Answer:
27.00 mL
Explanation:
Please see the step-by-step solution in the picture attached below.
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I found a similar problem to this as shown in the attached picture to helpme answer the problem. We use the M₁V₁ = M₂V₂ formula, wherein M₁ is the concentration of the original CuSO₄ solution, V₁ is the volume of CuSO₄ in the cuvette, M₂ is the concentration of Cu²⁺ in the cuvette, and V₂ is the total volume in the cuvette.
For cuvette 1:
M₁V₁ = M₂V₂
(0.06)(4 mL) = (M₂)(6+4 mL)
M₂ = <em>0.024 M Cu²⁺</em>
For cuvette 2:
M₁V₁ = M₂V₂
(0.06)(7 mL) = (M₂)(7+3 mL)
M₂ = <em>0.042 M Cu²⁺</em>
For cuvette 1:
M₁V₁ = M₂V₂
(0.06)(4 mL) = (M₂)(6+4 mL)
M₂ = <em>0.024 M Cu²⁺</em>
For cuvette 2:
M₁V₁ = M₂V₂
(0.06)(7 mL) = (M₂)(7+3 mL)
M₂ = <em>0.042 M Cu²⁺</em>
Answer:
0.161 moles
Explanation:
Given parameters:
Mass of Fe = 18g
Unknown:
Number of moles of Fe₂O₃ = ?
Solution:
To solve this problem, we have to work from the known to the unknown specie.
One cogent point we need to take from this problem is that oxygen gas is in excess. The Fe reacting is therefore the limiting reactant which implies that it will determine the extent of the reaction.
Now, the known specie is Fe;
The balanced reaction equation is shown below;
4Fe + 3O₂ → 2Fe₂O₃
Proceed to find the number of moles of Fe given;
Number of moles of Fe =
Molar mass of Fe = 56g/mol
Number of moles of Fe = = 0.32mole
From the balanced reaction equation;
4 moles of Fe produced 2 moles of Fe₂O₃
0.32 moles of Fe will produce = 0.161 moles of Fe₂O₃