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Calculate the enthalpy change, delta H, for the process in which 38.3 g of water is converted?

Calculate the enthalpy change, delta H, for the process in which 38.3 g of water is converted from liquid at 18.6 celcius to vapor at 25.0 celcius for water, delta Hvap= 44 kj/mol at 25 celcius and 8= 4.18j/(g*celcius) for H2O(l) Express your answer numerically in kilojoules.

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1. _____Enthalpy dHrxn = heat absorbed dHrxn = 0.0383 kg * [4.186 kJ/kgC * (25.0 - 18.6)C + (44.0 kJ/mole * 1 mole / 0.0180 kg)] = ?? SOLVE (dHrxn is pos as heat is required NOT released) Basic mathematics is a prerequisite to chemistry – I just try to help you with the methodology of solving the problem.