c. How much total energy is required to actually boil 1.0 L of water in a 550 g iron pot?

To determine the total energy required to boil 1.0 L of water in a 550 g iron pot, we need to consider two main components:1. The energy required to heat the water from its initial temperature to its boiling point.2. The energy required to heat the iron pot from its initial temperature to the boiling point of water.Let's assume the initial temperature of both the water and the pot is room temperature, approximately 25°C. The boiling point of water is 100°C.### Step 1: Calculate the energy required to heat the waterThe specific heat capacity of water is .- Volume of water = 1.0 L = 1000 mL- Mass of water = 1000 g (since the density of water is approximately 1 g/mL)- Temperature change for water ( ) = 100°C - 25°C = 75°CUsing the formula for heat energy: ### Step 2: Calculate the energy required to heat the iron potThe specific heat capacity of iron is .- Mass of iron pot = 550 g- Temperature change for iron pot ( ) = 100°C - 25°C = 75°CUsing the formula for heat energy: ### Step 3: Calculate the total energy requiredAdd the energy required for the water and the iron pot: Therefore, the total energy required to boil 1.0 L of water in a 550 g iron pot is approximately 332,063 J (or 332.1 kJ).