A 5.00-g sample of liquid water at 25.0 °C is heated by the addition of 84.0 J of energy. The final temperature of the water is __________ °C. The specific heat capacity of liquid water is 4.18 J/g-K.

Question

Quizplus · Accepted Answer

To solve the problem, we can use the formula:
q = mcΔT
where q is the energy absorbed by the water, m is the mass of the water, c is the specific heat capacity of water and ΔT is the change in temperature.
Rearranging the formula to solve for ΔT, we get:
ΔT = q/mc
Substituting the given values, we get:
ΔT = 84.0 J / (5.00 g × 4.18 J/g-K) = 3.99 K
Therefore, the final temperature is:
25.0 °C + 3.99 K = 29.0 °C
Thus, the best choice is D.

A 500-G Sample of Liquid Water at 25