SELECT * FROM question_mgmt as q WHERE id=1379 AND status=1 SELECT id,question_no,question,chapter FROM question_mgmt as q WHERE courseId=2 AND subId=9 AND chapterId=46 and ex_no='1' AND status=1 ORDER BY CAST(question_no AS UNSIGNED)

Question:

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?

Answer:

From the gas equation,

PV = (w/M) RT

Substituting the given data in the gas equation, we get

PV = (2.9 / M) x R x 368

&

PV = (0.184 / 2) x R x 290

From these two equation, we can write

(2.9 / M) x R x 368 = (0.184 / 2) x R x 290

By, striking throug R from both side, we get

(2.9 / M) x 368 = (0.184 / 2) x 290

Or

(2.9 / M)   =  (0.092 X 290) / 368

Or

M  = 2.9 x 368 / 0.092 x 290

= 40 g/mol

Hence, the molar mass of the gas is 40 g mol–1.


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