Question

Using the specific heat of water (4.2 J/°C/g) and the conversion factor 1 mL of water = 1 g or water, calculate the following:

The energy required to heat 100 mL of water by 40°C:

Answer 1

To calculate the energy required to heat 100 mL of water by 40°C, one uses the specific heat of water, which is 4.184 J/g°C. The calculation results in 16736 joules of energy needed.

Step-by-step explanation:

The student is asking how to calculate the energy required to heat 100 mL of water by 40°C using the specific heat of water. Given that the specific heat capacity of water is approximately 4.184 J/g°C, and knowing that 1 mL of water has a mass of about 1 g, we can use the formula:

Energy (J) = mass (g) × specific heat (J/g°C) × temperature change (°C)

Substituting the given values:

Energy = 100 g × 4.184 J/g°C × 40°C

Energy = 418.4 J × 40°C

Energy = 16736 J

Therefore, 16736 joules of energy are required to heat 100 mL of water by 40°C.