An oxide of nitrogen 30.43% nitrogen and its one molecule has mass of Which of the 1.527×10−22g. following statement(s) regarding this oxide is/are true?

Mass of one molecule 1.527 × 10 − 22 g Mass of molecule 1.527 × 10 − 22 × 6.023 × 10 23 = 92 gm m m M 0 = 30.43 100 × 92 = 28 gm atom of N = 28 14 = 2 m 0 = 92 − 28 = 64 gm atom of O = 64 16 = 4

Book Online Demo

Check Your IQ

Try Test

Courses

Dropper NEET Course Dropper JEE Course Class - 12 NEET Course Class - 12 JEE Course Class - 11 NEET Course Class - 11 JEE Course Class - 10 Foundation NEET Course Class - 10 Foundation JEE Course Class - 10 CBSE Course Class - 9 Foundation NEET Course Class - 9 Foundation JEE Course Class -9 CBSE Course Class - 8 CBSE Course Class - 7 CBSE Course Class - 6 CBSE Course

Offline Centres

An oxide of nitrogen 30.43% nitrogen and its one molecule has mass of Which of the $(1.527 \times 10^{- 22} g)$ . following statement(s) regarding this oxide is/are true?

see full answer

Talk to JEE/NEET 2025 Toppers - Learn What Actually Works!

Real Strategies. Real People. Real Success Stories - Just 1 call away

An Intiative by Sri Chaitanya

Its empirical formula is NO

Its empirical formula is ${NO}_{2}$

Its molecular formula is $N_{2} O_{4}$

Its molecular formula is $N_{2} O_{2}$

answer is B, C.

(Unlock A.I Detailed Solution for FREE)

Ready to Test Your Skills?

Check your Performance Today with our Free Mock Test used by Toppers!

Take Free Test

Detailed Solution

Mass of one molecule $(1.527 \times 10^{- 22} g)$

Mass of molecule $1.527 \times 10^{- 22} \times 6.023 \times 10^{23}$

$\begin{array}{l} = \frac{92 gm}{m} \\ m_{M_{0}} = \frac{30.43}{100} \times 92 = 28 gm \\ atom of N = \frac{28}{14} = 2 \\ m_{0} = 92 - 28 = 64 gm \\ atom of O = \frac{64}{16} = 4 \end{array}$