Find the gaseous equilibrium for which Kp < Kc.
1. PCl₅(g) ⇌ PCl₃(g) + Cl₂(g)2. N₂(g) + O₂(g) ⇌ 2NO(g)
3. 2HI(g) ⇌ H₂(g) + I₂(g)
4. N₂(g) + 3H₂(g) ⇌ 2NH₃(g)
Find the value of Kp for the reaction:
N₂(g) + 3H₂(g) ⇌ 2NH₃(g)
Given: Kc = 0.5 at 400 K and R = 0.0821 L atm mol⁻¹ K⁻¹.
1. 25.6 × 10⁻²2. 4.6 × 10⁻⁴
3. 46.6 × 10⁻⁴
4. 16.6 × 10⁻⁸
Find the value of Kc for the reaction:
2SO₂(g) + O₂(g) ⇌ 2SO₃(g)
at 700 K, if
Kₚ = 1.3 × 10⁻³ atm⁻¹
1. 1.4 × 10⁻²2. 7.4 × 10⁻²
3. 5.2 × 10⁻²
4. 3.1 × 10⁻²
Find the ratio Kp/Kc for the reaction:
SO₂(g) + ½O₂(g) ⇌ SO₃(g)
1. (RT)1/2
2. (RT)-1/2
3. (RT)
4. 1
Find the equilibrium constant Kc for the reaction:
½N₂(g) + ½O₂(g) + ½Br₂(g) ⇌ NOBr(g)
Given:
2NO(g) ⇌ N₂(g) + O₂(g) Kc₁ = 2.5 × 10³⁰
NO(g) + ½Br₂(g) ⇌ NOBr(g) Kc₂ = 1.6
2. 2.02 × 10⁻¹⁵
3. 1.01 × 10³⁰
4. 2.02 × 10¹⁵
If Kp of the reaction is 0.05 at 1000 K, then the value of Kc of the reaction
1. 20000 R
2. 0.02 R
3.
4.
What will be the change in the concentration of Cl₂ when the equilibrium concentration of PCl₃ is doubled in the reaction:
PCl₅(s) ⇌ PCl₃(g) + Cl₂(g)?
1. Cl₂ becomes half of its initial concentration
2. Cl₂ becomes one-fourth of its initial concentration
3. Cl₂ becomes four times its initial concentration
4. Cl₂ becomes twice its initial concentration
In the reaction, the equilibrium concentrations of PCl5 and PCl3 are 0.4 and 0.2 mole/liter respectively. If the value of Kc is 0.5, what is the concentration of Cl2 in mole/liter?
1. 2.0
2. 1.5
3. 1.0
4. 0.5
4 moles each of SO2 and O2 gases are allowed to react to form SO3 in a closed vessel. At equilibrium, 25% of O2 is used up. The total number of moles of all the gases at equilibrium is
1. 6.5
2. 7.0
3. 8.0
4. 2.0
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