A 100 g sample of a liquid with a specific heat
of 2 J/g · C absorbs 4000 J of heat energy. If
the sample started at 30
◦
C , what is the final
temperature? No phase change took place.
To find the final temperature, we can use the equation:
Q = m * c * ΔT
Where:
Q = heat energy absorbed (in joules)
m = mass of the sample (in grams)
c = specific heat capacity (in J/g · °C)
ΔT = change in temperature (in °C)
We know that Q = 4000 J, m = 100 g, c = 2 J/g · °C, and the initial temperature (T1) = 30 °C.
Now, let's rearrange the equation to solve for ΔT:
ΔT = Q / (m * c)
Substituting the known values:
ΔT = 4000 J / (100 g * 2 J/g · °C)
ΔT = 4000 J / (200 g · °C)
ΔT = 20 °C
To find the final temperature (T2), we add the change in temperature to the initial temperature:
T2 = T1 + ΔT
T2 = 30 °C + 20 °C
T2 = 50 °C
Therefore, the final temperature of the liquid sample is 50°C.