Law of Chemical Equilibrium and Equilibrium Constant

What is K_c for the following equilibrium when the equilibrium concentration of each substance is: [SO₂] = 0.60 M, [O₂] = 0.82 M and [SO₃] = 1.90 M?

\[\ce{2SO2(g) + O2(g) ⇌ 2SO3(g)}\]

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

\[\ce{CH3COOC2H5(aq) + H2O(l) ⇌CH3COOH (aq) + C2H5OH (aq)}\]

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

\[\ce{I2 (s) + 5F2 ⇌ 2IF5}\]

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

\[\ce{2NO(g) + Br2 (g) ⇌ 2NOBr (g)}\]

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, 

\[\ce{H2O (g) + CO (g) ⇌ H2 (g) + CO2 (g)}\] 

Calculate the equilibrium constant for the reaction.

At 700 K, the equilibrium constant for the reaction

\[\ce{H_{2(g)} + I_{2(g)} ↔ 2HI_{(g)}}\] 

is 54.8. If 0.5 molL^–1 of HI_(g) is present at equilibrium at 700 K, what are the concentration of H_2(g) and I_2(g) assuming that we initially started with HI_(g) and allowed it to reach equilibrium at 700 K?

K_p = 0.04 atm at 899 K for the equilibrium shown below. What is the equilibrium concentration of C₂H₆ when it is placed in a flask at 4.0 atm pressure and allowed to come to equilibrium?

\[\ce{C2H6 (g) ⇌ C2H4 (g) + H2 (g)}\]

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?

\[\ce{3Fe (s) + 4H2O (g) ⇌ Fe3O4 (s) + 4H2 (g)}\]