QuestionMay 14, 2025

18. A solution is prepared by dissolving 32 .0 g of NiSO_(4) in water. What current would be needed to deposit all of the nickel in 5.0 hours? A. 1.1 A B. 2.2 A C. 3.3 A D. 4.4 A E. 5.5 A

18. A solution is prepared by dissolving 32 .0 g of NiSO_(4) in water. What current would be needed to deposit all of the nickel in 5.0 hours? A. 1.1 A B. 2.2 A C. 3.3 A D. 4.4 A E. 5.5 A
18. A solution is prepared by dissolving 32 .0 g of NiSO_(4) in water. What current would be needed to deposit all of the nickel in 5.0 hours? A. 1.1 A B. 2.2 A C. 3.3 A D. 4.4 A E. 5.5 A

Solution
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Answer

B. 2.2 A Explanation 1. Calculate moles of NiSO_4 Molar mass of NiSO_4 is approximately 154.76 g/mol. Moles = \frac{32.0 \, \text{g}}{154.76 \, \text{g/mol}}. 2. Determine moles of Ni Each mole of NiSO_4 contains one mole of Ni. Therefore, moles of Ni = moles of NiSO_4. 3. Calculate charge needed to deposit Ni Use Faraday's law: Charge (C) = moles of Ni \times 96,485 C/mol (Faraday constant). 4. Calculate current Current (I) = \frac{\text{Charge (C)}}{\text{Time (s)}}. Convert 5 hours to seconds: 5 \times 3600 s.

Explanation

1. Calculate moles of $NiSO_4$<br /> Molar mass of $NiSO_4$ is approximately 154.76 g/mol. Moles = $\frac{32.0 \, \text{g}}{154.76 \, \text{g/mol}}$.<br />2. Determine moles of Ni<br /> Each mole of $NiSO_4$ contains one mole of Ni. Therefore, moles of Ni = moles of $NiSO_4$.<br />3. Calculate charge needed to deposit Ni<br /> Use Faraday's law: Charge (C) = moles of Ni $\times$ 96,485 C/mol (Faraday constant).<br />4. Calculate current<br /> Current (I) = $\frac{\text{Charge (C)}}{\text{Time (s)}}$. Convert 5 hours to seconds: $5 \times 3600$ s.
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