Let's solve the problem step by step as per Chegg guidelines: --- **Given:** - Mass of ice, \( m = 300\, \text{g} = 0.3\, \text{kg} \) - Initial temperature = 0°C - Final state: 300 g of water at 0°C - Latent heat of fusion of ice, \( L_f = 334\, \text{kJ/kg} \) --- ### **Step 1: Understanding the Process** To convert 300 g of ice at 0°C to 300 g of water at 0°C, only the phase change (melting) occurs; temperature does not change. So, the heat required is for the phase change (melting) only. --- ### **Step 2: Calculating the Required Heat** The heat required for melting: \[ Q = m \times L_f \] \[ Q = 0.3\, \text{kg} \times 334\, \text{kJ/kg} \] \[ Q = 100.2\, \text{kJ} \] --- **Final Answer:** \[ \boxed{100\, \text{kJ}} \] So, the answer is **D. 100 kJ**.

Certainly! Here's the detailed explanation for both steps in words: --- **Step 1: Understanding the process** The problem involves converting ice at 0°C into water at 0°C. Since the temperature remains constant at 0°C, the only change happening is the phase change from ice to water. No additional heating is required to raise the temperature because the ice is already at 0°C and the final water is also at 0°C. Therefore, the energy needed is solely for melting the ice, which involves overcoming the latent heat of fusion. --- **Step 2: Calculating the heat energy required** The amount of heat needed to melt the ice is calculated using the formula: \[ Q = m \times L_f \] where: - \( m \) is the mass of the ice (0.3 kg), - \( L_f \) is the latent heat of fusion of ice (334 kJ/kg). Multiplying these: \[ Q = 0.3\, \text{kg} \times 334\, \text{kJ/kg} = 100.2\, \text{kJ} \] Thus, approximately **100 kJ** of energy must be added to melt the ice completely into water at 0°C. --- **Final note:** The correct choice based on this calculation is **D. 100 kJ**.