Question

at standard pressure, water has unusual properties that are due to both its molecular structure and intermolecular forces. for example, although most liquids contract when they freeze, water expands, making ice less dense than liquid water. water has a much higher boiling point than most other molecular compounds having a similar gram-formula mass. determine the total amount of heat, in joules, required to completely vaporize a 50.0-gram sample of h2o( ) at its boiling point at standard pressure.

Answer 1

The total amount of heat required to completely vaporize a 50.0-gram sample of water at its boiling point at standard pressure is 122445.2 joules.

Step-by-step explanation:

Water has a high heat of vaporization, which means that it requires a considerable amount of heat energy to change from a liquid to a gas. The heat of vaporization for water is 586 cal. To determine the total amount of heat required to completely vaporize a 50.0-gram sample of water at its boiling point at standard pressure, we can use the equation:

Heat energy = mass x heat of vaporization

Substituting the values, we get:

Heat energy = 50.0 g x 586 cal/g = 29300 cal

To convert cal to joules, we multiply by 4.184:

Heat energy = 29300 cal x 4.184 J/cal = 122445.2 J