a)
Molar mass of CCl4,
MM = 1*MM(C) + 4*MM(Cl)
= 1*12.01 + 4*35.45
= 153.81 g/mol
mass(CCl4)= 300 g
use:
number of mol of CCl4,
n = mass of CCl4/molar mass of CCl4
=(3*10^2 g)/(1.538*10^2 g/mol)
= 1.95 mol
Mole fraction of solute = mol of solute / total mol
= 0.150 / (0.150 + 1.95)
= 0.0714
Answer: 0.0714
b)
Mass of solvent = 300 g = 0.300 Kg
Use:
Molality = mol of solute / mass of solvent in Kg
= 0.150 mol / 0.300 Kg
= 0.500 m
Answer: 0.500 m
0.150 mol of a solute is dissolved in 300. g of carbon tetrachloride. Calculate (a) the...
0.150 mol of a solute is dissolved in 300. g of carbon tetrachloride. Calculate (a) the mole fraction and (b) the molality of solute.
A solution is 5.43 % by mass benzene (C_6H_6) in carbon tetrachloride (CCl_4). The density of the solution is 1.55 g/mL. The molar masses of benzene and carbon tetrachloride are 78.1 g/mol and 154 g/mol respectively. What is the mole fraction, molarity and molality of the benzene?
A solution is prepared by dissolving 16.2 g of benzene (C6H6) in 282 g of carbon tetrachloride (CCl4). The density of the solution is 1.55 g/mL. The molar masses of benzene and carbon tetrachloride are 78.1 g/mol and 154 g/mol respectively. What is the mass percent, mole fraction, molarity and molality of the benzene?
Determine the molarity of a solute when 0.150 mol of the solute is dissolved into enough solvent to give a total volume of 350 ml. О o 4.3х10 м 0.35 м 0.15 м 2.3м о 0.43 м О О
For each solute, identify the better solvent: water or carbon tetrachloride. Water, H2O Carbon tetrachloride, CCl4
For each solute, identify the better solvent: water or carbon tetrachloride. Water, H20 Carbon tetrachloride, CCl4
For each Solute, Identity the better solvent water of carbon tetrachloride. Water, H20 Carbon tetrachloride, CCl4 CH20 NazS Brz CoH14
a. Calculate the mole fraction (x) of biphenyl (MW 154.21 g/mol) dissolved in naphthalene (MW = 128.17 g/mol) for a 0.250 m solution. Calculate the %mass biphenyl in the solution from part a.
A solution of NaCl (MW = 58.5 g/mol) in water (MW = 18.0 g/mol) has the molality of 3.01 molal and the density of 1.112 g/mL. Consider mass of solvent 1 Kg A) What is the mass percent of the solute? (B) What is the molarity of the solution? (C)What is the mole fraction of H2O?
How do you find the mass percent, mole fraction, and the molality for these two problems? P1. (Sec. 11.1) A solution is prepared by dissolving 113 grams of acetone (C3H6O) in 662 grams of water. With this information, calculate the solution's mass percent % of the solute, mole fraction of the solute, and the solutions molality. a) b) c) d) e) Mass Percent: 88.7%; Mole Fraction (Solute): 0.9068; & Molality: 5.70 mol/kg Mass Percent: 11.3%; Mole Fraction (Solute): 0.0932; &...