At 500 K, equilibrium constant, \[\ce{K_c}\], for the following reaction is 5. \[\ce{1/2 H2 (g) + 1/2 I2 (g) ⇌ HI (g)}\] What would be the equilibrium constant \[\ce{K_c}\] for the reaction \[\ce{2HI (g) ⇌ H2 (g) + I2 (g)}\]

At 500 K, equilibrium constant, KXc, for the following reaction is 5. 12HX2(g)+12IX2(g)↽−−⇀HI(g) What would be the equilibrium constant KXc for the reaction 2HI(g)↽−−⇀HX2(g)+IX2(g) - Chemistry

प्रश्न

At 500 K, equilibrium constant, $K_{c}$ , for the following reaction is 5.

$\frac{1}{2} H_{2} (g) + \frac{1}{2} I_{2} (g) \overset{- ⇀}{↽ -} HI (g)$

What would be the equilibrium constant $K_{c}$ for the reaction

$2 HI (g) \overset{- ⇀}{↽ -} H_{2} (g) + I_{2} (g)$

पर्याय

0.04
0.4
25
2.5

MCQ

उत्तर

0.04

Explanation:

If the equation is multiplied by 2, the equilibrium constant for the new equation is the square of $K$ it means we must do the square of 5 that is 25. Then and on reversing the reaction the value of the equilibrium constant is inversed means the value of K comes out to be 1/25 = 0.04.

shaalaa.com

Law of Chemical Equilibrium and Equilibrium Constant

या प्रश्नात किंवा उत्तरात काही त्रुटी आहे का?

Q 18 Q 17 Q 19

पाठ 7: Equilibrium - Multiple Choice Questions (Type - I) [पृष्ठ ८९]

APPEARS IN

एनसीईआरटी एक्झांप्लर Chemistry [English] Class 11

पाठ 7 Equilibrium
Multiple Choice Questions (Type - I) | Q 18 | पृष्ठ ८९

संबंधित प्रश्‍न

Write the expression for the equilibrium constant, Kc for the following reactions:

$2 Cu (NO_{3})_{2} (s) \overset{- ⇀}{↽ -} 2 CuO (s) + 4 NO_{2} (g) + O_{2} (g)$

Write the expression for the equilibrium constant, K_c for following reactions:

$Fe^{3 +} (aq) + 3 OH^{-} (aq) \overset{- ⇀}{↽ -} Fe (OH)_{3} (s)$

Nitric oxide reacts with Br₂ and gives nitrosyl bromide as per reaction given below:

$2 NO (g) + Br_{2} (g) \overset{- ⇀}{↽ -} 2 NOBr (g)$

When 0.087 mol of NO and 0.0437 mol of Br₂ are mixed in a closed container at the constant temperature, 0.0518 mol of NOBr is obtained at equilibrium. Calculate the equilibrium amount of NO and Br₂.

One mole of H₂O and one mole of CO are taken in 10 L vessel and heated to 725 K. At equilibrium, 40% of water (by mass) reacts with CO according to the equation,

$H_{2} O (g) + CO (g) \overset{- ⇀}{↽ -} H_{2} (g) + CO_{2} (g)$

Calculate the equilibrium constant for the reaction.

Calculate a) ΔG°and b) the equilibrium constant for the formation of NO₂ from NO and O₂ at 298 K

$NO (g) + \frac{1}{2} O_{2} (g) \overset{- ⇀}{↽ -} NO_{2} (g)$

where Δ_fG^⊝ (NO₂) = 52.0 kJ/mol

Δ_fG^⊝ (NO) = 87.0 kJ/mol

Δ_fG^⊝ (O₂) = 0 kJ/mol

Does the number of moles of reaction products increase, decrease or remain same when each of the following equilibria is subjected to a decrease in pressure by increasing the volume?

$3 Fe (s) + 4 H_{2} O (g) \overset{- ⇀}{↽ -} Fe_{3} O_{4} (s) + 4 H_{2} (g)$

The value of K_c for the reaction 3O₂ (g) ↔ 2O₃ (g) is 2.0 ×10^–50 at 25°C. If the equilibrium concentration of O₂ in the air at 25°C is 1.6 ×10^–2, what is the concentration of O₃?

On increasing the pressure, in which direction will the gas phase reaction proceed to re-establish equilibrium, is predicted by applying the Le Chatelier’s principle. Consider the reaction.

$N_{2} (g) + 3 H_{2} (g) \overset{- ⇀}{↽ -} 2 NH_{3} (g)$

Which of the following is correct, if the total pressure at which the equilibrium is established, is increased without changing the temperature?

The equilibrium constant for the reaction is ______ × 10²⁶.

$Fe + CuSO_{4} \overset{- ⇀}{↽ -} FeSO_{4} + Cu$ at 25°C.

Given $E_{Fe / {Fe}^{2 +}}^{0}$ = 0.44 V

$E_{Cu / {Cu}^{2 +}}^{0}$ = - 0.337 V

The decomposition of N₂O₄ to NO₂ was carried out in chloroform at 280°C. At equilibrium, 0.2 mol of N₂O₄ and 2 × 10⁻³ mol of NO₂ were present in 2 ℓ of the solution. The equilibrium constant for the reaction $N_{2} O_{4} \overset{- ⇀}{↽ -} 2 NO_{2}$ is ______.

At 500 K, equilibrium constant, KXc, for the following reaction is 5. 12HX2(g)+12IX2(g)↽−−⇀HI(g) What would be the equilibrium constant KXc for the reaction 2HI(g)↽−−⇀HX2(g)+IX2(g) - Chemistry

Advertisements

Advertisements

प्रश्न

पर्याय

उत्तर

APPEARS IN

संबंधित प्रश्‍न

Select a course

At 500 K, equilibrium constant, KXc, for the following reaction is 5. 12HX2(g)+12IX2(g)↽−−⇀HI(g) What would be the equilibrium constant KXc for the reaction 2HI(g)↽−−⇀HX2(g)+IX2(g) - Chemistry

Advertisements

Advertisements

प्रश्न

पर्याय

उत्तरShow Solution

APPEARS IN

संबंधित प्रश्‍न

Select a course

उत्तर