Statement 1 : Ammonia gas, $N H_{3}$ has a smaller density than argon gas, $A r$ , at $S T P$ .
Statement 2: The density of a gas at $S T P$ is found by dividing the molar mass by $22.4$ litres.

Both Statement 1 and Statement 2 are correct and Statement 2 is the correct explanation of Statement 1.

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Both Statement 1 and Statement 2 are correct and Statement 2 is not the correct explanation of Statement 1.

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Statement 1 is correct but Statement 2 is not correct.

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Statement 1 is not correct but Statement 2 is correct.

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Both the Statement 1 and Statement 2 are not correct.

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Solution

The correct option is A
Both Statement 1 and Statement 2 are correct and Statement 2 is the correct explanation of Statement 1.

Statement 1 : Ammonia gas, $N H_{3}$ has a smaller density than argon gas, $A r$ , at $S T P$ .
Statement 2: The density of a gas at $S T P$ is found by dividing the molar mass by 22.4 litres.
The gas having smaller molar mass will have smaller density. The molar masses of ammonia and $A r$ are 17 $g / m o l$ and 39.9 $g / m o l$ respectively.
Both Statement 1 and Statement 2 are correct and Statement 2 is the correct explanation of Statement 1.

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Statement 1 : Ammonia gas, NH3 has a smaller density than argon gas, Ar, at STP.Statement 2: The density of a gas at STP is found by dividing the molar mass by 22.4 litres.

Statement 1 : Ammonia gas, $N H_{3}$ has a smaller density than argon gas, $A r$ , at $S T P$ .
Statement 2: The density of a gas at $S T P$ is found by dividing the molar mass by $22.4$ litres.