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

Answer

Hi  

Here is your answer,

p₁=1.2 bar  

p₂= ?  

V₁= 120 mL  

V₂= 180 mL  

According to Boyle's law p₁V₁=p₂V₂

p₂= p₁V₁/V₂= 1.2 bar× 120mL/ 180mL = p₂ = 0.8 bar  

Hope it helps you!

Answer 2

$\huge \underline \mathsf \red {AnsWer:-}$

Given:

• Initial pressure, P1 = 1.2 bar
• Initial volume, V1 = 120 mL
• Final valume, V2 = 180 mL

Since the temperature remain constant, the the final pressure (P2) can be calculated using Boyle's law.

According to Boyle's law,

$p1v1 = p2v2$

$p2 = \frac{p1v1}{v2}$

$= \frac{1.2 \: \times \: \ 120}{180} \: \: bar$

$\mathsf \red { = 0.8 \: bar}$

Therefore:

• The pressure would be 0.8 bar.

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