Chapter Exam

Unit 7: Chemical Equilibrium and Acids - Bases — Online MCQ Test

Q: What is the expression for the equilibrium constant Kc for the reaction N2(g) + 3H2(g) ⇌ 2NH3(g)?

Answer: A. [NH3]^2 / ([N2][H2]^3) — For a balanced reaction, Kc is written as product concentrations raised to their stoichiometric coefficients divided by reactant concentrations similarly raised.

Q: According to Arrhenius theory, an acid is a substance that:

Answer: B. increases the concentration of H⁺ ions in water — Arrhenius acids produce H⁺ ions in aqueous solution, while Arrhenius bases produce OH⁻ ions.

Q: If the pressure of a gaseous equilibrium system is increased, the equilibrium shifts toward the side having:

Answer: B. fewer moles of gas — By Le Chatelier's principle, increasing pressure favors the side with fewer gaseous moles to reduce pressure.

Q: For the reaction 2SO2(g) + O2(g) ⇌ 2SO3(g), which change will favor SO3 formation at constant temperature?

Answer: C. Increasing the pressure — The forward reaction has fewer moles of gas on the product side. Higher pressure shifts equilibrium toward SO3 formation.

Q: Which statement about Kp and Kc is correct for the equilibrium N2O4(g) ⇌ 2NO2(g)?

Answer: B. Kp = Kc(RT) — Here Δn = 2 - 1 = 1, so Kp = Kc(RT)^1 = Kc(RT).

CHEMISTRY · CLASS 11 INTERMEDIATE 1 YEAR · Telangana State Board

Practice Unit 7: Chemical Equilibrium and Acids - Bases with a free chapter-wise online MCQ test for Telangana State Board CLASS 11 INTERMEDIATE 1 YEAR CHEMISTRY. This chapter covers: Focusing on dynamic equilibrium this chapter covers law of mass action equilibrium constants Kc and Kp Le Chatelier principle and ionic equilibrium. Students study Arrhenius Bronst.... AI-generated questions from basic to board-exam level, with instant results and explanations.

Questions

20m

Time Limit

Attempts Left

10 random questions from this chapter (mixed difficulty)
Questions you've seen before won't repeat until the pool resets
You have 20 minutes — exam auto-submits when time is up
Maximum 3 attempts per chapter
Results and explanations shown immediately after submission

New here? Register free — includes 3 free chapter exams.

Unit 7: Chemical Equilibrium and Acids - Bases — Important Questions & Answers (FAQ)

Frequently asked questions from Telangana State Board CLASS 11 INTERMEDIATE 1 YEAR CHEMISTRY — Unit 7: Chemical Equilibrium and Acids - Bases, with answers and explanations. These are sample questions; the exam has its own separate question set.

What is the expression for the equilibrium constant Kc for the reaction N2(g) + 3H2(g) ⇌ 2NH3(g)?

A. [NH3]^2 / ([N2][H2]^3) ✓
B. ([N2][H2]^3) / [NH3]^2
C. [NH3] / ([N2][H2])
D. [N2]^2 / ([H2]^3[NH3])

Answer: A. [NH3]^2 / ([N2][H2]^3)
For a balanced reaction, Kc is written as product concentrations raised to their stoichiometric coefficients divided by reactant concentrations similarly raised.

According to Arrhenius theory, an acid is a substance that:

A. increases the concentration of OH⁻ ions in water
B. increases the concentration of H⁺ ions in water ✓
C. donates a pair of electrons
D. accepts a pair of electrons

Answer: B. increases the concentration of H⁺ ions in water
Arrhenius acids produce H⁺ ions in aqueous solution, while Arrhenius bases produce OH⁻ ions.

If the pressure of a gaseous equilibrium system is increased, the equilibrium shifts toward the side having:

A. more moles of gas
B. fewer moles of gas ✓
C. higher molar mass
D. more solid products

Answer: B. fewer moles of gas
By Le Chatelier's principle, increasing pressure favors the side with fewer gaseous moles to reduce pressure.

For the reaction 2SO2(g) + O2(g) ⇌ 2SO3(g), which change will favor SO3 formation at constant temperature?

A. Increasing the volume
B. Adding a catalyst
C. Increasing the pressure ✓
D. Removing SO3 and decreasing pressure

Answer: C. Increasing the pressure
The forward reaction has fewer moles of gas on the product side. Higher pressure shifts equilibrium toward SO3 formation.

Which statement about Kp and Kc is correct for the equilibrium N2O4(g) ⇌ 2NO2(g)?