Answer:
Final Temperature = 298.28 K (25.28°C)
Explanation:
First off, lets least out our parameters (What we were given).
Mass of Tea (Mt) = 237g
Initial temp. of tea (T1) = 100 °C + 273 = 373K (Converting to Kelvin)
Mass of Ice (Mi) = 2.50 × 10² g = 250g
Initial temp. of ice (T1) = -18 °C + 273 = 255K (Converting to Kelvin)
If all the ice melts
Amount of Heat required to melt the ice [H] = Amount of heat required to raise its temperature to 0°C or 273K (Melting point) [H1] + Heat of Fusion [H2]
H1 = MiCΔT
ΔT = T2 - T1 = 255 - 273 = -18K
C = 2.09 J/gK (Specific Heat capacity of Ice)
H1 = 250 * 2.09 * (-18)
H1 = -9405 J
H2 = m·ΔHf
ΔHf = Heat of fusion of ice = 334 J/g
H2 = 250 * 334
H2 = 83500 J
Amount of Heat required to melt the ice [H] = H1 + H2
H = -9405 + 83500 = 74095 J
This means the heat was able to supply 74095 J to the tea.
Final temperature is calculated from:
H = MtCΔT
ΔT = H/MtC
ΔT = 74095/(237 * 4.184)
ΔT = 74095 / 991.61
ΔT = 74.72 K
With a temperature difference of 74. 72 K
Final temperature = Initial temperature - 74.72K
T2 = 373 - 74.74
T2 = 298.28 K (25.28°C)
