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Standard XII

Chemistry

Dalton's Law of Partial Pressures

1500 mL flask...

Question

$1500 m L$ flask contains $400 m g C O_{2}$ and $60 m g H_{2}$ at $100^{\circ} C$ .
(a) What is the total pressure in the flask?
(b) If the mixture is permitted to react to form water vapour of $100^{\circ} C$ , what will be left and what will be their partial pressures?

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Solution

(a) No. of moles of $O_{2} = \frac{400}{1000 \times 32} = 0.0125$
No. of moles of $H_{2} = \frac{60}{1000 \times 2} = 0.03$
Partial pressure of $O_{2} = \frac{0.0125 \times 0.0821 \times 373}{1.5} = 0.255 a t m$
Partial pressure of $H_{2} = \frac{0.03 \times 0.0821 \times 373}{1.5} = 0.612 a t m$
Total pressure $= 0.255 + 0.612 = 0.867 a t m$
(b) $2 H_{2} + O_{2} ⟶ 2 H_{2} O$
Initial $0.03 0.0125 0$
After reaction $0.005 0 0.025$
Partial pressure of $H_{2} = \frac{0.005 \times 0.0821 \times 373}{1.5} = 0.102 a t m$
Partial pressure of $H_{2} O = \frac{0.025 \times 0.0821 \times 373}{1.5} = 0.51 a t m$

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1500 mL flask contains 400 mg CO2 and 60 mg H2 at 100∘C.(a) What is the total pressure in the flask?(b) If the mixture is permitted to react to form water vapour of 100∘C, what will be left and what will be their partial pressures?

$1500 m L$ flask contains $400 m g C O_{2}$ and $60 m g H_{2}$ at $100^{\circ} C$ .
(a) What is the total pressure in the flask?
(b) If the mixture is permitted to react to form water vapour of $100^{\circ} C$ , what will be left and what will be their partial pressures?