A 32.0 g sample of liquid water at 21.0^°C absorbs 2276 J of heat energy.What will be the final temperature of the water? The specific heat of liquid water is 4.185 J/g^°C.

Question

Quizplus · Accepted Answer

We can use the formula:

q = m x c x ΔT

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

We can rearrange the formula to solve for ΔT:

ΔT = q / (m x c)

Substituting the given values, we get:

ΔT = 2276 J / (32.0 g x 4.185 J/g°C)

ΔT ≈ 17.0°C

Since the initial temperature was 21.0°C, the final temperature will be:

Final temperature = 21.0°C - 17.0°C = 38.0°C

Therefore, the best choice is C.

A 320 G Sample of Liquid Water at 21