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Chapter 1 - Transition Elements and Iron Metallurgy

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Chapter 3 - Chemical Equilibrium

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Lesson 2 Quiz: Ionic Equilibrium, pH Scale, Hydrolysis and Solubility Product (Ksp)

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1.
STEM Faradaic Problem 40: What mass of copper (atomic mass = 63.5 g/mol) is deposited at the cathode when a constant current of 9.65 A passes through a CuSO4 solution for 1,000 seconds? (Faraday constant = 96,500 C/mol)
6.35 g of Cu
3.175 g of Cu
12.70 g of Cu
1.587 g of Cu
2.
STEM Faradaic Problem 8: What mass of copper (atomic mass = 63.5 g/mol) is deposited at the cathode when a constant current of 9.65 A passes through a CuSO4 solution for 1,000 seconds? (Faraday constant = 96,500 C/mol)
12.70 g of Cu
3.175 g of Cu
6.35 g of Cu
1.587 g of Cu
3.
STEM Faradaic Problem 5: What mass of copper (atomic mass = 63.5 g/mol) is deposited at the cathode when a constant current of 9.65 A passes through a CuSO4 solution for 1,000 seconds? (Faraday constant = 96,500 C/mol)
3.175 g of Cu
1.587 g of Cu
6.35 g of Cu
12.70 g of Cu
4.
STEM Faradaic Problem 13: What mass of copper (atomic mass = 63.5 g/mol) is deposited at the cathode when a constant current of 9.65 A passes through a CuSO4 solution for 1,000 seconds? (Faraday constant = 96,500 C/mol)
3.175 g of Cu
1.587 g of Cu
12.70 g of Cu
6.35 g of Cu
5.
STEM Faradaic Problem 32: What mass of copper (atomic mass = 63.5 g/mol) is deposited at the cathode when a constant current of 9.65 A passes through a CuSO4 solution for 1,000 seconds? (Faraday constant = 96,500 C/mol)
3.175 g of Cu
12.70 g of Cu
1.587 g of Cu
6.35 g of Cu
6.
STEM Faradaic Problem 10: What mass of copper (atomic mass = 63.5 g/mol) is deposited at the cathode when a constant current of 9.65 A passes through a CuSO4 solution for 1,000 seconds? (Faraday constant = 96,500 C/mol)
3.175 g of Cu
1.587 g of Cu
6.35 g of Cu
12.70 g of Cu
7.
STEM Faradaic Problem 24: What mass of copper (atomic mass = 63.5 g/mol) is deposited at the cathode when a constant current of 9.65 A passes through a CuSO4 solution for 1,000 seconds? (Faraday constant = 96,500 C/mol)
3.175 g of Cu
12.70 g of Cu
1.587 g of Cu
6.35 g of Cu
8.
STEM Faradaic Problem 28: What mass of copper (atomic mass = 63.5 g/mol) is deposited at the cathode when a constant current of 9.65 A passes through a CuSO4 solution for 1,000 seconds? (Faraday constant = 96,500 C/mol)
6.35 g of Cu
12.70 g of Cu
1.587 g of Cu
3.175 g of Cu
9.
STEM Faradaic Problem 3: What mass of copper (atomic mass = 63.5 g/mol) is deposited at the cathode when a constant current of 9.65 A passes through a CuSO4 solution for 1,000 seconds? (Faraday constant = 96,500 C/mol)
6.35 g of Cu
12.70 g of Cu
3.175 g of Cu
1.587 g of Cu
10.
STEM Faradaic Problem 21: What mass of copper (atomic mass = 63.5 g/mol) is deposited at the cathode when a constant current of 9.65 A passes through a CuSO4 solution for 1,000 seconds? (Faraday constant = 96,500 C/mol)
6.35 g of Cu
3.175 g of Cu
12.70 g of Cu
1.587 g of Cu
11.
STEM Faradaic Problem 12: What mass of copper (atomic mass = 63.5 g/mol) is deposited at the cathode when a constant current of 9.65 A passes through a CuSO4 solution for 1,000 seconds? (Faraday constant = 96,500 C/mol)
3.175 g of Cu
6.35 g of Cu
1.587 g of Cu
12.70 g of Cu
12.
STEM Faradaic Problem 36: What mass of copper (atomic mass = 63.5 g/mol) is deposited at the cathode when a constant current of 9.65 A passes through a CuSO4 solution for 1,000 seconds? (Faraday constant = 96,500 C/mol)
3.175 g of Cu
6.35 g of Cu
1.587 g of Cu
12.70 g of Cu
13.
STEM Faradaic Problem 16: What mass of copper (atomic mass = 63.5 g/mol) is deposited at the cathode when a constant current of 9.65 A passes through a CuSO4 solution for 1,000 seconds? (Faraday constant = 96,500 C/mol)
12.70 g of Cu
3.175 g of Cu
6.35 g of Cu
1.587 g of Cu
14.
STEM Faradaic Problem 15: What mass of copper (atomic mass = 63.5 g/mol) is deposited at the cathode when a constant current of 9.65 A passes through a CuSO4 solution for 1,000 seconds? (Faraday constant = 96,500 C/mol)
6.35 g of Cu
12.70 g of Cu
1.587 g of Cu
3.175 g of Cu
15.
STEM Faradaic Problem 39: What mass of copper (atomic mass = 63.5 g/mol) is deposited at the cathode when a constant current of 9.65 A passes through a CuSO4 solution for 1,000 seconds? (Faraday constant = 96,500 C/mol)
3.175 g of Cu
1.587 g of Cu
6.35 g of Cu
12.70 g of Cu
16.
STEM Faradaic Problem 7: What mass of copper (atomic mass = 63.5 g/mol) is deposited at the cathode when a constant current of 9.65 A passes through a CuSO4 solution for 1,000 seconds? (Faraday constant = 96,500 C/mol)
3.175 g of Cu
6.35 g of Cu
1.587 g of Cu
12.70 g of Cu
17.
STEM Faradaic Problem 44: What mass of copper (atomic mass = 63.5 g/mol) is deposited at the cathode when a constant current of 9.65 A passes through a CuSO4 solution for 1,000 seconds? (Faraday constant = 96,500 C/mol)
1.587 g of Cu
6.35 g of Cu
3.175 g of Cu
12.70 g of Cu
18.
STEM Faradaic Problem 22: What mass of copper (atomic mass = 63.5 g/mol) is deposited at the cathode when a constant current of 9.65 A passes through a CuSO4 solution for 1,000 seconds? (Faraday constant = 96,500 C/mol)
6.35 g of Cu
1.587 g of Cu
12.70 g of Cu
3.175 g of Cu
19.
STEM Faradaic Problem 42: What mass of copper (atomic mass = 63.5 g/mol) is deposited at the cathode when a constant current of 9.65 A passes through a CuSO4 solution for 1,000 seconds? (Faraday constant = 96,500 C/mol)
6.35 g of Cu
12.70 g of Cu
3.175 g of Cu
1.587 g of Cu
20.
STEM Faradaic Problem 31: What mass of copper (atomic mass = 63.5 g/mol) is deposited at the cathode when a constant current of 9.65 A passes through a CuSO4 solution for 1,000 seconds? (Faraday constant = 96,500 C/mol)
1.587 g of Cu
6.35 g of Cu
3.175 g of Cu
12.70 g of Cu
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