Question
A 75 g cube of ice at $-10.0^{\circ} \mathrm{C}$ is placed in $0.500 \mathrm{kg}$ of water at $50.0^{\circ} \mathrm{C}$ in an insulating container so that no heat is lost to the environment. Will the ice melt completely? What will be the final temperature of this system?
Step 1
0^{\circ} \mathrm{C}$ to $0.0^{\circ} \mathrm{C}$. The formula for this is $Q = mc\Delta T$, where $m$ is the mass of the ice, $c$ is the specific heat capacity of ice, and $\Delta T$ is the change in temperature. Show more…
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A 75.0-g cube of ice at -10.0°C is placed in 0.790 kg of water at 50.0°C in an insulating container so that no heat is lost to the environment. Specific heat capacity (15.0°C) of water is 4.186 kJ/(kg·K) and that of ice (0°C) is 2.10 kJ/(kg·K) and heat of fusion of water is 333.7 kJ/kg. What will be the final temperature of this system?
You drop $500 \mathrm{g}$ of solid ice at $-35^{\circ} \mathrm{C}$ into a bucket of water $(1200 \mathrm{g})$ at $45^{\circ} \mathrm{C}$. Eventually, the ice all melts, and the entire system comes into thermal equilibrium. Find the final temperature of the system.
Temperature and Heat
Phases of Matter and Phase Changes
You drop 500 g. of solid ice at -35 deg.C. into a bucket of water (1200 g.) at 45 deg. C. Eventually, the ice all melts, and the entire system comes into thermal equilibrium. Find the final temperature of the system?
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