Total heat energy = 306.125 kJ
Step-by-step 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