Find the increase in entropy of 1.00 kg of ice originally at 0 degrees Centigrade, that is melted to form water

Here's how to calculate the increase in entropy:

To find the increase in entropy ($\Delta S$) during a phase change at constant temperature, we use the formula:

$$\Delta S = \frac{Q}{T}$$

where $Q$ is the heat absorbed and $T$ is the absolute temperature in Kelvin.

For melting, the heat absorbed ($Q$) is given by:

$$Q = mL_f$$

where $m$ is the mass and $L_f$ is the latent heat of fusion.

Given values:

• Mass of ice, $m = 1.00 \text{ kg}$
• Temperature, $T_C = 0^\circ \text{C}$
• Latent heat of fusion of water, $L_f = 334 \times 10^3 \text{ J/kg}$ (standard value)