\nTo calculate the total heat required, we need to consider the heat needed for each stage of the process:
\n1. Heat required to raise the temperature of 10 g of ice from -10\u00b0C to 0\u00b0C:
\n $Q_1 = m_{ice} \\times c_{ice} \\times \\Delta T_1$
\n Assuming specific heat of ice $c_{ice} = 0.5 \\, \\text{cal\/g}^\\circ\\text{C}$.
\n $Q_1 = 10 \\, \\text{g} \\times 0.5 \\, \\text{cal\/g}^\\circ\\text{C} \\times (0^\\circ\\text{C} – (-10^\\circ\\text{C})) = 10 \\times 0.5 \\times 10 = 50 \\, \\text{cal}$.
\n2. Heat required to melt 10 g of ice at 0\u00b0C into water at 0\u00b0C:
\n $Q_2 = m_{ice} \\times L_{fusion}$
\n Assuming latent heat of fusion of ice $L_{fusion} = 80 \\, \\text{cal\/g}$.
\n $Q_2 = 10 \\, \\text{g} \\times 80 \\, \\text{cal\/g} = 800 \\, \\text{cal}$.
\n After this step, we have 10 g of water at 0\u00b0C.
\n3. Heat required to raise the temperature of the 10 g of water (from melted ice) from 0\u00b0C to 10\u00b0C:
\n $Q_3 = m_{water(ice)} \\times c_{water} \\times \\Delta T_2$
\n Assuming specific heat of water $c_{water} = 1 \\, \\text{cal\/g}^\\circ\\text{C}$.
\n $Q_3 = 10 \\, \\text{g} \\times 1 \\, \\text{cal\/g}^\\circ\\text{C} \\times (10^\\circ\\text{C} – 0^\\circ\\text{C}) = 10 \\times 1 \\times 10 = 100 \\, \\text{cal}$.
\n4. Heat required to raise the temperature of the initial 10 g of water from 0\u00b0C to 10\u00b0C:
\n $Q_4 = m_{water(initial)} \\times c_{water} \\times \\Delta T_3$
\n $Q_4 = 10 \\, \\text{g} \\times 1 \\, \\text{cal\/g}^\\circ\\text{C} \\times (10^\\circ\\text{C} – 0^\\circ\\text{C}) = 10 \\times 1 \\times 10 = 100 \\, \\text{cal}$.<\/p>\nTotal heat required = $Q_1 + Q_2 + Q_3 + Q_4 = 50 + 800 + 100 + 100 = 1050 \\, \\text{cal}$.
\n<\/section>\n\n– Heat transfer during phase change (melting or freezing) involves latent heat ($Q = mL$).
\n– Heat transfer during temperature change involves specific heat ($Q = mc\\Delta T$).
\n– Need to account for heat required for each component (ice and water) and each process (heating ice, melting ice, heating water).
\n<\/section>\n