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States of Matter

Section: Chemistry

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Question : 2 of 31

Marks: +1, -0

At

27^{\circ} \mathrm{C}, 1 \mathrm{L}

\mathrm{H}_2

with a pressure of 1 bar is mixed with 2 L of

\mathrm{O}_2

with a pressure of 2 bar in a 10 L flask. What is the pressure exerted by gaseous mixture in bar? (Assume

\mathrm{H}_2

\mathrm{O}_2

as ideal gases)

[AP EAPCET 24 May 2025 S1]

$4$
$0.05$
$1$
$0.5$

Solution:

Calculating the partial pressure of

\mathrm{H}_2

in 10 L flask

\; p_{\mathrm{H}_2 \; \text{ initial }} \; \; V_{\mathrm{H}_2 \; \text{ initial }} = p_{\mathrm{H}_2 \; \text{ final }} \; \; V_{\text{ total }}

\; p_{\mathrm{H}_2 \; \text{ final }} = \; \frac{1 \times 1}{10} = 0.1 \text{ bar}

Using Boyle's law for partial pressure of

\mathrm{O}_2

p_{\mathrm{O}_2 \; \text{ final }} \; = \; \frac{p_{\mathrm{O}_2 \; \text{ initial }} \times V_{\mathrm{O}_2 \; \text{ initial }}}{V_{\text{ total }}}

\; = \; \frac{2 \times 2}{10} = 0.4 \text{ bar}

Use Dalton's law of partial pressure.

p_{\text{ total }} \; = p_{\mathrm{H} \; \text{ final }} \; \; + p_{\mathrm{O}_2 \; \text{ final }}

\; = 0.1+0.4=0.5 \text{ bar}

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