Q. No.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 NH₃
2. 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. | \(0 . 125 \times \left(10\right)^{- 15}\) |
Which of the following salts will give the highest pH in water?
1. KCl
2. NaCl
3. Na2CO3
4. CuSO4
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
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 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.
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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