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

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

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

answer:

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