Question

Calculate the energy needed to raise the temperature of 18.0g of water from 10.0C to 40.0C. The specific heat of water is 4.18 J/gC. *

Answer 1

Answer:

The energy needed to raise the temperature 18.0 grams of water is from 10.0°C to 40.0°C is 2,257.2 Joules.

Explanation:

$Q=mc\Delta T=mc\times (T_2-T_1)$

Where:

Q = heat absorbed  or heat lost

c = specific heat of substance

m = Mass of the substance

ΔT = change in temperature of the substance

$T_1,T_2$ : Initial and final temperature of the substance

We have mass of water = m = 18.0 g

Specific heat of water= c = 4.18 J/g°C

Initial and final temperature of the water= $T_1=10.0^oC$

Final temperature of the water= $T_2=40.0^oC$

Heat absorbed by the water:

$Q=18.0g\times 4.18/g^oC\times (40.0^oC-10.0^oC)=2,257.2 J$

The energy needed to raise the temperature 18.0 grams of water is from 10.0°C to 40.0°C is 2,257.2 Joules.