Answer:
Final temperature is 71·31 °C
Step-by-step explanation:
The amount of heat change in a body for a change in temperature of ΔT is m×s×ΔT
where
m is the mass of the substance
s is the heat capacity of the substance
ΔT is the temperature difference
At constant temperature the amount of heat for fusion of ice is m×L
where
m is the mass of the substance
L is the latent heat of the substance
Let the final temperature be T
As there is no heat loss to the surrounding
∴ The heat gained by the ice = The heat lost by the water
As the density of the water is 1 g/ml
∴ The mass of 90ml water will be 90 g
Heat gained by the ice when it is attained at 0°C and converted to water is
(10×2·08×11) + 10×6 = 288·8
But the heat loss by the water when water attains 0°C will be 90×4·18×80 = 30,096
As the heat loss is more therefore there will be further rise in temperature
Now the heat gain = 288·88 + 10×4·18×T
heat loss = 90×4·18×(80-T)
Here in the case of heat loss as we are already mentioning that the heat is lost so we are taking the magnitude of the heat change otherwise it would be 90×4·18×(T-80)
288·88 + 41·8×T = 9×41·8×(80-T)
41·8×9×80 - 288·8 = 10×41·8×T
∴T=71·31 °C