How much heat energy is absorbed when 41.5g of ice melts at stp? (picture attached)

= 13.857 kJ

Explanation:

The heat required to melt ice from its solid state to water or liquid states without change in temperature is given by the formula;

Heat = mLf ; where m is the mass of ice and Lf is the latent heat of fusion,

The mass of ice in moles = 41.5 g/18 g

                                         = 2.306 moles

Therefore;

Heat = 2.306 moles × 6.009 kJ/mol

        = 13.857 kJ

a corroding iron, if that's one of your choices