ZuoTi.Pro
Question

What mass of glucose (C H120) in kilograms (kg) should be dissolved in 15.9 kg of water to obtain a solution with a freezing
science   chemistry   
0 0
Add a comment Improve this question Transcribed image text
Next > < Previous
Sort answers by oldest

Homework Answers

Answer #1

use:

Δ Tf = Kf*mb

4.59 = 1.86 *mb

mb= 2.4677 molal

m(solvent)= 15.9 Kg

use:

number of mol,

n = Molality * mass of solvent in Kg

= (2.468 mol/Kg)*(15.9 Kg)

= 39.24 mol

Molar mass of C6H12O6,

MM = 6*MM(C) + 12*MM(H) + 6*MM(O)

= 6*12.01 + 12*1.008 + 6*16.0

= 180.156 g/mol

use:

mass of C6H12O6,

m = number of mol * molar mass

= 39.24 mol * 1.802*10^2 g/mol

= 7.069*10^3 g

Answer: 7.07*10^3 g

0 0
Add a comment
Know the answer?
Add Answer to:
What mass of glucose (C H120) in kilograms (kg) should be dissolved in 15.9 kg of water to obtain a solution with a...
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for? Ask your own homework help question. Our experts will answer your question WITHIN MINUTES for Free.
Similar Homework Help Questions

  • A solution of water (Kf=1.86 ∘C/m) and glucose freezes at − 2.35 ∘C. What is the...

    A solution of water (Kf=1.86 ∘C/m) and glucose freezes at − 2.35 ∘C. What is the molal concentration of glucose in this solution? Assume that the freezing point of pure water is 0.00 ∘C. Express your answer to three significant figures and include the appropriate units. View Available Hint(s) m m m = nothing nothing Submit Boiling points and molality Similar to the freezing-point depression, the boiling-point elevation ΔTb of a solution is quantitatively related to the molality m and...

  • Part B A solution of water (kr = 1.86°C/m) and glucose freezes at - 415°C What...

    Part B A solution of water (kr = 1.86°C/m) and glucose freezes at - 415°C What is the molal concentration of glucose in this solution? Assume that the freezing point of pure water is 0.00 °C Express your answer to three significant figures and include the appropriate units. View Available Hint(s) m= 2.34 m Submit Previous Answers X Incorrect: Try Again: 5 attempts remaining Part A solution of water (K = 0.512 °C/m) and glucose boils at 101.56 °C. What...

  • מו Calculate the mass of glucose (C6H606) that must be added to 100 g of water...

    מו Calculate the mass of glucose (C6H606) that must be added to 100 g of water to give a solution whose freezing point is -3.8°C. The freezing point depression constant of water is 1.86 °C/m. The molar mass of glucose is 180.16 g/mol Give your answer in grams to 3 significant figures

  • What is the freezing point and boiling point in Celsius of a solution 400 g of...

    What is the freezing point and boiling point in Celsius of a solution 400 g of ethylene glycol (MW=62 g/mol) dissolved in 500 g of water? The molal freezing point depression constant for water is 1.86 C/m The molal boiling point elevation constant of water is 0.512 C/m Please explain steps

  • A solution of ethylene glycol in water at 20 degrees celsius has a mass percent of...

    A solution of ethylene glycol in water at 20 degrees celsius has a mass percent of 9.78% of ethylene glycol with a density of 1.0108 g/mL. The freezing point depression constant for water (solvent for all solutions) is Kf=-1.86 percent celsius kg/mol and the boiling point elevation constant is Kb=0.512 degrees celsius kg/mol. The density of neat water at 20.0 degrees celsius is 0.9982 g/mL. Answer the following: 1. What is the molarity of the solution? 2. What is the...

  • A Review Constants Periodic Table The changes in boiling point (AT) or freezing point (AT) in...

    A Review Constants Periodic Table The changes in boiling point (AT) or freezing point (AT) in degrees Celsius from a pure solvent can be determined from the equations given here, respectively: AT) = m x K = moles of solute XK K. kilograms of solvent Since pure water boils at 100.00 °C, and since the addition of solute increases boiling point, the boiling point of an aqueous solution, Th, will be T - (100.00+AT) 'C Since pure water freezes at...

  • A certain substance X has a normal freezing point of 6.8 C and a molal freezing...

    A certain substance X has a normal freezing point of 6.8 C and a molal freezing point depression constant Kf=7.51C kg x mol-1 . A solution is prepared by dissolving some urea ((NH2)2CO) in 600 of X. This solution freezes at 5.0 C . Calculate the mass of urea that was dissolved. Be sure your answer has the correct number of significant digits.

  • 1.0345 g of palmitic acid dissolved in 8.7545 g of stearic acid. Calculate the freezing point...

    1.0345 g of palmitic acid dissolved in 8.7545 g of stearic acid. Calculate the freezing point of the solution. The molar mass of palmitic acid is 256.48 g/ mol. The molal freezing point constant , Kf for stearic acid is 4.5 degrees C/ m and pure stearic acid freezes at 69.3 degrees Celsius.

  • What is the freezing point (°C) of a solution prepared by dissolving 11.3 g of in 115 g of water? [Use these Molar Mass...

    What is the freezing point (°C) of a solution prepared by dissolving 11.3 g of in 115 g of water? [Use these Molar Masses: Ca = 40, N = 14, O = 16. Also, the molal freezing point depression constant for water is 1.86 °C/m.]

  • When 0.60 grams of a non-electrolyte unknown compound is dissolved in 10 grams of water, the...

    When 0.60 grams of a non-electrolyte unknown compound is dissolved in 10 grams of water, the freezing point of the solution is -1.86o C. Given that the freezing point of pure water is 0o C and that the freezing-point depression constant for water is 1.86 o C/mol/kg, calculate the molecular mass (g/mol) of the unknown compound.

ADVERTISEMENT
Free Homework Help App
Download From Google Play
Scan Your Homework
to Get Instant Free Answers
Need Online Homework Help?
Ask a Question
Get Answers For Free
Most questions answered within 3 hours.
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT