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3. A solution is prepared by dissolving 35.0 g of hemoglobin in enough water to make up 1.00 L in volume. The osmotic pressure of the solution is found to be 10.0 mmHg at 25.0 °C. Calculate the molar mass of hemoglobin.

3. A solution is prepared by dissolving 35.0 g of hemoglobin in enough water to make up 1.00 L in volume. The osmotic pressure of the solution is found to be 10.0 mmHg at 25.0 °C. Calculate the molar mass of hemoglobin.

Chemistry
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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Assume that all gases obey the Ideal Gas Law. Use separate paper. 1. A 20.0 L reactor is filled with air (20% oxygen, CO2 free), temperature recorded, 23.0°C. 1-Hexene (C6H12, 10.00 mL, d = 0.6685 g/mL, MW = 84.162 g/mol) was introduced and combusted. After the temperature equilibrated the total pressure in the reactor was 1.784 atm. Assume ideal gas behavior. a) If an excess oxygen was present in the reactor what was the pressure of the air prior to the introduction of the hydrocarbon? (hint: balance the equation) 2. A pond has an oxygen content of 2.401 × 10 mole/L. What is the atmospheric pressure that day if the temperature was 15°C and the humidity was 70%? Assume that the CO2 contribution is negligible. K for oxygen is 1.30 × 10° mol/L atm. 3. A solution is prepared by dissolving 35.0 g of hemoglobin in enough water to make up 1.00 L in volume. The osmotic pressure of the solution is found to be 10.0 mmHg at 25.0 °C. Calculate the molar mass of hemoglobin. 4. a) What is the osmotic pressure of an aqueous solution at 25°C if its freezing point is - 2.1°C? Assume that M and m are equivalent. K¢ for water is 1.86 °C/m b) What mass of fructose (180.16 g/mol) would you need to dissolve in 500 mL of water to achieve that effect? c) What mass of NaCl (58.44 g/mole) would you need to dissolve in 500 mL of water to achieve that effect?
Transcribed Image Text:Assume that all gases obey the Ideal Gas Law. Use separate paper. 1. A 20.0 L reactor is filled with air (20% oxygen, CO2 free), temperature recorded, 23.0°C. 1-Hexene (C6H12, 10.00 mL, d = 0.6685 g/mL, MW = 84.162 g/mol) was introduced and combusted. After the temperature equilibrated the total pressure in the reactor was 1.784 atm. Assume ideal gas behavior. a) If an excess oxygen was present in the reactor what was the pressure of the air prior to the introduction of the hydrocarbon? (hint: balance the equation) 2. A pond has an oxygen content of 2.401 × 10 mole/L. What is the atmospheric pressure that day if the temperature was 15°C and the humidity was 70%? Assume that the CO2 contribution is negligible. K for oxygen is 1.30 × 10° mol/L atm. 3. A solution is prepared by dissolving 35.0 g of hemoglobin in enough water to make up 1.00 L in volume. The osmotic pressure of the solution is found to be 10.0 mmHg at 25.0 °C. Calculate the molar mass of hemoglobin. 4. a) What is the osmotic pressure of an aqueous solution at 25°C if its freezing point is - 2.1°C? Assume that M and m are equivalent. K¢ for water is 1.86 °C/m b) What mass of fructose (180.16 g/mol) would you need to dissolve in 500 mL of water to achieve that effect? c) What mass of NaCl (58.44 g/mole) would you need to dissolve in 500 mL of water to achieve that effect?
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