Question

at a pressure of 101.3 kilopascal and a temperature of 373 K, heat is removed from a sample of water vapor, causing the sample to change from the gaseous phase to the liquid phase. This phase change is represented by the equation H20(g) -> H20(l) + heat. Determine the total amount of heat released by 5.00 grams of water vapor during the phase change shown in the given experiment

Answer 1

Answer:

The amount of heat released is 11.3 KJ

Explanation:

H20(g) -> H20(l) + heat

This reaction is changing state from gaseous to liquid without changing the temperature. This heat is know as Latent heat. It is the energy required for a phase change.

Heat released by 5 g of water vapor (Q) = M ×  L

where M = mass of vapor

L= latent heat

Latent heat can be divide into 2

1. Latent heat of fusion
2. Latent heat of vaporization

Since we are change the gaseous state to liquid, we will be working with Latent heat of vaporization which has a value of 22.6 x 10 ∧5 J/kg

                                     (Q) = M ×  L

                                           = 0.005 x 22.6 x 10 ∧5

                                           = 11300 J

                                           = 11.3 KJ