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

your answer would be a. 12.5 kg

false

because it does not have the potential to be entirely used up