Answer:
They should obtain the same Rf for the same compounds.
Explanation:
The <em>Rf</em> is defined as A/B. Where A is the displacement of the substance of interest, and B is the solvent front.
By dividing the substance's displacement by B, we make it so that the Rf factor is equal for identical compounds in the same mobile phase, no matter what the solvent front is.
<span>Kp is the equilibrium pressure constant calculated from the partial pressures of a reaction equation.
Kp =[pCF4]*[p CO2] / [p COF2]^2 = 2.2 x 10^6
When the mole fraction gets doubled we have
Kp = [pCO2]^2*[pCF4]^2 / [pCOF2]^4
Kp = [[pCF4]*[p CO2] / [p COF2]^2] * 2
Kp = (2.2 * 10^6) * 2
Kp = 4.8 * 10^12</span>
Answer:
See explanation
Explanation:
The p orbital is threefold degenerate. This implies that the p-sublevel is composed of three orbitals; px, py and pz.
According to Hund's rule, electrons occur singly when filling degenerate orbitals before pairing takes place. Since the three orbitals are degenerate, any of px, py or pz may be first filled.
If one lobe of any of the px, py or pz is first filled, the next electron must go into the next degenerate orbital. When all are filled, pairing of electron spins may now begin.
Answer:
ΔG = - 442.5 KJ/mol
Explanation:
Data Given
delta H = -472 kJ/mol
delta S = -108 J/mol K
So,
delta S = -0.108 J/mol K
delta Gº = ?
Solution:
The answer will be calculated by the following equation for the Gibbs free energy
G = H - TS
Where
G = Gibbs free energy
H = enthalpy of a system (heat
T = temperature
S = entropy
So the change in the Gibbs free energy at constant temperature can be written as
ΔG = ΔH - TΔS . . . . . . (1)
Where
ΔG = Change in Gibb’s free energy
ΔH = Change in enthalpy of a system
ΔS = Change in entropy
if system have standard temperature then
T = 273.15 K
Now,
put values in equation 1
ΔG = (-472 kJ/mol) - 273.15 K (-0.108 KJ/mol K)
ΔG = (-472 kJ/mol) - (-29.5 KJ/mol)
ΔG = -472 kJ/mol + 29.5 KJ/mol
ΔG = - 442.5 KJ/mol
