Question

Toluene (C7H8, molar mass = 92.13 g/mol) an organic compound often used as a solvent in...

Toluene (C7H8, molar mass = 92.13 g/mol) an organic compound often used as a solvent in paints is mixed with a similar organic compound benzene (C6H6, molar mass 78.11 g/mol). Calculate the molarity, molality, mass percent, and mole fraction of toluene in 2.00 x 103 mL of solution that contains 75.8 g of toluene and 95.6 g of benzene. The density of solution is 0.857 g/cm3.

Homework Answers

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
what are the partial and total vapor pressures of a solution obtained by mixing 35.8 g...
what are the partial and total vapor pressures of a solution obtained by mixing 35.8 g of benzene C6H6 and 56.7 g of toluene C7H8 at 25C? at 25C the vapor pressure of c6h6 = 95.1 mmHg and the vapor pressure of C7H8= 28.4 mmHg molar masses are c6h6= 78.11 g/mol and c7h8 = 92.13
100.0 g of benzene is mixed with 100.0 g of toluene to form a solution that...
100.0 g of benzene is mixed with 100.0 g of toluene to form a solution that can be considered ideal. What is the total vapor pressure (in Torr) of this solution at 293 K? The molar masses of benzene and toluene are 78.11 g/mol and 92.14 g/mol respectively. At 293 K the vapor pressures of pure benzene and pure toluene are 74.7 Torr and 22.3 Torr respectively. Report your result with 1 decimal place.
When 8.05 g of an unknown compound X was dissolved in 100 g of benzene C6H6,...
When 8.05 g of an unknown compound X was dissolved in 100 g of benzene C6H6, the vapor pressure of the benzene decreased from 100 torr to 94.8 torr at 26 degrees C. (MW C6H6 =78.0 g/mol.) a.) What is the mole fraction for unknown compound X? b.) What is the molar mass of unkown compound X?
An organic compound has a molar mass of 168.2 g/mol and contains 8.32% hydrogen atoms by...
An organic compound has a molar mass of 168.2 g/mol and contains 8.32% hydrogen atoms by mass. How many hydrogen atoms are in each molecule of this compund?
A solution contains 65.0 g of solvent. How much solute is present in the solution if...
A solution contains 65.0 g of solvent. How much solute is present in the solution if the mole fraction of the solute is 0.135? (molar mass of solvent=18g/mol; molar mass of solute 30g/mol)
1. An aqueous solution of sulfuric acid (6M H2SO4 in water) is flowing into a tank...
1. An aqueous solution of sulfuric acid (6M H2SO4 in water) is flowing into a tank at the rate of 100 liters/min (also can be written 100 L/min) having a density of 1.34 g/cm3. Calculate value of the items requested below and make sure you show HOW you obtained them. For parts (b) - (d), first write out the equation using symbols for the appropriate variables, and then algebraically solve for the unknown variables, and finally substitute in the numerical...
At a particular temperature, the partial molar volume of liquid A (MM = 69.5 g mol-1)...
At a particular temperature, the partial molar volume of liquid A (MM = 69.5 g mol-1) is 55.1 cm3 mol-1 and that of liquid B (MM = 127.2 g mol-1) is 87.1 cm3 mol-1. Given that the mole fraction of liquid A is 0.37, find the mass in kg of 23.8 L of the solution.
The sulfuric acid (98 g/mol) in a car battery has a density of 1.225 g/cm3 and...
The sulfuric acid (98 g/mol) in a car battery has a density of 1.225 g/cm3 and is 3.75 M. What is the molality, mole fraction and percentage of sulfuric acid by mass in this solution?
7. A compound has the empirical formula CH and a molar mass of 78.11 g/mol. What...
7. A compound has the empirical formula CH and a molar mass of 78.11 g/mol. What is its molecular formula? 8. Upon combustion, a compound containing only carbon and hydrogen produces 1.83 g CO2 and 0.901 g H2O. Find the empirical formula of the compound. 9. Write a balanced equation for the reaction between solid cobalt(III) oxide and solid carbon to produce solid cobalt and carbon dioxide gas.
Determine the molar mass of the solute. If 2.35 g of the unknown compound were dissolved...
Determine the molar mass of the solute. If 2.35 g of the unknown compound were dissolved in 30.46 g of PDB ( Kfp for PDB = 7.10 C/m) m=molality = moles solute/kg solvent Molar mass= grams of substance/mole of substance 1. Molar mass of solute is___________ On this molar mass calculation in a freezing point depression experiment determine the effect on molar mass, will it be higher, lower, or not change. 2. The thermometer you were using read temperatures consistently...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT