- 1(current)
Q. No.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
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)
Find the equilibrium constant for the reaction:
SO₃(g) ⇌ SO₂(g) + ½O₂(g)
Given:
2SO₂(g) + O₂(g) ⇌ 2SO₃(g), K = 278
1. 3.6 × 10⁻³2. 6.0 × 10⁻²
3. 1.3 × 10⁻⁵
4. 1.8 × 10⁻³
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.
A 20-litre container at 400 K contains CO2 (g) at pressure 0.4 atm and an excess of SrO (neglecting the volume of solid SrO). The volume of the container is now decreased by moving the movable piston fitted in the container.
The maximum volume of the container, when the pressure of CO2 attains its maximum value will be:
(Given that: SrCO3(s) ⇋ SrO(s) + CO2(g) , Kp = 1.6 atm)
| 1. | 10 litre | 2. | 2 litre |
| 3. | 4 litre | 4. | 5 litre |
Consider the given equilibrium constants:
\(\mathrm{{N}_2+3 {H}_2 ~\rightleftharpoons 2 {NH}_3 ~~~~~~~{K}_1 \\ {N}_2+{O}_2 ~~~\rightleftharpoons 2 {NO} ~~~~~~~~{K}_2 \\ {H}_2+\frac{1}{2} {O}_2 \rightleftharpoons {H}_2 {O} ~~~~~~~~{K}_3}\)
The equilibrium constant (K) of the following reaction will be:
\(2 \mathrm{NH}_3+\frac{5}{2} \mathrm{O}_2 \stackrel{\mathrm{~K}}{\rightleftharpoons} 2 \mathrm{NO}+3 \mathrm{H}_2 \mathrm{O}\)
| 1. | \( \dfrac{K_{2}K_{3}^{3}}{K_{1}}\) | 2. | \( \dfrac{K_{2}K_{3}}{K_{1}}\) |
| 3. | \( \dfrac{K_{2}^{3}K_{3}}{K_{1}}\) | 4. | \( \dfrac{K_{3}^{3}K_{1}}{K_{2}}\) |
Cu(OH)2(s) + 4 NH3(aq) \(\leftrightharpoons\) Cu(NH3)42+(aq) + 2 OH¯(aq)
| 1. | Keq = \(\dfrac{[Cu(NH_3)_4^{2+}][OH^-]}{[NH_3]}\) |
| 2. | Keq = \(\dfrac{[Cu(NH_3)_4^{2+}][2~OH^-]}{[4~NH_3]}\) |
| 3. | Keq = \(\dfrac{[Cu(NH_3)_4^{2+}][OH^-]^2}{[NH_3]^4}\) |
| 4. | Keq = \(\dfrac{[Cu(NH_3)_4^{2+}][2~OH^-]^2}{[4~NH_3]^4}\) |
\(H_2NCOONH_4 (s) \rightleftharpoons2 NH_3(g) + CO_2(g)\), the total pressure at equilibrium is 15 atmospheres. It can be concluded that the value of \(K_P\) will be:
1. 15 atm3
2. 50 atm3
3. 500 atm3
4. 100 atm3
Which of the following reactions satisfies the condition \(K_p>K_c \text { ? }\)
1. H2(g) + I2(g) → 2HI(g)
2. N2(g) + 3H2(g) → 2NH3(g)
3. 2SO3(g) → 2SO2(g) + O2(g)
4. PCl3(g) + Cl2(g) → PCl5(g)
For the equilibrium of the reaction,\(\mathrm{HgO}(\mathrm{~s}) \rightleftharpoons \mathrm{Hg}(\mathrm{~g})+\frac{1}{2} \mathrm{O}_ 2(\mathrm{~g}), \mathrm{K_P}\) for the reaction at a total pressure of "P" will be:
| 1. | \(\mathrm{K}_P={2 \over 3^{3/2}}\mathrm P^{3/2}\) | 2. | \(\mathrm{K}_P={2 \over 3^{1/2}}\mathrm P^{1/2}\) |
| 3. | \(\mathrm{K}_P={1 \over 3^{2/3}}\mathrm P^{3/2}\) | 4. | \(\mathrm{K}_P={1 \over 3^{2/3}}\mathrm P\) |
- 1(current)
Q. No.
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