i. The initial pressure of `PCl_(5)` present in one litre vessel at `200 K` is `2` atm. At equilibrium the pressure increases to `3` atm with temperature increasing to `250`. The percentage dissociation of `PCl_(5)` at equilibrium is

The degree of dissociation of PCl_(5) will be more at ………. pressure.

The degree of dissociation of PCl_(5) decreases with increase in pressure.

120 mm of pressure is developed at equilibrium when PCl5 ​ at 100 mm is subjected to decomposition. Then the percentage of dissociation of PCl5 is

3 mole of PCl_(5) were heated in a vessel of three litre capacity. At equilibrium 40% of PCl_(5) was found to be dissociated. What will be the equilibrium constant for disscoiation of PCl_(5) ?

Ammonia gas at 15 atm is introduced in a rigid vessel at 300 K. At equilibrium the total pressure of the vessel is found to be 40.11 atm at 300^@C .The degree of dissociation of NH_3 will be :

0.1 mol of PCl_(5) is vaporised in a litre vessel at 260^(@)C . Calculate the concentration of Cl_(2) at equilibrium, if the equilibrium constant for the dissociation of PCl_(5) is 0.0414 .

1 mole of N_2 and 3 moles of PCl_5 are placed in a 100 litre vessels heated at 227^(@) C the equilibrium pressure is 2.05 atm Assuming ideal behaviour,Calculate degree of dissociation of PCl_5 and K_p for the reaction PCl_5 (g) hArr PCl_3 (g) + Cl_2(g)

1 mol of Cl_(2) and 3 mol of PCl_(5) are placed in a 100 L vessel heated to 227^(@)C . The equilibrium pressure is 2.05 atm. Assuming ideal behaviour, calculate the degree of dissociation for PCl_(5) and K_(p) for the reaction. PCl_(5)(g) hArr PCl_(3)(g)+Cl_(2)(g)

The vapour density of PCl_(5) at 43K is is found to be 70.2 . Find the degree of dissociation of PCl_(5) at this temperature.

Nitrogen gas is kept in an open beaker at 273 K and 1 atm pressure. If the pressure of the surrounding suddenly falls to 0.5 atm and the temperature increases to 546 K, then the percentage of nitrogen remaining in the beaker is mn% of the initial amount. Then the value of m+n is: