Home
Class 12
CHEMISTRY
Cyclohexane and ethanol at a particular ...

Cyclohexane and ethanol at a particular temperature have vapour presure of 280 mm and 168 mm respectively. If these two solutions having mole fraction value of cyclohexane equal to `0.32` are mixed and the mixture has a total vapour pressure of 376 mm, will the mixture be an ideal solution ?

Text Solution

AI Generated Solution

To determine whether the mixture of cyclohexane and ethanol is an ideal solution, we will follow these steps: ### Step 1: Calculate the mole fraction of ethanol Given the mole fraction of cyclohexane (X_cyclohexane) is 0.32, we can find the mole fraction of ethanol (X_ethanol) using the formula: \[ X_{\text{ethanol}} = 1 - X_{\text{cyclohexane}} = 1 - 0.32 = 0.68 \] ...
Promotional Banner

Similar Questions

Explore conceptually related problems

Two liquids A and B have vapour pressure of 0.600 bar and 0.2 bar, respectively. In an ideal solution of the two, calculate the mole fraction of A at which the two liquids have equal partial pressures.

The vapour pressure of benzene and toluene are 150 mm and 50 mm respectively. A solution is prepared by mixing equal weights of benzene and toluene. Assuming the solution to be ideal, calculate the vapour pressure of the solution.

The vapour pressure of water at room temperature is 23.8 mm Hg. The vapour pressure of an aqueous solution of sucrose with mole fraction 0.1 is equal to

The vapour pressure of pure liquids A and B is 450 and 700mm Hg , respectively, at 350K. Find out the composition of the liquid mixture if the total vapour pressure is 600mm Hg . Also find the composition of the vapour phase.

At a constant temperature liquid 'A' has vapour pressure of 170 mm Hg and liquid 'B' has vapour pressure of 280 mm Hg . A solution of the two at the same temperature in which mole fraction of A is 0.7 has a total vapour pressure of 376 mm . Identify whether the solution process is Endothermic or Exothermic ?

In a mixture of A and B having vapour pressure of pure A and B are 400 m Hg and 600 mm Hg respectively. Mole fraction of B in liquid phase is 0.5. Calculate total vapour pressure and mole fraction of A and B in vapour phase .

Vapour pressure of pure liquids P and Q are 700 and 450 mm Hg respectively at 330K. What is the composition of the liquid mixture at 330 K, if the total vapour pressure is 600 mm Hg?

At 35^(@) C the vapour pressure of CS_(2) is 512 mm Hg and of asetone is 344 mm Hg.A solution of Cs_(2) and acetone in which the mole fraction of CS_(2) is 0.25, has a total vapour pressure of600 mmHg .which of the following Statement is /are correct?

The vapour pressure of ethanol and methanol are 44.0 mm and 88.0 mm Hg , respectively. An ideal solution is formed at the same temperature by mixing 60 g of ethanol with 40g of methanol. Calculate the total vapour pressure of the solution and the mole fraction of methanol in the vapour.

The vapour pressures of pure liquids A and B are 400 and 600 mm Hg respectively at 298 K. On mixing the two liquids, the sum of their initial volumes is equal to the volume of the final mixture. The mole fraction of liquid B is 0.5 in the mixture. The vapour pressure of the final solution, the mole fractions of components A and B in vapour phase, respectively are :