Question

Which of these statement(s) is/are true about a balloon filled with 1.00 mol N2 (g) at STP?

Answer 1

Answer:

I. The balloon has a volume of 22.4L

III. The balloon contains 6.022x10^23 molecules.

Explanation:

At stp, it has been proven that 1mole of a gas occupy 22.4L.

Therefore, option (i) is correct.

The molar mass N2 = 14.01 x 2 = 28.02g/mol

Number of mole of N2 = 1 mole

Mass of N2 =..?

Mass = mole x molar Mass

Mass of N2 = 1 x 28.02 = 28.02g.

The mass content of the balloon is 28.02g, therefore, option (ii) is wrong.

From Avogadro's hypothesis, we understood that 1 mole of any substance contains 6.02x10^23 molecules. This implies that 1 mole of N2 also contains 6.02x10^23 molecules

Therefore, option (iii) is correct.

The correct options to the question are:

Option i and option iii

Answer 2

Answer:

I and III are correct

Explanation:

Hello,

In this case, I. and III. are true since:

I. the STP conditions are referred to 273 K and 1 atm, therefore the volume is:

$V=\frac{nRT}{P}=\frac{1mol*0.082\frac{atm*L}{mol*K}*273K}{1atm}=22.4L$

II. In 1 mole of nitrogen (N₂) there are 28.02 g as it is diatomic, therefore this is false.

III. 1 mole of a substance, in this case nitrogen, equals 6.022x10²³ (Avogadro's number) particles, in this case molecules

Best regards.