Calculate the total heat energy needed to convert 100 g of ice at - 10°C to steam at 110°C.

Total heat energy = 306.125 kJ

Explanation:

We have to calculate the energy required to undergo a phase change from ice to water then to steam.

Step 1: To find the heat required to change the phase of water from ice at - 10°C to 0°C as,

q₁ = m * c (ice) * ΔT = 100g * 2.09 J/g°C * (0 - (-15)) °C = 3,135 J

Step 2: Phase change from ice to water at 0°C.

q₂ = m * ΔH (f) = 100 g * 334 J / g = 33400 J

Step 3: Heat needed to change the water at 0°C to 100°C

q₃ = m * c * ΔT = 100 g * 4.18 J / g°C * (100 - 0) °C = 41,800 J

Step 4: Heat needed to convert water to vapor at 100°C

q₄ = m * ΔHv = 100 g * 2257 J/g = 225,700 J

Step 5: Heat required to convert 100° C to 110°C vapor

q₅ = m * Cv * ΔT = 100g * 2.09 J/g° C * (110 - 100) °C = 2090 J

Total Energy = q₁ + q₂ + q₃ + q₄ + q₅

= 3,135 J + 33400 J + 41,800 J + 225,700 J + 2090 J = 306125 J

= 306.125 kJ