If 0.44g of a colourless oxide of nitrogen occupies 224 ml at 1520 mm of Hg and 273⁰C

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If 0.44g of a colourless oxide of nitrogen occupies 224 ml at 1520 mm of Hg and 273⁰C, then the compound is

Options

(a) N₂O
(b) NO₂
(c) NO₄
(d) N₂O₂

Correct Answer:

N₂O

Explanation:

Here, w = 0.44 g
P = 1520 mm of Hg = 2 atm, T = 273⁰C = 546 K
V = 224 mL = 0.224 L, R = 0.0821 L atm K⁻¹mol⁻¹
M = Molecular Weight
According to ideal gas equation, PV = (w / M) RT
2 × 0.224 = (0.44 / M) × 0.0821 × 546
Given: M = 44
.·. The compound is N₂O.

Related Questions:

1. In which of the following pairs, both the species are not isostructural ?
2. A compound that undergoes bromination easily is
3. A 6 volume sample of H₂O₂
4. Which of the following pairs of a chemical reaction is certain to result
5. Which one of the following is a chain growth polymer

Topics: States of Matter Gases and Liquids (80)
Subject: Chemistry (2512)

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