Question

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 H2O is 112,500 Joules.

Step-by-step explanation:

To determine the total amount of heat required to completely vaporize a 50.0-gram sample of H2O at its boiling point at standard pressure, we can use the heat of vaporization value for water. The heat of vaporization for water is about 2,250 J per gram. Therefore, to vaporize the entire 50.0-gram sample, we need to multiply the mass by the heat of vaporization:

Q = m × Hvap

Q = (50.0 g) × (2,250 J/g) = 112,500 J

Therefore, the total amount of heat required to completely vaporize a 50.0-gram sample of H2O is 112,500 Joules.

Answer 2

In order to calculate the amount of energy required, we must first check the latent heat of vaporization of water from literature. The latent heat of vaporization of any substance is the amount of energy required per unit mass to convert that substance from a solid to a liquid. For water this is 2,260 J/g. We now use the formula:
Energy = mass * latent heat
Q = 50 * 2,260
Q = 113,000 J

113,000 Joules of heat energy are required.