What is the heat change when a 53.5 g sample of water [C_water = 4.184 J/(g $\degree$C)] is cooled from 98.0 $\degree$C to 23.2 $\degree$C?

Question

Quizplus · Accepted Answer

The heat change can be calculated using the specific heat capacity of water, the mass of water, and the change in temperature:

q = mcΔT

where q is the heat change, m is the mass of the water, c is the specific heat capacity of water, and ΔT is the change in temperature.

Substituting the given values, we get:

q = (53.5 g)(4.184 J/(g°C))(23.2°C - 98.0°C) = -1.67 x 10^4 J

The negative sign indicates that the water lost heat, which makes sense since it was cooled. Therefore, the best choice is (B).

What Is the Heat Change When a 53 °\degree° C)] Is Cooled from 98