Question

Question #b91ab

Answer 1

`"100. g H"_2"O"`

Explanation:

The problem essentially wants you to convert a given amount of energy to grams of steam at `100^@"C"`, so right from the start, you know that you're going to need a conversion factor.

This conversion factor is called the enthalpy of vaporization of water

`DeltaH_"vap" = "2257 J g"^(-1)`

http://www.engineeringtoolbox.com/fluids-evaporation-latent-heat-d_147.html

The enthalpy of vaporization tells you how much heat is needed in order to convert `"1 g"` of liquid water at its normal boiling point of `100^@"C"` to steam at `100^@"C"`.

In your case, you need `"2257 J"` of heat in order to convert `"1 g"` of liquid water at `100^@"C"` to steam at `100^@"C"`.

This means that `"226,000 J"` will allow you to convert

`"226,000" color(red)(cancel(color(black)("J"))) * "1 g"/(2257color(red)(cancel(color(black)("J")))) = color(darkgreen)(ul(color(black)("100. g")))`

The answer is rounded to three sig figs, the number of sig figs you have for the amount of heat.