<span>If we use 100 mL of
solution:
V(ethylene glycol - C</span>₂H₆O₂) = 0,52 · 100 mL = 52 mL.<span>
V(water) = 0,48 · 100 mL = 48 mL.
m(C</span>₂H₆O₂) = 52 mL · 1,115 g/mL = 57,98 g.<span>
n(C</span>₂H₆O₂) = 57,98 g ÷ 62,07 g/mol = 0,934 mol.<span>
m(H</span>₂O)
= 48 mL · 0,988 g/mL = 47,424 g.<span>
n(H</span>₂O)
= 45,45 g ÷ 18 g/mol = 2,635 mol.<span>
mole fraction of solvent: 2,635 mol / (2,635 mol
+ 0,934 mol) =0,73.
Raoult's Law: p(solution) = mole fraction of
solvent · p(solvent).
<span>p(solution) = 0,73 · 92 torr = 67,33 torr.</span></span>
The molality of a solute is equal to the moles of solute per kg of solvent. We are given the mole fraction of I₂ in CH₂Cl₂ is <em>X</em> = 0.115. If we can an arbitrary sample of 1 mole of solution, we will have:
0.115 mol I₂
1 - 0.115 = 0.885 mol CH₂Cl₂
We need moles of solute, which we have, and must convert our moles of solvent to kg:
0.885 mol x 84.93 g/mol = 75.2 g CH₂Cl₂ x 1 kg/1000g = 0.0752 kg CH₂Cl₂
We can now calculate the molality:
m = 0.115 mol I₂/0.0752 kg CH₂Cl₂
m = 1.53 mol I₂/kg CH₂Cl₂
The molality of the iodine solution is 1.53.
<h3>
Answer:</h3>
0.699 mole CaCl₂
<h3>
Explanation:</h3>
To get the number of moles we use the Avogadro's number.
Avogadro's number is 6.022 x 10^23.
But, 1 mole of a compound contains 6.022 x 10^23 molecules
In this case;
we are given 4.21 × 10^23 molecules of CaCl₂
Therefore, to get the number of moles
Moles = Number of molecules ÷ Avogadro's constant
= 4.21 × 10^23 molecules ÷ 6.022 x 10^23 molecules/mole
= 0.699 mole CaCl₂
Hence, the number of moles is 0.699 mole of CaCl₂
Answer:
I’m pretty sure it’s Lions sleeping after a big meal
Explanation:
Answer:
It sounds like they are studying French phonemes
Explanations:
I just learned this.
