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

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Chemistry

8 October, 21:28

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

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Cory Herman · Answer 1

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

Latent heat of fusion 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