Advertisements
Advertisements
प्रश्न
Calculate the mole fraction of benzene in solution containing 30% by mass in carbon tetrachloride.
उत्तर
Let the total mass of the solution be 100 g, and the mass of benzene be 30 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 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
Thus, the mole fraction of C6H6 is given as:
`("Number of moles of C"_6"H"_6)/("Number of moles of C"_6"H"_6+"Number of moles of CCl"_4)`
= `0.385/(0.385+0.455)`
= 0.458
∴ Mole fraction of CCl4 = 1 − 0.458 = 0.542
APPEARS IN
संबंधित प्रश्न
Calculate (a) molality (b) molarity and (c) mole fraction of KI if the density of 20% (mass/mass) aqueous KI is 1.202 g mL−1.
Define Molality.
When KOH solution is added to potassium dichromate solution the colour of solution
changes to yellow, because _______
(A) chromate ion changes to dichromate ion
(B) dichromate ion changes to chromate ion
(C) oxidation number of chromium changes from + 6 to + 4
(D) oxidation number of chromium changes from + 4 to +6
Define molality.
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 the solution containing 7.1 g of Na2SO4 in 100 ml of aqueous solution is ____________.
10 g of NaCl is dissolved in 106 g of the solution. Its concentration is ____________.
5 ml of N HCl, 20 ml of N/2 H2SO4 and 30 ml of N/3 HNO3 are mixed together and volume made to one litre. The normality of the resulting solution is:
The volume of 4 N HCl and 10 N HCl required to make 1 litre of 6 N HCl are ____________.
200 ml of water is added to 500 ml of 0.2 M solution. What is the molarity of this diluted solution?
How many grams of concentrated nitric acid solution should be used to prepare 250 mL of 2.0M HNO3? The concentrated acid is 70% HNO3:
For preparing 0.1 N solution of a compound from its impure sample of which the percentage purity is known, the weight of the substance required will be:
A solution made by dissolving 40 g NaOH in 1000 g of water is ____________.
Which of the following units is useful in relating concentration of solution with its vapour pressure?
What is the mole fraction of solute in 1.00 m aqueous solutions?
Which of the following is a correct statement for C2H5Br?
Match the terms given in Column I with expressions given in Column II.
| Column I | Column II |
| (i) Mass percentage | (a) `"Number of moles of the solute component"/"Volume of solution in litres"` |
| (ii) Volume percentage | (b) `"Number of moles of a component"/"Total number of moles of all the components"` |
| (iii) Mole fraction | (c) `"Volume of the solute component in solution"/"Total volume of solution" xx 100` |
| (iv) Molality | (d) `"Mass of the solute component in solution"/"Total mass of the solution" xx 100` |
| (v) Molarity | (e) `"Number of moles of the solute components"/"Mass of solvent in kilograms"` |
Define the following modes of expressing the concentration of a solution. Which of these modes are independent of temperature and why?
V/V (volume percentage)
Calculate the mass percent of benzene (CoH6) and carbon tetrachloride (ccl4) if 22 g of benzene is dissolved in 122 g of carbon tetrachloride.
A sample of Ferrous sulphide reacts with dil. H2SO4 to from H2S which contains 9% hydrogen by volume. The percentage of fee in the sample, is ______.
