Advertisements
Advertisements
प्रश्न
Calculate the mole fraction of benzene in solution containing 30% by mass in carbon tetrachloride.
Advertisements
उत्तर
Given: Mass of benzene in the solution = 30 g
Let the mass of the solution = 100 g
∴ Mass of carbon tetrachloride = (100 − 30) g
= 70 g
Molar mass of benzene (C6H6) = (6 × 12 + 6 × 1) g mol−1
= 78 g mol−1
∴ Number of moles of benzene (C6H6) = `"Mass"/"Molar mass"`
= `(30 "g")/(78 "g mol"^(−1))`
= 0.385 mol
Molar mass of carbon tetrachloride (CCl4) = 1 × 12 + 4 × 35.5
= 154 g mol−1
∴ Number of moles of CCl4 = `"Mass"/"Molar mass"`
= `(70 "g")/(154 "g mol"^(−1))`
= 0.455 mol
Mole fraction of benzene (C6H6) = `"Number of moles of benzene"/("Number of moles of benzene" + "Number of moles of Carbon tetrachloride")`
= `0.385/(0.385 + 0.455)`
= `0.385/0.84`
= 0.458
∴ Mole fraction of CCl4 = 1 − 0.458
= 0.542
∴ The mole fraction of benzene in a solution containing 30% by mass of carbon tetrachloride is 0.542.
APPEARS IN
संबंधित प्रश्न
Define mole fraction.
A solution is obtained by mixing 300 g of 25% solution and 400 g of 40% solution by mass. Calculate the mass percentage of the resulting solution.
If the density of some lake water is 1.25 g mL−1 and contains 92 g of Na+ ions per kg of water, calculate the molality of Na+ ions in the lake.
If the solubility product of CuS is 6 × 10−16, calculate the maximum molarity of CuS in aqueous solution.
Nalorphene (C19H21NO3), similar to morphine, is used to combat withdrawal symptoms in narcotic users. Dose of nalorphene generally given is 1.5 mg. Calculate the mass of 1.5 × 10−3 m aqueous solution required for the above dose.
22.22 gram of urea was dissolved in 300 grams of water. Calculate the number of moles of urea and molality of the urea solution.
(Given: Molar mass of urea = 60 gram mol−1)
Define Normality.
Molality of a solution relates the ____________.
The sum of all mole fraction for a mixture is always equal to ____________.
1 M, 2.5 litre NaOH solution is mixed with another 0.5 M, 3 litre NaOH solution. Then find out the molarity of the resultant solution:
The molarity of pure water is ____________.
An aqueous solution of glucose is 10% in strength. The volume in which 1 g mole of it is dissolved, will be:
Mole fraction of the solute in a 1.00 molal aqueous solution is ____________.
Given below are two statements labelled as Assertion (A) and Reason (R).
Assertion (A): Molarity of a solution changes with temperature.
Reason (R): Molarity is a colligative property.
Select the most appropriate answer from the options given below:
What is the ratio of mass of an electron to the mass of a proton?
A solution has been prepared by dissolving 5 g of urea in 95 g of water. What is the mass percentage of urea in the solution?
What is the normality of 0.3 m H3Pcl solution?
4.5 g of compound A (MW = 90) was used to make 250 mL of its aqueous solution. The molarity of the solution in M is x × 10−1. The value of x is ______. (Rounded-off to the nearest integer)
The molarity of the solution prepared by dissolving 6.3 g of oxalic acid (H2C2O4 · 2 H2O) in 250 mL of water in mol L-1 is x × 10-2. The value of x is ______. (Nearest integer)
[Atomic mass: H : 1.0, C : 12.0, O : 16.0]
