Explanation:
5.00 mol H2O × (1 mol C6H12O6/6 mol H2O)
= 0.833 mol C6H12O6
5.00 mol H2O × (6 mol O2/6 mol H2O)
= 5.00 mol O2
Answer:
Molality = 8.57 m
Explanation:
Given data:
Molarity of solution = 5.73 M
density = 0.9327 g/mL
Molality of solution = ?
Solution:
Molality = moles of solute / kg of solvent.
Kg of solvent:
Mass of 1 L solution = density× volume
Mass of 1 L solution = 0.9327 g/mL × 1000 mL
Mass of 1 L solution = 932.7 g
Mass of solute:
Mass of 1 L = number of moles × molar mass
Mass = 5.73 mol × 46.068 g/mol
Mass = 263.97 g
Mass of solvent:
Mass of solvent = mass of solution - mass of solute
Mass of solvent = 932.7 g - 263.97 g
Mass of solvent = 668.73 g
In Kg = 668.73 /1000 = 0.6687 Kg
Molality:
Molality = number of moles of solute / mass of solvent in Kg
Molality = 5.73 mol / 0.6687 Kg
Molality = 8.57 m
Answer:
The answer to your question is 0.54M
Explanation:
Data
Final concentration = ?
Concentration 1 = 0.850 M
Volume 1 = 249 ml = 0.249 l
Concentration 2 = 0.420 M
Volume 2 = 0.667 M
Process
1.- Calculate the number of moles in both solutions
Number of moles 1 = Molarity 1 x Volume 1
= 0.850 x 0.249
= 0.212
Number of moles 2 = Molarity 2 x Volume 2
= 0.420 x 0.667
= 0.280
Total number of moles = 0.212 + 0.280
= 0.492
2.-Calculate the final volume
Final volume = Volume 1 + Volume 2
Final volume = 0.249 + 0.667
= 0.916 l
3.- Calculate Molarity
Molarity = 0.492 / 0.916
Molarity = 0.54
