2.9 g of a gas at 95°C occupied the same volume as 0.184 g of dihydrogen at 17°C, at the same pressure. What is the molar mass of the gas?.

Asked by Pragya Singh | 1 year ago |  127

1 Answer

Solution :-

Volume,

V = \( \dfrac{mRT}{Mp}\)

\( \dfrac{0.184  \; \times \; R \; \times \; 290}{ 2 \; \times \; p}\)

Let M be the molar mass of the unknown gas.

Volume occupied by the unknown gas is,

\( \dfrac{mRT}{Mp}\)

\( \dfrac{2.9  \; \times \; R \; \times \; 368}{ M \; \times \; p}\)

According to the ques,

\( \dfrac{0.184  \; \times \; R \; \times \; 290}{ 2 \; \times \; p}​ \)

\( = \dfrac{2.9  \; \times \; R \; \times \; 368}{ M \; \times \; p}​ \dfrac{0.184  \; \times \; 290}{ 2 } \)

\( = \dfrac{2.9  \;  \times \; 368}{ M }\)

M = \( \dfrac{2.9 \;\times \; 368 \; \times \; 2}{0.184 \; \times \; 290}\)

= 40g mol-1

Therefore, the molar mass of the gas is 40g mol-1

Answered by Pragya Singh | 1 year ago

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