A 0.158 g sample of an unknown enzyme is dissolved in water to make 0.134 L of solution. The osmotic pressure of the solution at 25 °C is found to be 0.718 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, where R = 0.08314 L-bar-K-l. mol-. 1 = R-T-M What is the molarity of the solution?
A 0.158 g sample of an unknown enzyme is dissolved in water to make 0.134 L of solution. The osmotic pressure of the solution at 25 °C is found to be 0.718 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, where R = 0.08314 L-bar-K-l. mol-. 1 = R-T-M What is the molarity of the solution?
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter13: The Chemistry Of Solutes And Solutions
Section: Chapter Questions
Problem 41QRT: A sample of water contains 0.010 ppm lead ions, Pb2+. (a) Calculate the mass of lead ions per liter...
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Transcribed Image Text:A 0.158 g sample of an unknown enzyme is dissolved in water to make 0.134 L of solution. The osmotic pressure of the
solution at 25 °C is found to be 0.718 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, where R = 0.08314 L-bar-K-l. mol-.
1 = R:T·M
What is the molarity of the solution?
.126
M =
mol·L-
Incorrect
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