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3 years ago

ICl has a higher boiling point than Br2. What is the best explanation for this?

Chemistry

2 answers:

Burka [1]3 years ago

8 0

Answer:

b. ICl experiences dipole-dipole interactions

Explanation:

The molecule with the stronger intermolecular forces will have the higher boiling point.

In Br₂, the Br-Br bond has a dipole moment of zero, because the two atoms are identical.

In ICl, the I-Cl bond, has two different atoms. One must be more electronegative than the other, so there will be a non-zero bond dipole.

ICl will have the higher boiling point.

a is wrong. Br₂ is nonpolar, so it has no dipole-dipole interactions.

c is wrong. Br₂ cannot form hydrogen bonds, because there is no hydrogen.

d is wrong. ICl has dipole-dipole interactions.

77julia77 [94]3 years ago

6 0

Answer:

B. ICl experiences dipole-dipole interactions.

Explanation:

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Answer:

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Explanation:

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907.185 x 0.04 =

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3 years ago

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3 years ago

In a water molecule (H2O), the oxygen atom has two unshared pairs of electrons and two bonding pairs of electrons. How do the un

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Answer:

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3 years ago

Ethanol, C2H6O, is most often blended with gasoline - usually as a 10 percent mix - to create a fuel called gasohol. Ethanol is

weeeeeb [17]

Answer:

This means 463 grams of ethanol would provide less amount of energy

Explanation:

Step 1: Data given

Heat of combustion of ethanol = 326.7 kcal/mol

The heat of combustion of octane = 1.308*10³ kcal/mol

Mass of octane = 463 grams

Molar mass octane = 114.23 g/mol

Molar mass ethanol = 46.07 g/mol

Step 2: Calculate moles octane

Moles octane = mass octane / molar mass octane

Moles octane = 463 grams / 114.23 g/mol

Moles octane = 4.05 moles

Step 3: Calculate energy of combustion of 4.05 moles octane

Combustion of 1 mol octane gives us: 1.308 * 10³ kcal/mol

Combustion of 4.05 moles octane gives us 4.05 * 1.308 * 10³ kcal/mol = 5.30 * 10³ kcal

This means the combustion reaction of 463 grams of octane gives us 5.30 * 10³ kcal

Step 4:

Heat of combustion of ethanol = 326.7 kcal/mol

OR in words: combustion of 1 mol ethanol gives us 326.7 kcal energy

Moles ethanol = 463 grams / 46.07 g/mol

Moles ethanol = 10.05 moles

Since combustion of 1 mol ethanol gives us 326.7 kcal

10.05 moles ethanol will give us = 10.05 * 326.7 = 3283.3 kcal = 3.28 * 10³ kcal

5.30 * 10³ kcal > 3.28 * 10³ kcal

This means 463 grams of ethanol would provide less amount of energy

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3 years ago

1. How many moles of CO2 can be produced from a reaction of 10.0 moles CzHg?

mr_godi [17]

Answer:

$20$ moles of CO2 can be produced from a reaction of 10.0 moles C2H6

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In this reaction -

2 moles of C₂H6 produces four molecules of Carbon dioxide (CO2)

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Thus, 10 moles of C₂H6 will produce $2 * 10 = 20$ moles of Carbon dioxide (CO2)

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3 years ago