Write the electronic configuration of iron in fecl2 and fecl3
2 answers:
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Answer:
The range of [H⁺] is from 2.51 x 10⁻⁶ M to 6.31 x 10⁻⁶ M,
Explanation:
To answer this problem we need to keep in mind the <u>definition of pH</u>:
- pH = -log [H⁺]
So now we <u>calculate [H⁺] using a pH value of 5.2 and of 5.6</u>:
- 5.2 = -log [H⁺]
-5.2 = log [H⁺]
= [H⁺]
6.31 x 10⁻⁶ M = [H⁺]
- 5.6 = -log [H⁺]
-5.6 = log [H⁺]
= [H⁺]
2.51 x 10⁻⁶ M = [H⁺]
Hello!
In a chemical reaction, 28g of iron reacts with 16g of sulfur to produce _________ of iron sulfide.
We have the following data:
m(Fe) - mass of iron = 28 g
m(S) - mass of sufur = 16 g
MM(Fe) - molar mass of iron ≈ 56 g/mol
MM(S) - molar mass of sulfur ≈ 32 g/mol
n(Fe) - number of mol of iron = ?
n(S) - number of mol of sulfur = ?
Solving:
* to n(Fe)
* to n(S)
The stoichiometric reaction will be in the same proportion (1 : 1), let us see:
1 mol of Fe -------------- 1 mol of FeS
0.5 mol of Fe ------------ 0.5 mol of FeS
Will the reaction of the iron mass with the mass of sulfur produce how many grams of iron sulfide? We will see:
n(FeS) - number of mol of iron sulfide = 0.5 mol
m(FeS) - mass of iron sulfide = ? (in grams)
MM(FeS) - Molar Mass of iron sulfide = 56 + 32 = 88 g/mol
Solving:
Answer:
44 grams of iron sulfide
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