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Dennis_Churaev [7]
3 years ago
14

Which formula can be used to calculate the molar mass of ammonia (NH3)?

Chemistry
1 answer:
Vesnalui [34]3 years ago
7 0

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

<u>Explanation:</u>

Molar mass is defined as the sum of the atoms present in a compound each multiplied with the number of atoms present in it.

For a compound A_xB_y

The molar mass will be = [(x\times \text{Molar mass of A})+(y\times \text{Molar mass of B})]

So, for the given compound NH_3,

The molar mass will be = [(1\times \text{Molar mass of Niyrogen})+(3\times \text{Molar mass of Hydrogen})]

Hence, the correct answer is Option C.

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The common laboratory solvent benzene is often used to purify substances dissolved in it. The vapor pressure of benzene , C6H6,
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As the relative lowering of vapor pressure is directly proportional to the amount of dissolved solute.

The formula for relative lowering of vapor pressure will be,

\frac{p^o-p_s}{p^o}=i\times x_2

where,

\frac{p^o-p_s}{p^o}= relative lowering in vapor pressure

i = Van'T Hoff factor = 1 (for non electrolytes)

x_2 = mole fraction of solute  =\frac{\text {moles of solute}}{\text {total moles}}

Given : 18.16 g of compound is present in 228.6 g of benzene

moles of solute = \frac{\text{Given mass}}{\text {Molar mass}}=\frac{18.16g}{Mg/mol}

moles of solvent (benzene) = \frac{\text{Given mass}}{\text {Molar mass}}=\frac{228.6g}{78g/mol}=2.93moles

x_2 = mole fraction of solute  =\frac{\frac{18.16g}{Mg/mol}}{\frac{18.16g}{Mg/mol}+2.93}

\frac{73.03-71.88}{73.03}=1\times \frac{\frac{18.16g}{Mg/mol}}{\frac{18.16g}{Mg/mol}+2.93}

M=387.3g/mol

The molecular weight of this compound is 387.3g/mol

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