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  • Stuck here, help me understand: A 0.5 dm3 flask contains gas A and 1 dm3 flask contains gas B at the same temperature. If density of A = 3 g/dm3 and that of B = 1.5 g/dm3 and the molar mass of A = 1/2 of B, the ratio of pressure exerted by gases is :

A 0.5 dm3 flask contains gas A and 1 dm3 flask contains gas B at the same temperature. If density of  A = 3 g/dm3 and  that of B = 1.5 g/dm3 and the molar mass of A = 1/2 of B, the ratio of pressure exerted by gases is : 

  • Option 1)

      \frac{P_{A}}{P_{B}} = 2

  • Option 2)

    \frac{P_{A}}{P_{B}} = 1

  • Option 3)

    \frac{P_{A}}{P_{B}} = 4

  • Option 4)

    \frac{P_{A}}{P_{B}} = 3

 

Answers (1)

best_answer

As we learnt in 

Ideal Gas Law in terms of density -

PM=d RT

- wherein

where

d - density of gas

P - Pressure

R - Gas Constant

T - Temperature

M - Molar Mass

 

P_{A}= \frac{3RT}{M_{A}}\: \: \: ;P_{B}= \frac{1.5RT}{M_{B}}

\frac{P_{A}}{P_{B}}= \frac{2M_{B}}{M_{A}}= \frac{2\times 2M_{A}}{M_{A}}= 4

 


Option 1)

  \frac{P_{A}}{P_{B}} = 2

Incorrect

Option 2)

\frac{P_{A}}{P_{B}} = 1

Incorrect

Option 3)

\frac{P_{A}}{P_{B}} = 4

Correct

Option 4)

\frac{P_{A}}{P_{B}} = 3

Incorrect

Posted by

Plabita

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