Answer:
The final temperature is 36.24 °C
Explanation:
Step 1: Data given
Mass of copper = 155.0 grams
Initial temperature of copper = 179.0 °C
Mass of water = 250.0 grams
The initial temperature of water = 28.1 °C
The specific heat of copper = 0.385 J/g°C
The specific heat of water = 4.184 J/g°C
Step 2: Calculate the final temperature
Qlost = -Qgained
Q =m*c*ΔT
Qcopper = -Qwater
m(copper)*c(copper)*ΔT(copper) = -m(water)*c(water)*ΔT(water)
⇒with mass of copper = 155.0 grams
⇒with c(copper) = the specific heat of copper = 0.385 J/g°C
⇒with ΔT = the change of temperature of copper = T2 - T1 = T2 - 179.0°C
⇒with mass water = 250.0 grams
⇒with c(water) = the specific heat of water = 4.184 J/g°C
⇒with ΔT = with ΔT = the change of temperature of copper = T2 - T1 = T2 - 28.1 °C
155.0 * 0.385 * (T2 - 179.0°C) = - 250 * 4.184 *  (T2 - 28.1 °C)
T2 = 36.24 °C
The final temperature is 36.24 °C
