What will be the pressure of the gaseous mixture when 0.5 L of $$H_2$$at 0.8 bar and 2.0 L of dioxygen at 0.7 bar are introduced in a 1L vessel at o 27°C ?

Asked by Pragya Singh | 1 year ago |  57

##### Solution :-

Let the partial pressure of $${H_{ 2 }}$$​ in the container be $$p_{H_{ 2 }}$$​​.

Now,

$${p_{ 1 }}$$ = 0.8 bar

$${p_{ 2 }} = p_{H_{ 2 }}$$

$${V_{ 1 }} = 0.5 L$$

$${V_{ 2 }}= 1 L$$

It is known that,

$${p_{ 1 }}​ {V_{ 1 }}= {p_{ 2 }}​ {V_{ 2 }}$$

$${p_{ 2 }}= \dfrac{p_{ 1 } \; \times \; V_{ 1 }}{V_{ 2 }} p_{H_{ 2 }}$$

$$= \dfrac{ 0.8 \; \times \; 0.5 }{ 1 }$$

= 0.4 bar

Now, let the partial pressure of O2 in the container be $$p_{O_{ 2 }}$$.

Now,

$${p_{ 1 }}= 0.7bar$$

$${V_{ 1 }}= 2.0 L$$

$${V_{ 2 }}= 1 L$$

$${p_{ 2 }}​ = p_{O_{ 2 }}$$ = ?

$${p_{ 1 }}{V_{ 1 }}​ = {p_{ 2 }}{V_{ 2 }}$$

$${p_{ 2 }}= \dfrac{p_{ 1 } \; \times \; V_{ 1 }}{V_{ 2 }}$$

$$p_{O_{ 2 }} = \dfrac{ 0.7 \; \times \; 20 }{ 1 }$$

= 1.4 bar

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

$$p_{total}= p_{H_{ 2 }} + p_{O_{ 2 }}$$

= 0.4 + 1.4

= 1.8 bar

Answered by Abhisek | 1 year ago

### Related Questions

#### Explain the physical significance of Van der Waals parameters.

Explain the physical significance of Van der Waals parameters.

#### Critical temperature for carbon dioxide and methane are 31.1°C and – 81.9°C respectively.

Critical temperature for carbon dioxide and methane are 31.1°C and – 81.9°C respectively. Which of these has stronger intermolecular forces and why?

#### In terms of Charles’ law explain why -273°C is the lowest possible temperature.

In terms of Charles’ law explain why -273°C is the lowest possible temperature.

What would be the SI units for the quantity $$\dfrac{pV^2 T^2}{n}$$