Answer:
Buoyancy.
Explanation:
Think of a balloon and a bowling ball. The volume of the balloon is the same for the bowling ball, but not the mass.
86.7 kJ
<h3>
Further explanation</h3>
<u>Given:</u>
Molar mass (Mr) of ethanol = 46.07 g/mol
<u>Question:</u>
How much energy is required to vaporize 98.6 g of ethanol (C₂H₅OH) at its boiling point?
<u>The Process:</u>
Observe this . This means that 40.5 kJ of energy is required to vaporize every 1 mole of ethanol at its boiling point. Therefore we must first convert grams into moles.
<u>Question:</u>
Step-1:
Let us count the number of moles of 98.6 g of ethanol.
We obtain 2.14 moles of ethanol.
Step-2:
Let us calculate how much energy is required to vaporize 2.14 moles of ethanol at its boiling point.
The amount of energy required is
Thus, the amount of energy required to vaporize 98.6 g of ethanol at its boiling point is 86.7 kJ.
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Quick Steps
<h3>Learn more</h3>
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- Write the equilibrium constant for the reaction brainly.com/question/10608589
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Keywords: how much, energy required, to vaporize, ethanol, C₂H₅OH, its boiling point, ΔHvap, molar mass, moles, converts, kJ/mol
Answer:
faster because atoms move faster when heated . If the temperature of the salt is extremely hot, a thin layer of vapor will form on the surface, insulating the salt from the water.
Explanation: