Question

A solution is prepared by mixing 25 mL pentane (C5H12, d = 0.63 g/cm3) with 30...

A solution is prepared by mixing 25 mL pentane (C5H12, d = 0.63 g/cm3) with 30 mL hexane (C6H14, d = 0.66 g/cm3). Assuming that the volumes add on mixing, calculate the mass percent, mole fraction, molality, and molarity of the pentane.

Homework Answers

Answer #1

we know that

1 cm3 = 1 ml

also

mass = density x volume

so

mass of pentane = 25 x 0.63 = 15.75 g

mass of hexane = 30 x 0.66 = 19.8 g

now

total mass = 15.75 + 19.8

total mass = 35.55

now

% mass = mass of pentane x 100 / total mass

% mass = 15.75 x 100 / 35.55

% mass = 44.3

so

the mass percent of pentane is 44.3 %

now

moles = mass / molar mass

so

moles of pentane = 15.75 / 72 = 0.21875

moles of hexane = 19.8 / 86 = 0.23023

now

total moles = 0.21875 + 0.23023 = 0.44898

now

mol fraction of pentane = moles of pentane / total moles

mol fraction of pentane = 0.21875 / 0.44898

mol fraction of pentane = 0.487


now

molality = moles of pentane x 1000 / mass of hexane (g)

molality = 0.21875 x 1000 / 19.8

molallity of pentane = 11.048

now

total volume = 25 + 30 = 55 ml

now

molarity = moles of pentane x 1000 / volume of sollution (ml)

molarity = 0.21875 x 1000 / 55

molarity of pentane = 3.98

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
A solution is prepared by dissolving 20.2 mL of methanol (CH3OH) in 100.0 mL of water...
A solution is prepared by dissolving 20.2 mL of methanol (CH3OH) in 100.0 mL of water at 25 ∘C. The final volume of the solution is 118 mL. The densities of methanol and water at this temperature are 0.782 g/mL and 1.00 g/mL, respectively. For this solution, calculate each of the following. A. Molarity B. Molality C. Percent by Mass D. Mole fraction
A solution was prepared by dissolving 26.0 g of KCl in 225 g of water. The...
A solution was prepared by dissolving 26.0 g of KCl in 225 g of water. The composition of a solution can be expressed in several different ways. Four of the most common concentration units are defined as follows:. mass %=mass of componenttotal mass of solution×100%; mole fraction (X)=moles of componenttotal moles of solution; molarity (M)=moles of soluteliters of solution; molality (m)=moles of solutemass of solvent (kg) Part A Calculate the mass percent of KCl in the solution. Part B Calculate...
A) A solution is prepared by dissolving 50.4 g sucrose (C12H22O11) in 0.332 kg of water....
A) A solution is prepared by dissolving 50.4 g sucrose (C12H22O11) in 0.332 kg of water. The final volume of the solution is 355 mL. For this solution, calculate the molarity. Express the molarity in units of moles per liter to three significant figures. B) Calculate the molality. Express the molality in units of moles per kilogram of solvent to three significant figures. C) Calculate the percent by mass.Express the percent by mass to three significant figures. D) Calculate the...
Calculate the molarity, molality, and mole fraction of a solution created by mixing 500.0 mL of...
Calculate the molarity, molality, and mole fraction of a solution created by mixing 500.0 mL of ethanol (C2H6O / d = 0.789 g/mL) with 4.267 g of benzene (C6H6 / d = 0.876 g/mL). Assume the density of the solution is the same as ethanol.
A solution is prepared by dissolving 25.00 g of acetic acid (CH3COOH) in 750.0 g of...
A solution is prepared by dissolving 25.00 g of acetic acid (CH3COOH) in 750.0 g of water. The density of the resulting solution is 1.105 g/mL. A) Calculate the mass percent of acetic acid in the solution. B) Calculate the molarity of the solution. C) Calculate the molality of the solution. D) Calculate the mole fraction of acetic acid in the solution. E) What is the concentration of acetic acid in ppm?
A sodium hydroxide solution is made by mixing 13.64 g NaOH with 100 g of water....
A sodium hydroxide solution is made by mixing 13.64 g NaOH with 100 g of water. The resulting solution has a density of 1.131 g/mL. a. What is the molarity of this solution? b. What is the molality of the solution? c. What is the mass fraction of NaOH in the solution? d. What is the mole fraction of NaOH in the solution?
A solution is prepared by dissolving 20.2 mL of methanol in 100.0 mL of water. The...
A solution is prepared by dissolving 20.2 mL of methanol in 100.0 mL of water. The final volume of this solution is 118ml. The densities of methanol and water are 0.782 g/mL and 1.00 g/mL, respectively. For this solution, calculate the following- molarity molality mass % MOLE FRACTION VOLUME OF SOLVENT MASS OF SOLVENT MOLES OF SOLVENT VOLUME OF SOLUTE MOLES OF SOLUTE MASS OF SOLUTE VOLUME OF SOLUTION MASS OF SOLUTION
An automobile antifreeze mixture is made by mixing equal volumes of ethylene glycol (d = 1.114...
An automobile antifreeze mixture is made by mixing equal volumes of ethylene glycol (d = 1.114 g/mL; M = 62.07 g/mol) and water (d = 1.00 g/mL) at 20°C. The density of the mixture is 1.070 g/mL. Express the concentration of ethylene glycol as (a) volume percent % v/v (b) mass percent % w/w (c) molarity M (d) molality m (e) mole fraction
7) If a solution is prepared by mixing 15.7 mL of CH3CH2OH (d = 0.792 g/mL)...
7) If a solution is prepared by mixing 15.7 mL of CH3CH2OH (d = 0.792 g/mL) and 457 mL of CH3CH2CH2OH (d = 0.911 g/mL) what is the concentration in molality m? Show work A) 0.648 m B) 0.812 m C) 1.57 m D) 2.01 m E) 4.98 m
A solution is prepared by dissolving 61.5 mL of methanol in 115.0 mL of water at...
A solution is prepared by dissolving 61.5 mL of methanol in 115.0 mL of water at 25 ∘C . The final volume of the solution is 173.4 mL . The densities of methanol and water at this temperature are 0.782 g/mL and 1.00 g/mL , respectively. For this solution, calculate each of the following. [Molarity, molality, mass percent]
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT