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3 years ago

Determine the molecular mass of the following compounds:

Chemistry

1 answer:

antiseptic1488 [7]3 years ago

5 0

The molecular mass of the compound, Cl₂CO is 99 g/mol

Molecular mass of a compound can simply be obtained by adding the molar masses of the different elements present in the compound.

With the above information in mind, we can obtain the molecular mass of the compound as follow:

<h3>Molecular formula of compound => Cl₂CO</h3>

Molar mass of Cl = 35.5 g/mol

Molar mass of C = 12 g/mol

Molar mass of O = 16 g/mol

<h3>Molar mass of Cl₂CO =? </h3>

Molar mass of Cl₂CO = (35.5×2) + 12 + 16

= 71 + 12 + 16

Therefore the molecular mass of Cl₂CO is 99 g/mol

Learn more: brainly.com/question/11209783

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Answer:

Br - C ≡ N

Explanation:

To draw the Lewis line-bond structure we need to bear in mind the octet rule, which states that in order to gain stability each <em>atom tends to share electrons until it has 8 electrons in its valence shell</em>.

C has 4 e⁻ in its valence shell so it will form 4 covalent bonds.

Br has 7 e⁻ in its valence shell so it will form 1 covalent bond.

N has 5 e⁻ in its valence shell so it will form 3 covalent bonds.

The most stable structure that respects these premises is:

Br - C ≡ N

It does not have any H atom.

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What are even covalent chlorides? Question D

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I hope my answer helps you

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3 years ago

Part 1. determine the molar mass of a 0.458-gram sample of gas having a volume of 1.20 l at 287 k and 0.980 atm. show your work.

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The molar mass of 0.458-gram sample of gas having a volume of 1.20 l at 287 k and 0.980 atm is 9.15g/mol.
If this sample was placed under extreme pressure, the volume of the sample will decrease.

<h3>How to calculate molar mass?</h3>

The molar mass of a substance can be calculated by first calculating the number of moles using ideal gas law equation:

PV = nRT

Where;

P = pressure
V = volume
T = temperature
R = gas law constant
n = no of moles

0.98 × 1.2 = n × 0.0821 × 287

1.18 = 23.56n

n = 1.18/23.56

n = 0.05moles

mole = mass/molar mass

0.05 = 0.458/mm

molar mass = 0.458/0.05

molar mass = 9.15g/mol

Therefore, the molar mass of 0.458-gram sample of gas having a volume of 1.20 l at 287 k and 0.980 atm is 9.15g/mol
If this sample was placed under extreme pressure, the volume of the sample will decrease.

Learn more about gas law at: brainly.com/question/12667831

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2 years ago