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4 years ago

What is the strongest type of intermolecular force present in chf3?

Chemistry

1 answer:

stealth61 [152]4 years ago

6 0

Answer:

The strongest type of intermolecular force present in CHF₃ is dipole - dipole interaction.

Explanation:

There are 3 basic types of intermolecular forces (forces between molecules):

London dispersion force
Dipole - dipole force
Hydrogen bonds.

London dispersion forces are weak attraction forces between molecules due to temporary displacement of the electron density over the atoms, resulting in the formation of temporary dipoles. The electrostatic attraction between those dipoles is the weak dispersion force.

Dipole - dipole attraction forces happen in polar molecules, such as CHF₃, because the dipoles are permanent. The dipoles are the result of the assymetryc distribution of the electron charge, due to the presence of atoms with different electronegativities. In CHF₃, F is much more electronegative than C, causing the uneven distribution of the electrons, which leads to the formation of the dipoles and the dipole - dipole forces which are stronger than london dispersion forces.

Hydrogen bonds, the strongest intermolecular forces, are only present when hydrogen is bonded to a small a very electronegative atom, like oxygen, nitrogen or fluor. Since, in CHF₃, hydrogen is bonded to C, there is not formation of hydrogen bonds.

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Consider the following reaction:C2H4(g) + F2(g) -----------> C2H4F2(g) Delta H = -549 kJEstimate the carbon-fluorine bond ene

frutty [35]

Answer:

Bond energy of carbon-fluorine bond is 485 kJ/mol

Explanation:

Enthalpy change for a reaction, is given as:

$\Delta H_{rxn}=\sum [n_{i}\times (E_{bond})_{i}]-\sum [n_{j}\times (E_{bond})_{j}]$

Where $(E_{bond})_{i}$ and $(E_{bond})_{j}$ represents average bond energy in breaking "i" th bond and forming "j" th bond respectively. $n_{i}$ and $n_{j}$ are number of moles of bond break and form respectively.

In this reaction, one mol of C=C, four moles of C-H and one mol of F-F bonds are broken. One mol of C-C bond, four moles of C-H bonds and two moles of C-F bonds are formed

So, $-549kJ=(1mol\times 614kJ/mo)+(4mol\times E_{C-H})+(1mol\times 154kJ/mol)-(1mol\times 347kJ/mol)-(4mol\times E_{C-H})-(2mol\times E_{C-F})$

or, $-549kJ=(1mol\times 614kJ/mo)+(1mol\times 154kJ/mol)-(1mol\times 347kJ/mol)-(2mol\times E_{C-F})$

or, $E_{C-F}=485kJ/mol$

So bond energy of carbon-fluorine bond is 485 kJ/mol

8 0

3 years ago

Methane burns in the presence of oxygen to form carbon dioxide and water.

wlad13 [49]

Answer:

= 9.28 g CO₂

Explanation:

First write a balanced equation:

CH₄ + 2O₂ -> 2H₂O + CO₂

Convert the information to moles

7.50g CH₄ = 0.46875 mol CH₄

13.5g O₂ = 0.421875 mol O₂

Theoretical molar ratio CH₄:O₂ -> 1:2

Actual ratio is 0.46875 : 0.421875 ≈ 1:1

If all CH₄ is used up, there would need to be more O₂

So O₂ is the limiting reactant and we use this in our equation

Use molar ratio to find moles of CO₂

0.421875 mol O₂ * 1 mol CO₂/2 mol O₂=0.2109375 mol CO₂

Then convert to grams

0.2109375 mol CO₂ = 9.28114 g CO₂

round to 3 sig figs

= 9.28 g CO₂

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3 years ago

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