Question

What mass of sucrose (C12H22O11) would you combine with 5.00 * 102 g of water to make a solution with an osmotic pressure of 8.55 atm at 298 K? (Assume a density of 1.0 g>mL for the solution.)

Name: what mass of sucrose c12h22o11 would you combine with 500 102 g of water to make a solution with an osmotic pressure of 855 atm at 298 k assume a density of 10 gml for the solution 2
Uploaded: 2019-03-23T21:58:00-08:00
Duration: 1 min 29 s
Channel: George Mckeown
Description: what mass of sucrose c12h22o11 would you combine with 500 102 g of water to make a solution with an osmotic pressure of 855 atm at 298 k assume a density of 10 gml for the solution 2

          What mass of sucrose (C12H22O11) would you combine with
5.00 * 102 g of water to make a solution with an osmotic
pressure of 8.55 atm at 298 K? (Assume a density of 1.0 g>mL for
the solution.)

Added by Dorothy M.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Chapter 13

Instant Answer

Solved by Expert George Mckeown

03/23/2019

Step 1

55 \text{ atm} \] \[ i = 1 \text{ (since sucrose does not ionize)} \] \[ M = \text{ molar mass of sucrose} = 342.3 \text{ g/mol} \] \[ R = 0.08206 \text{ L atm/mol K} \] \[ T = 298 \text{ K} \] \[ 8.55 = 1 \times M \times 0.08206 \times 298 \] \[ M = Show more…

Show all steps

Thanks for your feedback!

What mass of sucrose (C12H22O11) would you combine with 5.00 * 102 g of water to make a solution with an osmotic pressure of 8.55 atm at 298 K? (Assume a density of 1.0 g>mL for the solution.)