This is all part of the same problem. Please answer everything, I do not know ho
ID: 517783 • Letter: T
Question
This is all part of the same problem. Please answer everything, I do not know how to do it and I need help.
Unknown # 14
Trial
Mass FeCl2(g)
Volume KMnO4 (mL)
Molarity KMnO4 (mol/L)
1
2.0124
30.01
2.72
2
2.0464
30.65
2.66
3
1.9772
30.13
2.70
Write a balanced net ionic equation for the reaction in acidic solution of FeCl2 and KMnO4
What are the moles of MnO4- used in the titration?
How many moles of FeCl2 were in the unknown?
What is the mass of FeCl2 in the sample?
What is the % FeCl2 in the unknown sample?
What is the average % iron in the unknown sample using your best three answers?
Trial
Mass FeCl2(g)
Volume KMnO4 (mL)
Molarity KMnO4 (mol/L)
1
2.0124
30.01
2.72
2
2.0464
30.65
2.66
3
1.9772
30.13
2.70
Explanation / Answer
The balanced net ionic equation for the reaction in acidic solution of FeCl2 and KMnO4 as follows:
KMnO4 + 5 FeCl2 + 8 HCl --> MnCl2 + 5 FeCl3 + KCl + 4 H2O
MnO4^- + 5 Fe^2+ + 8 H^+ --> Mn^2+ + 5 Fe^3+ + 4 H2O
What are the moles of MnO4- used in the titration?
Trial 1
Number of moles = molarity * volume in L
= 2.72*30.01/1000= 0.082 Moles MnO4–
Trial 2
Number of moles = molarity * volume in L
= 2.66*30.65/1000= 0.082 Moles MnO4–
Trial 3
Number of moles = molarity * volume in L
= 2.70*30.13/1000= 0.081 Moles MnO4–
How many moles of FeCl2 were in the unknown?
MnO4^- + 5 Fe^2+ + 8 H^+ --> Mn^2+ + 5 Fe^3+ + 4 H2O
Trail 1:
moles of FeCl2 =
0.082 Moles MnO4– *5/1
= 0.41 moles of FeCl2
Trail 2:
moles of FeCl2 =
0.082 Moles MnO4– *5/1
= 0.41 moles of FeCl2
Trail 3:
moles of FeCl2 =
0.081 Moles MnO4– *5/1
= 0.405 moles of FeCl2
What is the mass of FeCl2 in the sample?
molar mass of FeCl2 = 126.751 g/mol
Trail 1:
the mass of FeCl2 in the sample=
moles of FeCl2 * molar mass of FeCl2, 126.751 g/mol
= 0.41 moles of FeCl2 *126.751 g/mol
= 51.97 g FeCl2
Trail 2:
the mass of FeCl2 in the sample=
moles of FeCl2 * molar mass of FeCl2, 126.751 g/mol
= 0.41 moles of FeCl2 *126.751 g/mol
= 51.97 g FeCl2
Trail 3:
the mass of FeCl2 in the sample=
moles of FeCl2 * molar mass of FeCl2, 126.751 g/mol
= 0.405 moles of FeCl2 *126.751 g/mol
= 51.33 g FeCl2
What is the % FeCl2 in the unknown sample?
% FeCl2 in the unknown sample = mass of FeCl2 in the sample / sample mass*100
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