The question asks for the amount of heat required to change 200 grams of ice from process B to process C. To calculate this, we need to consider two factors: the specific heat capacity of ice and the heat of fusion of ice. The specific heat capacity of ice is given as 2,100 J/kg°C, which means it takes 2,100 joules of heat to raise the temperature of 1 kilogram of ice by 1 degree Celsius. The heat of fusion of ice is given as 336,000 J/kg, which means it takes 336,000 joules of heat to change 1 kilogram of ice into water at its melting point.
Since we have 200 grams of ice, we need to convert this to kilograms by dividing by 1,000 (1 kilogram = 1,000 grams). So, 200 grams is equal to 0.2 kilograms.
To calculate the heat required to change the ice from process B to process C, we first need to calculate the heat required to raise the temperature of the ice from its initial temperature to its melting point. This can be done using the formula Q = mcΔT, where Q is the heat, m is the mass, c is the specific heat capacity, and ΔT is the change in temperature. In this case, the initial temperature is unknown, but since the ice is at process B, we can assume it is below the melting point. Let's assume it is at -10°C. So, the change in temperature would be 0°C - (-10°C) = 10°C.
Using the formula Q = mcΔT, we can calculate the heat required to raise the temperature of the ice:
Q = (0.2 kg)(2,100 J/kg°C)(10°C) = 4,200 J
Next, we need to calculate the heat required to change the ice into water at its melting point. This can be done using the formula Q = mL, where Q is the heat, m is the mass, and L is the latent heat of fusion. In this case, the mass is 0.2 kilograms and the latent heat of fusion is 336,000 J/kg.
Using the formula Q = mL, we can calculate the heat required to change the ice into water:
Q = (0.2 kg)(336,000 J/kg) = 67,200 J
Therefore, the correct