Q. No.The equilibrium constant for the reaction:
N2(g) + O2 (g) ⇄ 2NO(g) is K.
What will be the equilibrium constant for the reaction: \(\frac{1}{2}\)N2(g) + \(\frac{1}{2}\)O2(g) ⇄ NO(g)?
1.
2.
3. K
4.
Aqueous solution of which of the following compounds is the best conductor of electric current?
| 1. | Acetic acid, \(\mathrm{C_{2} H_{4} O_{2}}\) | 2. | Hydrochloric acid, \(\mathrm{HCl}\) |
| 3. | Ammonia, \(\mathrm{N H_{3}}\) | 4. | Fructose, \(\mathrm{C_{6} H_{12} O_{6}}\) |
The value of the equilibrium constant for a particular reaction is 1.6 × 1012. When the system is in equilibrium, it will include:
1. All reactants
2. Mostly reactants
3. Mostly products
4. Similar amounts of reactants and products
Which of the following salts will give the highest pH in water?
1. KCl
2. NaCl
3. Na2CO3
4. CuSO4
Find the condition that shifts the following exothermic equilibrium towards the formation of NH₃:
N₂(g) + 3H₂(g) ⇌ 2NH₃(g) + heat
1. Increasing the concentration of NH₃2. Decreasing the pressure
3. Decreasing the concentration of H₂
4. Increasing the pressure and decreasing the temperature
A buffer solution is prepared in which the concentration of NH3 is 0.30 M and the concentration of is 0.20 M. If the equilibrium constant, Kb for NH3 equals 1.8×10–5, then what is the pH of this solution?
(log 1.8 = 0.25; log 0.67 = –0.176)
1. 9.43
2. 11.72
3. 8.73
4. 9.08
Find the equilibrium constant K for the reaction:
NO₂(g) ⇌ ½N₂(g) + O₂(g)
Given:
N₂(g) + O₂(g) ⇌ 2NO(g), K₁
2NO(g) + O₂(g) ⇌ 2NO₂(g), K₂
1. 4K₁K₂2. [1/(K₁K₂)]¹ᐟ²
3. 1/(K₁K₂)
4. 1/(2K₁K₂)
| 1. | \(0 . 5 \times \left(10\right)^{- 10}\) | 2. | \(0 . 5 \times \left(10\right)^{- 15}\) |
| 3. | \(0 . 25 \times \left(10\right)^{- 10}\) | 4. | \(0 . 125 \times \left(10\right)^{- 15}\) |
When equal volumes of 0.1 M NaOH and 0.01 M HCl are mixed, the pH of the resulting solution will be:
| 1. | 12.65 | 2. | 2.0 |
| 3. | 7.0 | 4. | 1.04 |
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