According to its formula FeSO4.7H2O
we can get the percent % by the mass of H2O from this formula
%mass of H2O = (mass of water H2O/ mass of the hydrate)x100
when the mass of water = molar mass x 7 = 18 x 7 = 126
and the mass of hydrate (feSO4) = molar mass = 278
So by substitution:
%mass of H2O = (126/278) x 100 = 45%
We assume that the volume of the molecules themselves in a gas sample is negligible compared to the bulk volume of the gas sample: this helps us to explain why gases are so compressible.
According to this equation:
AgCl(s) ↔ Ag+(aq) + Cl-(aq)
so K1 = [Ag+][Cl-]
when [Ag+] = [Cl-] we can assume both = X
and when we have X the solubility = 1.33 x 10^-5 mol / L
by substitution:
∴ K1 = X^2
= (1.33 x 10^-5)^2
= 1.77 x 10^-10
by using vant's Hoff equation:
ln(K2/K1) = (ΔH/R)*(1/T2-1/T1)
when ΔH = 65700 J / mol
R = 8.314
T1 = 25+273 = 298 K
T2 = 47.7 +273 =320.7
by substitution:
∴㏑(K2/1.77 x 10^-10) = (65700/8.314) * ( 1/320.7 - 1/ 298)
by solving for K2
∴K2 = 2.7 x 10^-11
and when K2 = X^2
∴ the solubility X = √(2.7 x 10^-11)
= 5.2 x 10^-6 mol/L
The first one
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Answer:
Explanation:
The oxidation reduction reactions are called redox reaction. These reactions are take place by gaining or losing the electrons and oxidation state of elements are changed.
Oxidation:
Oxidation involve the removal of electrons and oxidation state of atom of an element is increased.
Reduction:
Reduction involve the gain of electron and oxidation number is decreased.
Oxidizing agents:
Oxidizing agents oxidize the other elements and itself gets reduced.
Reducing agents:
Reducing agents reduced the other element are it self gets oxidized.
In given example,
Magnesium is able to <u>reduced</u> the copper and copper is able to <u>oxidized</u> the magnesium.
Zinc is able to <u>oxidized</u> the magnesium and magnesium is able to <u>reduced</u> the zinc.
Copper is able to <u>oxidized</u> the zinc and zinc is able to <u>reduced</u> the copper.
