A. The final temperature of the system is 0°C.
B. The amount of ice (if any) remaining is 0.0331 g
C. The initial temperature of the water that would be enough to just barely melt all of the ice is 20.57 °C.
<h3>What is specific heat?</h3>
The specific heat is the amount of heat required to change the temperature by 1°C. It is denoted by C.
Heat lost or gained is represented as
Q = m C ΔT
Given, Mass of ice, mice = 9x10⁻² kg, Mass of water, mw =0.35 kg, T = 13 °C
A. If ice is in excess, final water temperature will be 0°C.
B. Specific heat of water Cp = 1000 cal/kg°C
Latent heat of ice L = 80 kcal/kg
In that case, heat lost by water =Heat gain by ice
Q = mCp x dT = mL
0.35 x 1000 x 13 = m x 80 x 1000
m = 0.0569 kg of ice.
The gram of ice remaining = 0.09 - 0.0569
= 0.0331 gram of ice.
Thus, the amount of ice remaining is 0.0331 g
C. Heat required to melt 90 gram of ice, Q mL
Q = 90 x 80 = 7200 cal.
If the initial temperature of water needed = T,
mCp x dT = mL
350 x T = 7200
T = 20.57 °C
Thus, the initial temperature of the water that would be enough to just barely melt all of the ice is 20.57 °C.
Learn more about specific heat.
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