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

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.

admin:

Related Questions

  1. In which of the following compounds, nitrogen exhibits highest oxidation state
  2. Which of the following compounds is isomeric with 2,2,4,4-tetramethylhexane
  3. At 25⁰C, the dissociation constant of a base, BOH, is 1.0 ˣ 10⁻¹².
  4. Among the following the least thermally stable is
  5. Glucose molecule reacts with X number of molecules of phenylhydrazine to yield