10 g of ice at 10^∘ C is mixed with 100 g of water at 50^∘ C in a calorimeter. The final tempe

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10 g of ice at 10^∘ C is mixed with 100 g of water at 50^∘...

$10 \mathrm{~g}$ of ice at $10^{\circ} \mathrm{C}$ is mixed with $100 \mathrm{~g}$ of water at $50^{\circ} \mathrm{C}$ in a calorimeter. The final temperature of the mixture is: (a) $3.82^{\circ} \mathrm{C}$ (b) $38.2^{\circ} \mathrm{C}$ (c) $4.2^{\circ} \mathrm{C}$ (d) $42^{\circ} \mathrm{C}$

$10 \mathrm{~g}$ of ice at $10^{\circ} \mathrm{C}$ is mixed with $100 \mathrm{~g}$ of water at $50^{\circ} \mathrm{C}$ in a calorimeter. The final temperature of the mixture is:
(a) $3.82^{\circ} \mathrm{C}$
(b) $38.2^{\circ} \mathrm{C}$
(c) $4.2^{\circ} \mathrm{C}$
(d) $42^{\circ} \mathrm{C}$

Key Concepts

Calorimetry

Calorimetry involves measuring the heat exchanged in physical and chemical processes. It is used to determine energy changes when substances at different temperatures are mixed, reaching a state of thermal equilibrium.

Specific Heat Capacity

Specific heat capacity is the amount of heat required to raise the temperature of a unit mass of a substance by one degree. This concept is fundamental in calculating the thermal energy changes when substances are heated or cooled.

Latent Heat of Fusion

Latent heat of fusion is the energy absorbed or released when a substance undergoes a phase change from solid to liquid (or vice versa) at a constant temperature. It is key in understanding the energy requirements for melting ice without a temperature change.

Thermal Equilibrium

Thermal equilibrium is reached when all components in a system have the same temperature and no further net heat exchange occurs. This state is the result of energy redistribution and is the final condition after mixing substances with different initial temperatures.

Conservation of Energy

The principle of conservation of energy states that energy cannot be created or destroyed, only transferred or converted. In calorimetry, this principle is applied by equating the heat lost by the warmer substance to the heat gained by the cooler substance until equilibrium is achieved.

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