Ncert Exercises & Solutions

5.8 What will be the pressure of the gaseous mixture when 0.5 L of H2 at 0.8 bar and 2.0 L of dioxygen at 0.7 bar are introduced in a 1L vessel at 27°C?

NEETprep Answer:

Let the partial pressure of $H_{2}$ in the vessel be $p H_{2}$ .

Now,

$p_{1} = 0.8 b a r p_{2} = p_{H_{2}}$
$V_{1} = 0.5 L V_{2} = 1 L$

It is known that,

$p_{1} V_{1} = p_{2} V_{2}$
$\Rightarrow p_{2} = \frac{p_{1} V_{1}}{V_{2}}$
$\Rightarrow p_{H_{2}} = \frac{0.8 \times 0.5}{1}$
$= 0.4 b a r$

Now, let the partial pressure of $O_{2}$ in the vessel be $p_{O_{2}}$ .

Now,

$p_{1} 0.7 b a r p_{2} = p_{O_{2}} = ?$
$V_{1} = 2.0 L V_{2} = 1 L$

$p_{1} V_{1} = p_{2} V_{2}$
$\Rightarrow p_{2} = \frac{p_{1} V_{1}}{V_{2}}$
$\Rightarrow p_{O_{2}} = \frac{0.7 \times 20}{1}$
$= 0.4 b a r$

Total pressure of the gas mixture in the vessel can be obtained as:

$p_{t o t a l} = p_{H_{2}} + p_{O_{2}}$
$= 0.4 + 1.4$
$= 1.8 b a r$

Hence, the total pressure of the gaseous mixture in the vessel is 1.8 bar.

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