Equilibrium — Class 11 Chemistry NCERT Solutions (Free)

Free step-by-step NCERT solutions for Class 11 Chemistry chapter "Equilibrium" — 9 important questions with detailed answers for CBSE board exam preparation.

TL;DR: Free step-by-step NCERT solutions for Class 11 Chemistry chapter "Equilibrium" — 9 important questions with detailed answers for CBSE board exam prepa…

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Key Questions Covered:

  1. Define equilibrium constant Kc. How does it differ from Kp?
  2. Calculate Kc for the reaction: H2 + I2 ⇌ 2HI at equilibrium when [H2] = 0.5 M…
  3. What does Le Chatelier's principle state? Give an example with the Haber proc…
  4. + 6 more questions in the full chapter

Solutions Summary:

Question Status
Define equilibrium constant Kc. How does it differ from Kp? ✓ Solved
Calculate Kc for the reaction: H2 + I2 ⇌ 2HI at equilibri… ✓ Solved
What does Le Chatelier's principle state? Give an example… ✓ Solved

Showing 3 of 9 questions

Q1: Define equilibrium constant Kc. How does it differ from Kp?

Equilibrium constant Kc is the ratio of concentrations of products to reactants, each raised to their stoichiometric coefficients at equilibrium. For reaction: aA + bB ⇌ cC + dD Kc = [C]^c [D]^d / [A]^a [B]^b Difference from Kp: - Kc uses molar concentrations (mol/L) - Kp uses partial pressures (a...

Q2: Calculate Kc for the reaction: H2 + I2 ⇌ 2HI at equilibrium when [H2] = 0.5 M, [I2] = 0.5 M, [HI] = 1 M

Given reaction: H2 + I2 ⇌ 2HI Equilibrium concentrations: [H2] = 0.5 M [I2] = 0.5 M [HI] = 1 M Kc = [HI]^2 / ([H2][I2]) Kc = (1)^2 / (0.5 × 0.5) Kc = 1 / 0.25 Kc = 4 Therefore, the equilibrium constant Kc = 4 (dimensionless for this reaction)

Q3: What does Le Chatelier's principle state? Give an example with the Haber process.

Le Chatelier's Principle states: When a system in equilibrium is disturbed, it shifts to counteract the disturbance and restore equilibrium. Haber Process: N2(g) + 3H2(g) ⇌ 2NH3(g), ΔH = -92.4 kJ/mol Applications: 1. Increase pressure: Shifts RIGHT (fewer moles of gas on products side: 4 mol ->...

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