1.

135 mL of a gas is collected over water at 25°C and 0.993 bar. if the gas weighs 0.160 grams and aqueous tension is is 0.0317 calculate the molar mass of the gas. ​

Answer»

ANSWER:

The molar mass of the gas is 30.108 mol/gms.

Explanation:

We have given that

P  = 0.993 - 0.0317

P   = 0.9613  bar  = 0.9487 atm

T = 25°C = 273 + 25 = 298K, V =135 ml = 0.135 ltr

R is a universal constant. So,

R = 0.0821 ltr/mol

No.\ of\ moles(n) = \dfrac{mass\ of\ gas(w)}{molar\ mass\ of\ gas(m)}

mass of gas = 0.16

We have to find molar mass of gas:

We KNOW that

PV = NRT

PV = \dfrac wm RT

0.9487 \times 0.135 =\dfrac {0.16}m \times 0.0821 \times 298\\\\m = \dfrac {0.16\times 0.0821 \times 298}{0.9487 \times 0.135} = \dfrac{3.914}{0.13}= 30.108 mol/gms

The molar mass of the gas is 30.108 mol/gms.


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