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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: - For an endothermic reaction, energy of activation is Ea and enthalpy of reaction
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Topics: States of Matter Gases and Liquids
(80)
Subject: Chemistry
(2512)
Important MCQs Based on Medical Entrance Examinations To Improve Your NEET Score
- For an endothermic reaction, energy of activation is Ea and enthalpy of reaction
- Oxidation numbers of carbon in CH₂Cl₂,CO₂ and CO₃²⁻ are respectively
- How many mole of MNO₄⁻ ion will react with 1 mole of ferrous oxalate in acidic medium
- Which of the following orders of ionic radii is correctly represented
- If n = 6, the correct sequence for filling of electrons will be:
Topics: States of Matter Gases and Liquids (80)
Subject: Chemistry (2512)
Important MCQs Based on Medical Entrance Examinations To Improve Your NEET Score
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