Lewis structure of Fe2s3
1. Lewis structure of Fe2s3
Answer:
Lewis structure of Fe2s3 is the one who teaches us like math and he also teaches a lot of children like us this is a big help to us because we get an example in his videos
Explanation:
si Lewis structure of Fe2s3 siya yung nagtuturo sa atin kagaya ng math at madami rin syang natuturuan na mga bata katulad natin malaking tulong ito saatin dahil nakakakuha tayo ng halimbawa sa kanyang mga video.
2. How many moles of Fe2S3
Answer:
Molar mass of Fe2S3 is 207.8850 g/mol
207.8850/////////////
3. when the equation Fe+S --> Fe2S3 is balanced, what is the coefficient for sulfur?
Problem:
Balance the equation Fe + S₈ ⇒ Fe₂ S₃
Answer:
16 Fe + 3 S₈ ⇒ 8 Fe₂S₃ ↓ ↓ Reactant ProductThe coefficient for sulfur in the reactant will be 3.
We need to balance the equation in every chemical reaction since according to the law of conservation of mass, "during chemical reaction, atoms are not destroyed or change" which means, the mass of reactant will always be equal to the mass of the product.
In balancing, we can add the coefficient which is the number before the element or the compound in the equation. coefficient also must be a whole number not a fraction or decimal number.
For more information, kindly visit the link below:
brainly.ph/question/2134122
4. For the reaction 2Fe + 3S → Fe2S3, how many grams of sulfur are involved in this reaction if 95 grams of iron are needed to react with sulfur?
Answer:
83 g
Explanation:
Step 1: Write the balanced equation
2 Fe + 3 S ⇒ Fe₂S₃
Step 2: Calculate the moles corresponding to 95 g of Fe
The molar mass of Fe is 55.85 g/mol.
95 g × 1 mol/55.85 g = 1.7 mol
Step 3: Calculate the moles of S needed to react with 1.7 moles of Fe
The molar ratio of Fe to S is 2:3. The moles of S needed are 3/2 × 1.7 mol = 2.6 mol
Step 4: Calculate the mass corresponding to 2.6 moles of S
The molar mass of S is 32.07 g/mol.
2.6 mol × 32.07 g/mol = 83 g
5. What is the predominant IMFA for iron sulfide (Fe2S3)? a. Hydrogen bonding b. Dispersion force c. Ion-dipole interaction d. Dipole-dipole interaction
Answer:
A.hydrogen bonding
Explanation:
Also indicate which force, hydrogen bonding (H), dipolar (P), or dispersion (D)
hopp is help6. 8. For the reaction 2Fe + 39 → Fe2S3, how many grams of sulfur are involved in thisreaction if 83 grams of iron are needed to react with sulfur?A. 2.2B. 63.4C. 68.3D.71
Answer:
A
Explanation:
Hope it helps☺️❤️ ty ty
7. 1.) Sixty grams of FeCl3 reacts with 50.0 grams of H2S. 2 FeCl3 (s) + 3 H2S (g) ---> 6 HCl + Fe2S3 (s) (A) What is the limiting reactant? (B) What is the mass of HCl produced?
Solution (A):
Step 1: Calculate the molar mass of each reactant.
For FeCl₃
molar mass = (55.85 g/mol × 1) + (35.45 g/mol × 3)
molar mass = 162.2 g/mol
For H₂S
molar mass = (1.008 g/mol × 2) + (32.07 g/mol × 1)
molar mass = 34.086 g/mol
Step 2: Determine the mole ratios needed.
Using FeCl₃
mole ratio = 2 mol FeCl₃ : 6 mol HCl
Using H₂S
mole ratio = 3 mol H₂S : 6 mol HCl
Step 3: Calculate the number of moles of HCl produced by each reactant.
Using FeCl₃
[tex]\text{moles of HCl = 60.0 g FeCl₃} × \frac{\text{1 mol FeCl₃}}{\text{162.2 g FeCl₃}} × \frac{\text{6 mol HCl}}{\text{2 mol FeCl₃}}[/tex]
[tex]\text{moles of HCl = 1.1097 mol}[/tex]
Using H₂S
[tex]\text{moles of HCl = 50.0 g H₂S} × \frac{\text{1 mol H₂S}}{\text{34.086 g H₂S}} × \frac{\text{6 mol HCl}}{\text{3 mol H₂S}}[/tex]
[tex]\text{moles of HCl = 2.934 mol}[/tex]
Step 4: Determine the limiting reactant.
Since FeCl₃ produces less number of moles of HCl
[tex]\boxed{\text{FeCl₃ is the limiting reactant.}}[/tex]
Solution (B)
Step 1: Calculate the molar mass of HCl.
molar mass = (1.008 g/mol × 1) + (35.45 g/mol × 1)
molar mass = 36.458 g/mol
Step 2: Calculate the mass of HCl produced.
Since FeCl₃ is the limiting reactant
[tex]\text{mass of HCl = 1.1097 mol HCl} × \frac{\text{36.458 g HCl}}{\text{1 mol HCl}}[/tex]
[tex]\boxed{\text{mass of HCl = 40.46 g}}[/tex]
#CarryOnLearning
8. 1.) Sixty grams of FeCl3 reacts with 50.0 grams of H2S. 2 FeCl3 (s) + 3 H2S (g) ---> 6 HCl + Fe2S3 (s) (A) What is the limiting reactant? (B) What is the mass of HCl produced?
a. FeCl₃ as a limiting reactant
b. The mass of HCl produced : = 40.515 g
Further explanationA reaction coefficient is a number in the chemical formula of a substance involved in the reaction equation. The reaction coefficient is useful for equalizing reagents and products.
Given
60 g FeCl₃
50 g H₂S
Required
the limiting reactant
the mass of HCl
Solution
Reaction
2 FeCl₃ (s) + 3 H₂S (g) ⇒ 6 HCl + Fe₂S₃ (s)
a. The method that can be used to find limiting reagents is to divide the number of moles of known substances by their respective coefficients, and the small quotient will be used up or as a limiting reagent
mol FeCl₃ :
= 60 g : 162,2 g/mol
= 0.37
mol H₂S :
= 50 g : 34,1 g/mol
= 1.47
mol : coefficient :
FeCl₃ : H₂S = 0.37/2 : 1.47/3 = 0.185 : 0.49
FeCl₃ as a limiting reactant(smaller ratio)
b. mol HCl based on limiting reactant(FeCl₃)
From the equation, mol ratio FeCl₃ : HCl = 2 : 6, so mol HCl :
= 6/2 x mol FeCl₃
= 6/2 x 0.37
= 1.11
mass HCl :
= mol x molar mass
= 1.11 x 36.5 g/mol
= 40.515 g
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9. Exercise 5. On the basis of the equilibrium constant values, indicate for each reaction if the reactants or the products are favored. 1. NH3(aq) + H2O=NH4*(ag) + OH(aq) K = 1.8 x 10-5 2. PbC204= Pb2+(aq) + C2042- (aq) K= 1.0 x 10-11 3. HS-(aq) + H+ (aq) = H2S(aq) K= 1.0 x 107 4. H2O =H+ + OH-(aq) K = 1.0 x 10-14 5.2 Fe3+(aq) + 3 S2-(aq) = Fe2S3(s) K= 1.0 x 1088
Answer:
1.7
2.13
3.5
4.9
5.17
Explanation:
