A bioreactor with a capacity of 25 liters contains initially 0.01 cubic meters of a 50 mM glucose solution (MW = 180 g/mol). a) What is the final concentration of glucose (expressed in mM) if an additional 12 liters of 30 mM glucose solution is pumped into the bioreactor? b) Instead of (a), if 12 liters of plain water are added to the bioreactor, what is the final concentration of gluCose (expressed in mM)? c) Instead of (a) or (b), if an additional 5 liters of 15 mM glucose solution plus 1O liters of water are added, what is the final concentration of glucose: i. Expressed as molarity? ii. Expressed as % w/v? (% w/v means grams per 100 mL of solution, you result will be expressed as % w/v, example 5.3 % w/v) iii. Expressed as g/cm?? Expressed as ppm? (ppm means parts per million, that is, g per 10° g of solution- see Section 2.4.5 in your book) You can assume that the density of the solution (glucose + water) is the same as the density of water - this iv. assumption is appropriate since this is a dilute solution. Assume density of water to be 1 g/cm?.

A bioreactor with a capacity of 25 liters contains initially 0.01 cubic meters of a 50 mM glucose solution (MW = 180 g/mol). a) What is the final concentration of glucose (expressed in mM) if an additional 12 liters of 30 mM glucose solution is pumped into the bioreactor? b) Instead of (a), if 12 liters of plain water are added to the bioreactor, what is the final concentration of gluCose (expressed in mM)? c) Instead of (a) or (b), if an additional 5 liters of 15 mM glucose solution plus 1O liters of water are added, what is the final concentration of glucose: i. Expressed as molarity? ii. Expressed as % w/v? (% w/v means grams per 100 mL of solution, you result will be expressed as % w/v, example 5.3 % w/v) iii. Expressed as g/cm?? Expressed as ppm? (ppm means parts per million, that is, g per 10° g of solution- see Section 2.4.5 in your book) You can assume that the density of the solution (glucose + water) is the same as the density of water - this iv. assumption is appropriate since this is a dilute solution. Assume density of water to be 1 g/cm?.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Rubbing alcohol, C3H7OH) is sold as a 70.0% v/v solution for external use only. What volume of pure C3H7OH, is present in a 500.0 mL bottle?
Human blood cell is 0.135M in NaCl and 0.005M in KCl. If a drop of blood is placed in an aqueous solution with a molarity of 0.135M CsCl. What will happen to the blood cells in the drop?
You place 0.03531g of CaCl₂ into a 500.0 mL volumetric flask and dissolve the solid with water to the mark on the flask. You then dilute 2.75 mL of this solution to 50.0 mL in a volumetric flask. What is the concentration of Ca in ppm in the resulting solution? [You can assume a density of 1.000 g/mL for the solution]
6.02 x 10^20 molecules of urea are present in 100 mL of its solution. The concentration of solution is: ( O 0.001 M 0.02 M O 0.01 M O 0.1 M
When 100.0 g of an unknown compunf was dissolved in 1.00 kg of water, the boiling point was raised by 3.62 C. What is the molar mass of this unknown compound? (Kb for water is 0.51 C/m)
A 300 mL solution containing 1.85 g CaCl2 is mixed with a 500 mL solution containing 1.95 g NaCl. What is the final ppm concentration of Na+, Ca2+ and Cl-?
what is the concentration ofglucose c6h12o6MM=180.16g/mol solution that was prepared by dissolving 50.500g of glucose in 500.0ml of solution?assume the solution has a density of 1.00g/ml %mm M
A chemist prepared an aquenous solution using solid Magnesium hydroxide Mg(OH)2 and water at 25.0 C. Answer the following questions. The density of this solution was measured to be 1.10 g/mL. (useful information, kf= 1.86 C/m, kb=0.512 C/m) a. Calculate the mass of water and the mass of Mg(OH)2 in grams require to make a 180. g of 0.140 m Mg(OH)2 solution.
A copper(II) sulfate solution is 14.0% CuSO4 by mass. It is simultaneously 1.01 M at 20 °C. (a) Compute the density of this solution. Density= 8 cm-3 (b) What volume of this solution should be used in preparing 1.44 L of a 9.60×10-² M copper(II) sulfate solution? Volume mL