3-2 g of oxygen and 0-2 g of hydrogen are placed in 1-12 litre flask at 0-C- Find the total pressure in atm of the gas mixture-

The molecular weights of oxygen and hydrogen are 32 g/mol and 2 g/mol respectively. #160;The number of moles of oxygen = 3.2 g32 g/mol = 0.1 mol. T ...

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Standard XII

Chemistry

Ideal Gas Equation

3.2 g of oxyg...

Question

$3.2 g$ of oxygen and $0.2 g$ of hydrogen are placed in $1.12 l i t r e$ flask at $0^{\circ} C$ . Find the total pressure in atm of the gas mixture.

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Solution

The molecular weights of oxygen and hydrogen are 32 g/mol and 2 g/mol respectively.

The number of moles of oxygen $= \frac{3.2 g}{32 g / m o l} = 0.1 m o l .$

The number of moles of hydrogen $= \frac{0.2 g}{2 g / m o l} = 0.1 m o l .$

Total number of moles $= 0.1 + 0.1 = 0.2$ moles.

Total pressure $P = \frac{n R T}{V} = \frac{0.2 m o l e s \times 0.08206 L a t m / m o l K \times 273.15 K}{1.12 L} = 4 a t m$

Thus, the total pressure in atm of the gas mixture will be 4 atm.

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3.2 g of oxygen and 0.2 g of hydrogen are placed in 1.12 litre flask at 0∘C. Find the total pressure in atm of the gas mixture.

$3.2 g$ of oxygen and $0.2 g$ of hydrogen are placed in $1.12 l i t r e$ flask at $0^{\circ} C$ . Find the total pressure in atm of the gas mixture.