The osmotic pressure of blood is 5950.8 mmHg at 41ºC. What mass of glucose, C 6 H 12 O 6 , is needed to prepare 5.51 L of solution. The osmotic pressure of the glucose solution is equal to the osmotic pressure of blood.

We're told the osmotic pressure of blood is 5,950.8 millimeters of mercury at 41 degrees Celsius. What mass of glucose, which is c 6h1206, is needed to prepare 5.51 liters of solution? The osmotic pressure of the glucose solution is equal to the osmotic pressure of blood. Alright. So osmotic pressure equals I times molarity times r times t. What we need to realize is osmotic pressure is going to be in atmospheres, so what I'm gonna do first is I'm gonna convert the millimeters of mercury into atmospheres. So one atmosphere is 760 millimeters of mercury. So when we do that we get 7.83 atmospheres here as our osmotic pressure. And that's gonna equal 1 because our solid of glucose is covalent. Covalent things don't break up into ions. Here, we don't know the moles of glucose, that's what we need to find, divided by liters of solution, which is given to us. R is our gas constant, and t is our temperature in Kelvin. So I'm gonna add 273.15 to this number here and that'll give me my Kelvin. So that's 314.15 Kelvin. All we have to do now is solve for x. So I'm gonna multiply r times this temperature. So when I do that I'm going to get 7.83 equals 25.779149 times x divided by 5.51. Again, where did I get this 25 in change? Came from multiplying r times the temperature. Now cross multiply 7.83 times 5.51, when I do that I'm gonna get 43.14 33 and that still equals 25.779149x, divide both sides now by 43.1433 actually, not by that, by 25 0.779149, and that'll give me my x. So we're gonna work it over here. So here your x equals 1 point 67357 moles of glucose. Because remember our x that we're solving for was our moles of glucose. If I know the moles, then I can figure out the the mass. We just say 1 mole of glucose and its molecular weight or molar mass is 180.156 grams. That's the weight of the 6 carbons, 12 hydrogens, and 6 oxygens. So that gives me as my total at the end, 302 grams of glucose. So that would be my final answer.

The osmotic pressure of blood is 5950.8 mmHg at 41ºC. What mass o...

1. Matter and Measurements4h 29m

2. Atoms and the Periodic Table5h 23m

3. Ionic Compounds2h 18m

4. Molecular Compounds2h 18m

5. Classification & Balancing of Chemical Reactions3h 17m

6. Chemical Reactions & Quantities2h 35m

7. Energy, Rate and Equilibrium3h 46m

8. Gases, Liquids and Solids3h 25m

9. Solutions4h 10m

10. Acids and Bases3h 29m

11. Nuclear Chemistry56m

BONUS: Lab Techniques and Procedures1h 38m

BONUS: Mathematical Operations and Functions47m

12. Introduction to Organic Chemistry1h 34m

13. Alkenes, Alkynes, and Aromatic Compounds2h 12m

14. Compounds with Oxygen or Sulfur1h 6m

15. Aldehydes and Ketones1h 1m

16. Carboxylic Acids and Their Derivatives1h 11m

17. Amines38m

18. Amino Acids and Proteins1h 51m

19. Enzymes1h 37m

20. Carbohydrates1h 46m

21. The Generation of Biochemical Energy2h 8m

22. Carbohydrate Metabolism2h 22m

23. Lipids2h 26m

24. Lipid Metabolism1h 45m

25. Protein and Amino Acid Metabolism1h 37m

26. Nucleic Acids and Protein Synthesis2h 54m

The osmotic pressure of blood is 5950.8 mmHg at 41ºC. What mass of glucose, C₆H₁₂O₆, is needed to prepare 5.51 L of solution. The osmotic pressure of the glucose solution is equal to the osmotic pressure of blood.

Watch next

The osmotic pressure of blood is 5950.8 mmHg at 41ºC. What mass of glucose, C6H12O6, is needed to prepare 5.51 L of solution. The osmotic pressure of the glucose solution is equal to the osmotic pressure of blood.

Watch next

Osmotic Pressure practice set

The osmotic pressure of blood is 5950.8 mmHg at 41ºC. What mass of glucose, C₆H₁₂O₆, is needed to prepare 5.51 L of solution. The osmotic pressure of the glucose solution is equal to the osmotic pressure of blood.