Question

A vessel of 120 mL capacity contains a certain amount of gas at 35 °C and 1.2 bar pressure. The gas is transferred to another vessel of volume 180 mL at 35°C. What would be its pressure ?​

Answer 1

Explanation:

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Answer 2

Chemistry /class - 11th

AnSwer :-

Given :-

• Initial pressure, p$_{1}$= 1.2bar
• Initial volume, V$_{1}$= 120ml
• Final volume, V$_{2}$= 180ml

To find :-

The final pressure, p$_{2}$

Solution :-

Since the temperature remains constant, the final pressure (p$_{2}$) can be calculated using Boyle's law.

According to Boyle's law,

p$_{1}$V$_{1}$ = p$_{2}$V$_{2}$

$\sf p_2 = \dfrac{p_1V_1}{V_2} = \dfrac{1.2 \times 120}{180} bar = 0.8bar$

thus, the pressure would be 0.8bar

Know more :

• Boyle's law :- At constant temperature, the pressure of a fixed amount of a gas varies inversely with its volume.

For the given mass of a gas at constant temperature, volume of the gas is inversely proportional to the pressure acting on it.

For a gas,

1. v ∝ 1/p
2. pV = constant
3. p$_{1}$V$_{1}$= p$_{2}$V$_{2}$