Osmotic pressure is the pressure that would have to be applied to a pure solvent to prevent it from passing into a given solution by osmosis.
That can be mathematical computed from the expression:
Osmotic pressure=C×R×T
Where,
C= Concentration
R=Gas constant
T=Temperature
Concentration=Number of moles of solute/Volume(L)
=0.005*1000/100
=0.05
R= 0.08206 atm L/mol K
T=25+273
=298
Osmotic pressure= 0.05×0.08206×298
=1.2 atm
Number 9 adding oil lubricates the chain making it easier to pedal. Also the oil prevents rusting
Answer:
All of the statements above are true.
Explanation:
Ice is solid water. Ice consists of an array of water molecules arranged into a crystal lattice. Ice has spaces between the water molecules so it is less dense than liquid water. Ice is about 9% less dense than liquid water. This accounts for the fact that it floats on water.
Ice contains more hydrogen bonds per water molecule when compared to liquid water.
Answer:
- In general, polar solutes are most soluble in highly polar solvents.
Explanation:
The general rule is "like dissolves like" which means that <em>polar solvents </em>dissolve polar (or ionic) <em>solutes</em> and <em>non-polar solvents</em> dissolve non-polar solutes.
In order for a solvent dissolve a solute, the strength of the interacttion (force) between the solute and the solvent units (atoms, molecules, or ions) must be stronger than the strength of the forces that keep together he particles of the pure substances (known as intermolecular forces).
Since the nature of the interactions between the units are electrostatic, the more polar is the solvent the better it will be able to attract and surround the solute particles, keeping them separated and in solution. That mechanism explains why polar solutes will be most soluble in highly polar solvents.
I believe that the balanced chemical reaction is:
C6H12O6 + 6 O2 → 6 CO2
+ 6 H2O
So the number of grams
of oxygen required is:
mass O2 required = 48
g C6H12O6 * (1 mole C6H12O6 / 180.16 g) * (6 mole O2 / 1 mole C6H12O6) * (32
grams O2 / 1 mole)
<span>mass O2 required =
51.15 grams</span>
