Unit 7: Chemical Equilibrium and Acids - Bases — Online MCQ Test
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.
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....
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Unit 7: Chemical Equilibrium and Acids - Bases — Important Questions & Answers
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.
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.
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.
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.
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)?
- A. Kp = Kc because Δn = 0
- B. Kp = Kc(RT)
- C. Kp = Kc(RT)²
- D. Kp = Kc/RT
Answer: B. Kp = Kc(RT)
Here Δn = 2 - 1 = 1, so Kp = Kc(RT)^1 = Kc(RT).
Here Δn = 2 - 1 = 1, so Kp = Kc(RT)^1 = Kc(RT).