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If the energy from the condensation of 1.00 g of H2O ( g ) at 100 C is used to melt H2O ( s ) at 0 C, how many grams of ice will be melted?

If the energy from the condensation of 1.00 g of H2O (g) at 100 °C is used to melt H2O (s) at 0 °C, how many grams of ice will be melted? What will be the final temperature of the combined water from the condensation and the melting when thermal equilibrium is established?

ΔHfus =  6.02 kJ/mol

ΔHvap = 40.65 kJ/mol

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Grams of ice will be melted = 6.75 g The final temperature... View the full answer

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