to get the heat released or absorbed,
Q = mc(T2-T1)
m = mass of substance
c = specific heat capacity
T2 = final temperature
T1 = initial temperature
**note: if Q is (-), heat is released and if (+), heat is absorbed
now we can only apply this to substances that did not change its phase, but in the problem, we see that phase change occurs. from vapor->liquid
thus we need another data called Latent Heat of Vaporization to calculate for the heat required to change its phase:
H = m(Lv)
m = mass
Lv = Latent Heat of Vaporization
**note: H is (-) if heat is released and (+) if heat is absorbed
Q, total = Q1 + H + Q2
Q,total = mc(T2-T1) + mLv + mc(T3-T2)
T3 = 90 deg
T2 = 100 deg (boiling point of water)
T1 = 120 deg
since heat is removed, H is negative. now for every 1 kg of steam,
Q,total = 1*(c)*(100-120) - 1*Lv + 1*(c)*(90-100)
Q,total = -20*c - 10*c - Lv
Q,total = -30*c - Lv
now you look for the specific heat of water, c, and latent heat of vaporization, Lv. note that units must already be in Joules or calories.
hope this helps~ :)
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