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Art [367]
3 years ago
11

Calculate the amount of heat energy required to evaporate 27.5 g of water at 100.0°C. (molar heat of vaporization of liquid wate

r = 4.07 ✕ 104 J/mol)
a. 6.20 ✕ 107 kJ
b. 2.02 ✕ 104 kJ
c. 1.22 ✕ 10-2 kJ
d. 6.20 ✕ 104 J
e. 1.12 ✕ 103 kJ
Chemistry
1 answer:
frez [133]3 years ago
8 0

Answer:

D. 6.20 × 10^4 J

Explanation:

The heat change in changing water from a liquid state to a gaseous state without change in temperature is given by the formula;

Heat = MLv ; where m is the mass and Lv is the latent heat of vaporization.

In this case we will use mass in terms of number of moles as the latent heat is given in joules/mole.

Therefore;

Moles of water = 27.5 g/18 g/mol

                         = 1.528 moles

Hence;

Heat = 1.528 moles × 4.07 ×10^4 J/mol

        = 6.20 × 10^4 Joules

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Table salt is also known as sodium chloride, because it is
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Sodom chloride is an ionic compound.

<h3>What is sodium chloride?</h3>

Sodium chloride is a compound that is formed by the combination of sodium and chlorine atoms. The compound is ionic as the ions of the atoms combine. Sodium looses one electron that can now be gained by chlorine.

Since the compound is ionic, it has a high melting and boiling point. This implies that the compound could melt as high as 801 degrees centigrade. The boiling point of the compound is much higher.

We can represent the compound using the ball and stick or the space filling model. The ball and stick model of sodium chloride has been shown in the image attached to this answer.

Learn more about ball and stick model:brainly.com/question/17217225

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