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Question about Galvanic and Electrolyte Cells

Chemistry

Originais Teachy

Galvanic and Electrolyte Cells

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(Originais Teachy 2023) - Question Easy of Chemistry

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During a visit to the Chemistry laboratory, the students learned about the functioning of batteries, being presented with a Daniell cell, in which one half-cell has a Zinc (Zn) electrode and 1.0 mol/L of ZnSO4, and the other half-cell contains a Copper (Cu) electrode and 1.0 mol/L of CuSO4. The students were instructed to check the standard reduction potential and oxidation potential of the half-cells (E¬į), determine the direction of the current, and calculate the potential difference (ddp) of the cell. Given this, answer: a) What is the standard reduction potential (E¬į) of the two half-cells of Zinc and Copper? Consult a table of reduction potentials. b) Considering the reduction potentials obtained in item a. Which is the anode and which is the cathode, and in which direction does the flow of electrons occur in the cell? c) Calculate the potential difference (ddp) between the Zinc and Copper electrodes in this Daniell cell, using the formula E¬į(cell) = E¬į(cathode) - E¬į(anode).

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In the laboratory, you are asked to calculate the enthalpy of formation for ammonia (NH3). You have the following data at your disposal: The enthalpy of formation for hydrogen gas (H2) is 0 kJ/mol, for nitrogen gas (N2) is 0 kJ/mol, and the enthalpy of reaction for the formation of ammonia is -92.4 kJ/mol. Using this information, calculate the enthalpy of formation for ammonia. Remember, the enthalpy of formation is the change in enthalpy when one mole of a substance is formed from its constituent elements.

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