A 100-g cube of ice at 0^∘ C is dropped into 1.0 kg of water that was originally at 80^∘ C. Wha

step 1 So here the equation would be the mass of the ice multiplied by the latent heat of formation plu

A 100-g cube of ice at 0^∘ C is dropped into 1.0 kg of...

A $100-\mathrm{g}$ cube of ice at $0^{\circ} \mathrm{C}$ is dropped into $1.0 \mathrm{~kg}$ of water that was originally at $80^{\circ} \mathrm{C}$. What is the final temperature of the water after the ice has melted?

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Key Concepts

Latent Heat of Fusion

Latent heat of fusion is the energy needed to change a substance from a solid to a liquid at its melting point without changing its temperature. This concept is essential when considering phase changes, such as ice melting into water.

Thermal Equilibrium

Thermal equilibrium is the condition reached when objects in thermal contact no longer exchange heat because they have the same temperature. Analyzing thermal equilibrium allows us to determine the final temperature of a system after heat transfer processes have concluded.

Conservation of Energy

This principle states that energy cannot be created or destroyed, only transformed from one form to another. In thermal problems, it means that the total amount of heat lost by warmer substances is equal to the total amount of heat gained by cooler substances in an isolated system.

Specific Heat Capacity

Specific heat capacity is the amount of energy required to raise the temperature of one kilogram of a substance by one degree Celsius. It plays a crucial role in determining how a substance's temperature changes when it absorbs or loses heat.

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