Answer:
oxidation number of an element in any particular molecule or ion is the electrical charge it has based on a set of rules if an element has gained or lost electrons in a reaction
Answer : The volume of helium gas occupied are, 67.2 L
Explanation :
First we have to calculate the number of moles of helium gas.
As we know that, 1 mole of gas contains number of atoms.
As, number of helium atoms present in 1 mole of helium gas
So, number of helium atoms present in mole of helium gas
Now we have to calculate the volume of helium gas occupied.
As we know that at STP, 1 mole of gas occupies 22.4 L volume of gas.
As, 1 mole of helium gas occupies 22.4 L volume of helium gas
So, 2.999 mole of helium gas occupies volume of helium gas
Thus, the volume of helium gas occupied are, 67.2 L
Answer is: <span>the molarity of the diluted solution 0,043 M.
</span>V(NaOH) = 75 mL ÷ 1000 mL/L = 0,075 L.
c(NaOH) = 0,315 M = 0,315 mol/L.
n(NaOH) = c(NaOH) · V(NaOH).
n(NaOH) = 0,075 L · 0,315 mol/L.
n(NaOH) = 0,023625 mol.
V(solution) = 0,475 L + 0,75 L.
c(solution) = 0,023625 mol ÷ 0,550 L.
c(solution) = 0,043 mol/L.
Answer:
Aluminum (Al) is the only metal in period 3 on the periodic table.
Answer:
The maximum wavelength of light that can dissociate diatomic chlorine into the monatomic chlorine form is 984 nm.
Explanation:
Given: ΔHf° value for atomic chlorine is +121.7 kJ/mol
1 Step
Converting kJ/mol into kJ (knowing that in 1 mol there is 6.023*10^23 molecules)
ΔHf° in kJ = 121.7 kJ/mol* 1 mole / 6.023*10^23
ΔHf° = 2.02*10^-22 kJ
ΔHf° = E = 2.02*10^-19 J
2 Step
Converting ΔHf° to a wavelength:
knowing the E = h*C/У
h = 6.626 x 10^-34 J·s
C = 3.00 x 10^8 m/s
У = h*C/E = (6.63 x 10^-34 J·s)(3.00 x 108 m/s) / 2.02*10^-19 J
У = 9.84*10^-7 m = 984 nm
3 Step (What type of radiation?)
UV-A wavelength range = 315 nm to 400 nm
UV-B wavelength range = 280 nm to 315 nm
UV-C wavelength range = 100 nm to 280 nm
This wavelength is not corresponding to any of the wavelength range (UV-A, UV-B, UV-C).