The mass of oxygen gas occupying a volume of 11.2 liters at a temperature $27^{\circ} C$ and of 760 of mercury is:

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Solution

Given

Temperature, $T = 273 + 27 = 300 K$

760 mm mercury pressure, $P = 10^{5} P a$

Volume, $V = 11.2 L = 11.2 \times 10^{- 3} m^{3}$

Gas constant for oxygen, $R = \frac{¯ ¯¯ ¯ R}{M} = \frac{8314}{32} = 259 J k g^{- 1} K^{- 1}$

From ideal gas equation,

$P V = n ¯ ¯¯¯¯ ¯ R_{0} T$

$P V = \frac{m}{M} ¯ ¯¯¯¯ ¯ R_{0} T = m R T$

$m = \frac{P V}{R T} = \frac{10^{5} \times 11.2 \times 10^{- 3}}{259 \times 300} = 0.0144 k g = 14.4 g r a m$

Hence, mass of gas is $14.4 g r a m$

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The mass of oxygen gas (in Kilo grams) occupying a volume of 11.2 litre at a temperature 27 $^{0}$ C and a pressure of 76cm of mercury is :

(Molecular weight of oxygen = 32)

3.5

O_{2}

27^{o} C

760

= 16

25^{\circ} C

m m

m L

m m

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