Answer:
E. (None of these).
It is 0.333 M.
Explanation:
A molar solution would contain 183 g in 1 liter.
By proportion, this solution contains 18.3 * 1000/300
= 61 g per liter.
So it is 61 / 183 = 0.333 M.
Answer:
V O2 = 1.623 L
Explanation:
- 1 mol ≡ 6.022 E23 molecules
∴ molecules O2 = 4.00 E22 molecules
⇒ moles O2 = (4.00 E22 molecules O2)×(mol O2/6.022 E23 molecules)
⇒ moles O2 = 0.0664 moles
at STP:
∴ T = 25°C ≅ 298 K
∴ P = 1 atm
assuming ideal gas:
∴ V = RTn/P
⇒ V O2 = ((0.082 atm.L/K.mol)(298 K)(0.0664 mol))/( 1 atm)
⇒ V O2 = 1.623 L
Answer:
<u>Optical purity = 76.9231 %</u>
<u>Specific rotation of mixture = - 97.6923 °</u>
Explanation:
The mass of the racemic mixture = 3 g
It means it contains R enantiomer = 1.5 g
S enantiomer = 1.5 g
Amount of Pure R = 10 g
Total R = 11.5 g
Total volume = 500 mL + 500 mL = 1000 mL = 1 L
[R] = 11.5 g/L
[S] = 1.5 g/L
Enantiomeric excess = 
= 
= 76.9231 %
<u>Optical purity = 76.9231 %</u>
Also,
Optical purity = 
Optical rotation of pure enantiomer = −127 °
<u>Specific rotation of mixture = - 97.6923 °</u>
The physical explanation is that increasing temperature increases the kinetic energy of the gas molecules. Hence, their random motion breaks more intermolecular bonds and the gas is less dissolved in the solvent. In contrast, solid solutes in water have increased solubility with increased temperatures.
Answer: A & D
Explanation:
The two main forces are temperature and salinity.
