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Bad White [126]
3 years ago
15

Estimate the molar mass of a gas that effuses at 1.80 times the effusion rate of carbon dioxide. answer in units of g/mol.

Chemistry
1 answer:
Effectus [21]3 years ago
3 0
From Grahams Law the rates of effusion of two gases are inversely proportional to the square roots of their molar masses at the same temperature and pressure.
Therefore; R1/R2 = √mm2/√mm1
The molecular mass of Carbon dioxide is 44 g
Hence;  1.8 = √(44/x
             3.24 = 44/x
                x = 44/3.24
                   = 13.58 
Therefore, the molar mass of the other gas is 13.58 g/mol
           
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<u>Answer:</u>

<u>For 1:</u> The correct answer is Option A.

<u>For 2:</u> The correct answer is Option B.

<u>For 3:</u> The correct answer is Option C.

<u>Explanation:</u>

<u>For 1:</u>

Atomic number is defined as the number of electrons or number of protons that are present in a neutral atom. It is represented as Z.

Z = Atomic number = Number of electrons = Number of protons

Mass number is defined as the sum of number of protons and number of neutrons present in an atom. It is represented as A.

A = Mass number = Number of protons + Number of neutrons

Hence, the correct answer is Option A.

  • <u>For 2:</u>

The isotopic representation of an atom is: _Z^A\textrm{X}

where,

Z = Atomic number of the atom

A = Mass number of the atom

X = Symbol of the atom

We are given:

An isotopic representation of beryllium atom:  _4^9\textrm{Be}

Thus, the number '4' represents the atomic number of beryllium, number '9' represents the mass number of beryllium atom.

Hence, the correct answer is Option B.

  • <u>For 3:</u>

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In CO_2 compound:

Mass of oxygen = 32 g

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Thus, the ratio of mass of oxygen in CO_2 and CO is:

CO_2:CO=32:16=2:1

Hence, the correct answer is Option C.

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