Home
Class 12
CHEMISTRY
Per two gram of charcoal, a gas is adsor...

Per two gram of charcoal, a gas is adsorbed by 0.1 g and 0.2 g at 10 torr and 80 torr pressure respectively. Calculate the n value in Freundlich adsorption isotherm.

Text Solution

AI Generated Solution

To solve the problem, we will use the Freundlich adsorption isotherm equation, which is given by: \[ \frac{x}{m} = k \cdot p^{\frac{1}{n}} \] Where: - \( x \) = mass of gas adsorbed ...
Promotional Banner

Similar Questions

Explore conceptually related problems

The pressure of a gas is 2.5 atm . Calculate the value in torr.

The vapour preesure of two pure liquids A and B are 5 and 10 torr respectively. Calculate the total pressure of the solution (in torr) obtained by mixing 2 mole of A and 3 mole of B.

One gram of charcoal adsorbs 400 " mL of " 0.5 M acetic acid to form a mono layer and the molarity of acetic acid reduced to 0.49. Calculate the surface area of charcoal adsorbed by each molecule of acetic acid. The surface area of charcoal is 3.01xx10^(2)m^(2)g^(-1) .

The density of a gas is found to be 1.56 g dm^(-3) at 0.98 bar pressure and 65^(@)C . Calculate the molar mass of the gas.

1.0 g of a metal oxide gave 0.2 g of metal. Calculate the equivalent weight of the metal.

The mass of 525 cm^(3) of a gaseous compound at 28^(@)C and 730 torr was found to be 0.900 g. Calculate the molar mass of the compound.

At 27^@C , a cylinder of 20 L capacity contains three gases He, O_2 " and " N_2 . Their masses are 0.502 g, 0.250 g and 1.00 g respectively. If all these gases behave ideally, calculate the partial pressure of each gas as well as the total pressure.

At 70^@C vapour pressure of pure benezene and pure toluene are 500 torr and 200 torr, respectively. In a homogeneous mixture of toluene with benzene at 70^@C , the mole fraction of benezene is 0.4. Calculate the vapour pressure of the mixture.

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) .

4 g of O_2 and 2g of H_2 are confined in a vessel of capacity 1 litre at 0^@C . Calculate the partial pressure of each gas, and