At a certain temperature and total pressure of `10^5`Pa,iodine vapour contains 40% by volume of 1 atoms`I_2(g) hArr 2I(g)` Calculate `K_p` for the equilibrium.

At 1127 K and 1 atm pressure , a gaseous mixtue of CO and CO_2 in equilibrium with solid carbon has 90.55% CO by mass C(s) + CO_2 hArr 2CO(g) Calculate K_c for this reaction at the above temperature.

A sample of HI(g) is placed in flask at a pressure of 0.2f atm.At equilibrium the partial pressure of HI(g) is 0.04 atm.What is K_p for the given equilibrium? 2HI (g) hArr H_2 (g) + I_2(g)

One mole of H_2O and one mole of CO are taken in 10L vessel and heated to 725 K.At equilibrium 40% of water (by mass) reacts with CO according to the equatin H_2O(g0 + CO(g) hArr H_2(g) +CO_2(g) Calculate the equilibrium constant for the reaction.

200 cm3 of an aqueous solution of a protein contain1.26g of the prote in.The osmotic pressure of such a solution at 300 K is found to be 2.57 xx 10^(-3) bar. Calculate the molarimass of-the protein.

A mixture of 1.57 mol of n_2 ,1.92 mol of H_2 and 8.13 mol of NH_3 is introduced into a 20 L reaction vessel at 500 kAt this temperature,the equilibrium constant. K_C for the reaction N_2(g) + 3H_2(g) hArr 2NH_3(g) is 1.7 xx 10 ^2 .Is the reaction mixture at equilibrium?If not,what is the direction of the net reaction?

One mole of an ideal gas is compressed from 500 cm3 against a constant external pressure of 1.2 xx 10^5 Pa The work involved in the process is 36.0 J. Calculate the final volume.

Write the expression for the equilibrium constant, K_C for each of the following reactions: I_2(s) +5F_2(g) hArr 2IF_5(l)

Write the expression for the equilibrium constant, K_C for each of the following reactions: 2NOCI(g) hArr 2NO (g) + CI_2(g)

Calculate the difference in heat of reaction at constant pressure and at constant volume at 300K. C_(s) + 2H_(2(g) rarr CH_(4(g) (R = 8.314 J K^(-1) mol^(-1)