The pressure of iodine gas at `1273 K` is found to be `0.112` atm whereas the expected

At 1000^@C the pressure of iodine gas is found to be 0.112 atm whereas the expected pressure is 0.074 atm. The increased pressure is due to dissociation, I_2 hArr 2I . Calculate K_p . Also find out pressure at which I_2 will be 90% dissociation at 1000^@C .

The pressure of iodine gas at a particular temperature is found to be 0.111atm , where as the expected pressure is 0.074 atm , the increased pressure is due to I_(2)hArr 2I . Calculate K_(p) for this equilibrium.

At 1000K, the pressure of iodine gas is found to be 0.112 atm due to partial dissociation of I_(2)(g) into I(g). Had there been no dissociation, the pressure would have been 0.074 atm. Calculate the value of K_(p) for the reaction: I_(2)(g) hArr 2I(g) .

At 1000K , the pressure of iodine gas is found to be 0.1 atm due to partial dissociation of I_(2)(g) into I(g) . Had there been no dissociation, the pressure would have been 0.07 atm . Calculate the value of K_(p) for the reaction: I_(2)(g)hArr2I(g) .

Osmotic pressure of insulin solution at 298 K is found to be 0.0072atm . Hence, height of water Column due to this pressure is

A cylinder contains oxygen at pressure of 28 atm and at a temperature of 300 K. the mass of oxygen the gas, the pressure is found to be 7 atm and the temperature is 200 K. what mass of the gas has been used?

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 :