(a) Calculate the mass of Li formed by electrolysis of molten LiCl by a current of 7.5 × 10⁴ A flowing for a period of 24 h. Assume the electrolytic cell is 85% efficient. (b) What is the minimum voltage required to drive the reaction?

검증된 단계별 안내

Step 1: Determine the total charge (Q) passed through the electrolytic cell using the formula Q = I \(\times\) t, where I is the current (7.5 \(\times\) 10^4 A) and t is the time in seconds (24 hours converted to seconds).

Step 2: Calculate the number of moles of electrons (n_e) using the formula n_e = \(\frac{Q}{F}\), where F is Faraday's constant (approximately 96485 C/mol).

Step 3: Use the stoichiometry of the reaction to find the moles of Li produced. The reaction is Li^+ + e^- \(\rightarrow\) Li, indicating a 1:1 mole ratio between electrons and lithium.

Step 4: Calculate the theoretical mass of Li produced using the formula mass = moles \(\times\) molar mass of Li (approximately 6.94 g/mol).

Step 5: Adjust for the efficiency of the cell by multiplying the theoretical mass by the efficiency (85%) to find the actual mass of Li produced.

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주요 개념

질문에 올바르게 답하기 위해 반드시 이해해야 하는 핵심 개념들은 다음과 같습니다.

Electrolysis

Electrolysis is a chemical process that uses electrical energy to drive a non-spontaneous reaction. In this process, an electric current is passed through an electrolyte, causing the decomposition of the compound. For molten LiCl, electrolysis results in the formation of lithium metal and chlorine gas at the electrodes. Understanding the principles of electrolysis is essential for calculating the mass of lithium produced.

Faraday's Laws of Electrolysis

Faraday's Laws of Electrolysis quantify the relationship between the amount of substance produced at an electrode and the quantity of electric charge passed through the electrolyte. The first law states that the mass of a substance altered at an electrode is directly proportional to the total electric charge passed. This principle is crucial for calculating the mass of lithium formed in the given electrolysis scenario.

Electrolytic Cell Efficiency

The efficiency of an electrolytic cell refers to the ratio of the actual amount of product formed to the theoretical amount predicted by Faraday's laws. In this case, the cell is stated to be 85% efficient, meaning that only 85% of the theoretical lithium mass calculated from the charge is actually produced. This efficiency factor is vital for accurately determining the mass of lithium formed during the electrolysis process.

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교과서 질문

A mixture of copper and gold metals that is subjected to electrorefining contains tellurium as an impurity. The standard reduction potential between tellurium and its lowest common oxidation state, Te4+, is Te4+1aq2 + 4 e- ¡ Te1s2 E°red = 0.57 V Given this information, describe the probable fate of tellurium impurities during electrorefining. Do the impurities fall to the bottom of the refining bath, unchanged, as copper is oxidized, or do they go into solution as ions? If they go into solution, do they plate out on the cathode?

423

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교과서 질문

(a) A Cr³⁺(aq) solution is electrolyzed, using a current of 7.60 A. What mass of Cr(s) is plated out after 2.00 days?

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(a) Calculate the mass of Li formed by electrolysis of molten LiCl by a current of 7.5 × 104 A flowing for a period of 24 h. Assume the electrolytic cell is 85% efficient. (b) What is the minimum voltage required to drive the reaction?

비슷한 문제에 대한 검증된 영상 답변:

주요 개념

Electrolysis

Faraday's Laws of Electrolysis

Electrolytic Cell Efficiency

(a) Calculate the mass of Li formed by electrolysis of molten LiCl by a current of 7.5 × 10⁴ A flowing for a period of 24 h. Assume the electrolytic cell is 85% efficient. (b) What is the minimum voltage required to drive the reaction?