Question #b01e8

1 Answer
Sep 22, 2017

Answer:

#"33,360 J"#

Explanation:

The idea here is that the enthalpy of fusion, #DeltaH_"fus"#, tells you the amount of energy needed to convert #"1 g"# of a given substance from solid at its melting point to liquid at its melting point.

In your case, the enthalpy of fusion of water

#DeltaH_"fus" = color(darkorange)("333.6 J")color(white)(.)color(blue)("g"^(-1)#

tells you that in order to turn #color(blue)("1 g")# of ice at its normal melting point of #0^@"C"# to liquid water at #0^@"C"#, you need to provide #color(darkorange)("333.6 J")# of heat.

This means that you will need

#100.0 color(red)(cancel(color(black)("g"))) * color(darkorange)("333.6 J")/(color(blue)(1)color(red)(cancel(color(blue)("g")))) = color(darkgreen)(ul(color(black)("33,360 J")))#

The answer is rounded to four sig figs, the number of sig figs you have for the mass of the sample.