/cal = 4,235.68 J