What amount of heat is required to convert a 1.5 kg block of ice at − 15.0 ° C to steam at 150.0 ° C? Assume the specific heat of water to be 4.18 J\g ° C, specific heat of ice to be 2.108 J\g ° C, specific heat of steam to be 1.996 J\g ° C, Δ H _fus= 333.55 J\g, and Δ H _vap= 2.26 kJ\g.

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Explanation:The heat required to convert 1.5 kg of ice at -15.0 °C to steam at 150.0 °C can be calculated as follows:Heat required to raise the temperature of ice from -15.0 °C to 0 °C:Q1 = m * c_ice * ΔT = 1.5 kg * 2.108 J/g °C * 15 °C = 47.43 kJHeat required to melt the ice at 0 °C:Q2 = m * ΔH_fus = 1.5 kg * 333.55 J/g = 499.83 kJHeat required to raise the temperature of water from 0 °C to 100 °C:Q3 = m * c_water * ΔT = 1.5 kg * 4.18 J/g °C * 100 °C = 627 kJHeat required to vaporize the water at 100 °C:Q4 = m * ΔH_vap = 1.5 kg * 2.26 kJ/g = 3390 kJHeat required to raise the temperature of steam from 100 °C to 150 °C:Q5 = m * c_steam * ΔT = 1.5 kg * 1.996 J/g °C * 50 °C = 149.7 kJTotal heat required:Q = Q1 + Q2 + Q3 + Q4 + Q5 = 47.43 kJ + 499.83 kJ + 627 kJ + 3390 kJ + 149.7 kJ = 4713.99 kJ ≈ 4711 kJTherefore, the correct answer is D) 4,711 kJ.

What Amount of Heat Is Required to Convert a 1