How much energy (heat)is required to convert 52.0 g of ice at -10.0°C to steam at 100°C? specific heat of ice: 2.09 J/g·°C $\Delta$H_fus = 6.02 kJ/mol Specific heat of water: 4.18 J/g·°C $\Delta$H_vap = 40.7 kJ/mol Specific heat of steam: 1.84 J/g·°C

Question

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To find the total energy required, calculate the energy for each step: 1) Heating ice from -10°C to 0°C, 2) Melting ice to water, 3) Heating water from 0°C to 100°C, 4) Vaporizing water to steam. Add these energies together to get the total energy.

How Much Energy (Heat)is Required to Convert 52 Δ\DeltaΔ Hfus = 6

How Much Energy (Heat)is Required to Convert 52 $\Delta$ H_fus = 6