Chemical Equili...

If K_p​ for a reaction, A(g)+2B(g) ⇌ 3C(g) + D(g) is 0.05 atm at 1000K, its K_c​ in terms of R will be:

The vapour density of N₂​O₄​ at a certain temperature is 30. What is the percentage dissociation of N₂​O​₄ at this temperature ?

If PCl₅ is 80% dissociated at 523 K, what is the vapour density of the equilibrium mixture at 523 K ?

Ammonium carbamate when heated to 200⁰C gives a mixture of NH₃ and CO₂ with vapour density of 13.

The degree of dissociation of ammonium carbonate is:

In the reaction, H₂​(g)+I₂​(g) ⇌ 2HI(g) the concentration of H_2​, I₂​ and HI at equilibrium are 8.0, 3.0 and 28 moles per litre respectively. What will be the equilibrium constant ?

For the reaction, N₂(g) + 3H₂(g) ⇌ 2NH₃(g), the partial pressures of N₂ and H₂ are 0.80 and 0.40 atmosphere respectively at equilibrium. The total pressure of the system is 2.80 atmosphere. What is K_p for the above reaction?

A two litre flask contains 1.4 gm nitrogen and 1.0 gm hydrogen. The ratio of active mass of nitrogen and hydrogen would be -

The reaction A(g)+B(g) ⇋ C(g)+D(g) is studied in a one litre vessel at 250^∘C. The initial concentration of A was 3n and that of B was n. When equilibrium was attained, equilibrium concentration of C was found to be equal to the equilibrium concentration of B. What is the concentration of D at equilibrium?

The value of K_c​ for the reaction :

A + 3 B ⇌ ​2C at 400°C is 0.5. Calculate the value of K_P​

Two moles of ammonia was introduced in an evacuated vessel of 1L capacity. At high temperature, the gas undergoes partial dissociation according to the equation:

2NH₃​(g) ⇌ N₂​(g) + 3H₂​(g)

At equilibrium the concentration of ammonia was found to be 1mol. What is the value of K ?