Respuesta:
0.11 L
Explicación:
Paso 1: Escribir la ecuación balanceada
2 LiOH + H₂SO₃ ⇒ Li₂SO₃ + H₂O
Paso 2: Calcular la masa de solución de H₂SO₃
25 mL de solución de H₂SO₃ tiene una denisdad de 1.03 g/mL.
25 mL × 1.03 g/mL = 28 g
Paso 3: Calcular la masa de H₂SO₃ en 26 g de Solución de H₂SO₃
La riqueza de H₂SO₃ es 60%, es decir, cada 100 g de solución hay 60 g de H₂SO₃.
26 g Sol × 60 g H₂SO₃/100 g Sol = 16 g H₂SO₃
Paso 4: Calcular los moles correspondientes a 16 g de H₂SO₃
La masa molar de H₂SO₃ es 82.07 g/mol.
16 g × 1 mol/82.07 g = 0.19 mol
Paso 5: Calcular los moles de LiOH que reaccionan con 0.19 moles de H₂SO₃
La relación molar de LiOH a H₂SO₃ es 2:1. Los moles de LiOH que reaccionan son 2/1 × 0.19 mol = 0.38 mol.
Paso 6: Calcular el volumen de solución de LiOH
0.38 moles de LiOH están en una solución 3.5 M. El volumen requerido es:
0.38 mol × 1 L/3.5 mol = 0.11 L
Answer:
a): not necessarily due to London Dispersion Forces and dipole-dipole interactions.
b): not necessarily due to London Dispersion Forces.
Explanation:
There are three major types of intermolecular interaction:
- Hydrogen bonding between molecules with H-O, H-N, or H-F bonds and molecules with lone pairs.
- Dipole-dipole interactions between all molecules.
- London dispersion forces between all molecules.
The melting point of a substance is a result of all three forces, combined.
Note that the more electrons in each molecule, the stronger the London Dispersion Force. Generally, that means the more atoms in each molecule, the stronger the London dispersion force. The strength of London dispersion force between large molecules can be surprisingly strong.
For example, 
(water) molecules are capable of hydrogen bonding. The melting point of at 
is around 
. That's considerably high when compared to other three-atom molecules.
In comparison, the higher alkane hexadecane (
, straight-chain) isn't capable of hydrogen bonding. However, under a similar pressure, hexadecane melts at around 
above the melting point of water. The reason is that with such a large number of atoms (and hence electrons) per molecule, the London dispersion force between hexadecane molecules could well be stronger than that the hydrogen bonding between water molecules.
Similarly, the dipole moments in HCl (due to the highly-polar H-Cl bonds) are much stronger than those in hexadecane (due to the C-H bonds.) However, the boiling point of hexadecane under standard conditions is much higher (at around 
than that of HCl.
Hello there,
Ione pairs of electrons that are present in a molecule of C2O are...
4
Each Oxygen forms two bonds with Carbon
Hope I Helped!
-Char
It's a trick question because all of them contain both iconic and covalent bonds.
Hope it helps!! :) have fun
