A 0.358 g sample of an unknown enzyme is dissolved in water to make 0.142 L of solution. The osmotic pressure of thesolution at 25 'C is found to be 0.740 mbar. Calculate the molecular mass of the enzyme.STRATEGY1. Determine the molarity of the enzyme solution.2. Determine the moles of enzyme.3. Calculate the molecular mass of the enzyme.You can determine the molarity of the solution based on the osmotic pressure.* = R T M (where R = 0.08314 L bar K-. mol-)1 bar(0.740 mbar)1000 mbarM =RT= 2.99 x 10-$ mol · L-!(0.08314 L bar K- · mol-) (298 K)How many moles of enzyme are in 0.142 L of a 2.99 × 10-$ M solution?moles of enzyme:Question Source: MRG-General ChemistryMacBook AirF6F7F8F9F10&785%24

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How many moles of enzyme are in 0.142 L of a 2.99 × 10-5 M solution?

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...

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Question

A 0.358 g sample of an unknown enzyme is dissolved in water to make 0.142 L of solution. The osmotic pressure of the
solution at 25 'C is found to be 0.740 mbar. Calculate the molecular mass of the enzyme.
STRATEGY
1. Determine the molarity of the enzyme solution.
2. Determine the moles of enzyme.
3. Calculate the molecular mass of the enzyme.
You can determine the molarity of the solution based on the osmotic pressure.
* = R T M (where R = 0.08314 L bar K-. mol-)
1 bar
(0.740 mbar)
1000 mbar
M =
RT
= 2.99 x 10-$ mol · L-!
(0.08314 L bar K- · mol-) (298 K)
How many moles of enzyme are in 0.142 L of a 2.99 × 10-$ M solution?
moles of enzyme:
Question Source: MRG-General Chemistry
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