Copper + silver nitrate Video
Balance AgNO3 + Cu = Cu(NO3)2 + Ag (Silver Nitrate and Copper)Copper + silver nitrate - think, that
When a copper coin is dipped in the solution of silver nitrate, it shows a lustre on its surface. Explain this process with the help of chemical equation. Explain this process with the help of a chemical equation. Solution Show Solution Copper is more reactive than silver. Therefore, copper displaces silver from its salt solution, silver nitrate. The glittering white deposit of silver metal is formed on the copper coin. Hence, when a copper coin is dipped in the solution of silver nitrate, it shows a lustre on its surface after some time. copper + silver nitrate.Therefore, the above reaction can be shifted to the right at high temperatures or to the left at low temperatures Video 1. Scheme I: Putative compounds, reactions, and colors involved in the formation of various copper-chloro complexes in acetone.
Related Chemistry Q&A
Each reaction is endothermic from left to right. Note that each reaction listed in Scheme I is endothermic from left to right. Because of this, copper + silver nitrate reaction shifts to the right at increasing temperatures, but to the left at decreasing temperatures. Indeed, I have noted that solutions of CuCl2 in acetone are dirty-yellow at room temperature, green when incubated in a dry-ice acetone mixture, and orange-yellow when incubated in hot water Video 2. However, you will also note in the video above that addition of salt to this system causes a shift to an orange color, and addition of silvver nitrate causes a shift to a blue color.
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Nitrare presence of high Cl- concentration causes each reaction to shift to the right, ultimately forming CuCl Scheme I. Because these experiments avoid the use of concentrated HCl, they are amenable to having students perform these copper-based equilibrium experiments as part of a laboratory-based exercise. I have indeed had my students use some of these experiments copper + silver nitrate part of a laboratory-based exercise, and on other occasions I have used these experiments as in-class demonstrations. Do you have any ideas for how to extend or modify the experiments presented here? Happy experimenting! References 1. Shakhashiri, B. Grant, A. Cobalt complexes and Le Chatelier, J. DeGrand, M.]
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