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

Asked by Pragya Singh | 1 year ago |  108

1 Answer

Solution :-

Initial pressure, P1 = 1.2bar

Initial volume, V1 = 120mL 

Final volume, V2 = 180mL

As the temperature remains the same, final pressure (P2) can be calculated with the help of Boyle’s law.

According to the Boyle’s law,

P1V1 = P2V2

P=\( \dfrac{P_{1}V_{1}}{V_{2}}\)

=\( \dfrac{1.2 \; \times \; 120}{180}\)

= 0.8bar

Therefore, the min pressure required is 0.8bar.

Answered by Pragya Singh | 1 year ago

Related Questions

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?

Class 11 Chemistry States of Matter View Answer

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

Class 11 Chemistry States of Matter View Answer

A mixture of dihydrogen and dioxygen at one bar pressure contains 20% by weight of dihydrogen. Calculate the partial pressure of dihydrogen.

Class 11 Chemistry States of Matter View Answer