Question
In the production of printed circuit boards for the electronics industry, a $0.60-\mathrm{mm}$ layer of copper is laminated onto an insulating plastic board. Next, a circuit pattern made of a chemically resistant polymer is printed on the board. The unwanted copper is removed by chemical etching, and the protective polymer is finally removed by solvents. One etching reaction is$\left[\mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4}\right] \mathrm{Cl}_{2}(a q)+4 \mathrm{NH}_{3}(a q)+\mathrm{Cu}(s)$$\longrightarrow 2\left[\mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4}\right] \mathrm{Cl}(a q)$a. Is this reaction an oxidation-reduction process? Explain.b. $A$ plant needs to manufacture 10,000 printed circuit boards, each $8.0 \times 16.0 \mathrm{~cm}$ in area. An average of $80 . \%$ of the copper is removed from each board (density of copper $=8.96$ $\mathrm{g} / \mathrm{cm}^{3}$ ). What masses of $\left[\mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4}\right] \mathrm{Cl}_{2}$ and $\mathrm{NH}_{3}$ are neededto do this? Assume $100 \%$ yield.
Step 1
Each board has an area of \(8.0 \, \text{cm} \times 16.0 \, \text{cm} = 128.0 \, \text{cm}^2\). For 10,000 boards, the total area is: \[ 10,000 \, \text{boards} \times 128.0 \, \text{cm}^2/\text{board} = 1,280,000 \, \text{cm}^2 \] Show more…
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In the production of printed circuit boards for the electronics industry, a 0.60 -mm layer of copper is laminated onto an insulating plastic board. Next, a circuit pattern made of a chemically resistant polymer is printed on the board. The unwanted copper is removed by chemical etching, and the protective polymer is finally removed by solvents. One etching reaction is $\left[\mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4}\right] \mathrm{Cl}_{2}(a q)+4 \mathrm{NH}_{3}(a q)+\mathrm{Cu}(s) \longrightarrow$ $2\left[\mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4}\right] \mathrm{Cl}(a q)$ a. Is this reaction an oxidation-reduction process? Explain. b. A plant needs to manufacture 10,000 printed circuit boards, each $8.0 \mathrm{cm} \times 16.0 \mathrm{cm}$ in area. An average of $80 . \%$ of the copper is removed from each board (density of copper $=8.96 \mathrm{g} / \mathrm{cm}^{3}$ ). What masses of $\left[\mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4}\right] \mathrm{Cl}_{2}$ and $\mathrm{NH}_{3}$ are needed to accomplish this task? Assume $100 \%$ yield.
In the production of printed circuit boards for the electronics industry, a 0.60 -mm layer of copper is laminated onto an insulating plastic board. Next, a circuit pattern made of a chemically resistant polymer is printed on the board. The unwanted copper is removed by chemical etching, and the protective polymer is finally removed by solvents. One etching reaction is $$ \mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{Cl}_{2}(a q)+4 \mathrm{NH}_{3}(a q)+\mathrm{Cu}(s) \longrightarrow $$ $$ 2 \mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{Cl}(a q) $$ A plant needs to manufacture $10,000$ printed circuit boards, each $8.0 \times 16.0 \mathrm{cm}$ in area. An average of $80 . \%$ of the copper is removed from each board (density of copper $=8.96 \mathrm{g} / \mathrm{cm}^{3}$ . What masses of $\mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{Cl}_{2}$ and $\mathrm{NH}_{3}$ are needed to do this? Assume 100$\%$ yield.
Copper is an excellent electrical conductor widely used in making electric circuits. In producing a printed circuit board for the electronics industry, a layer of copper is laminated on a plastic board. A circuit pattern is then printed on the board using a chemically resistant polymer. The board is then exposed to a chemical bath that reacts with the exposed copper, leaving the desired copper circuit, which has been protected by the overlaying polymer. Finally, a solvent removes the polymer. One reaction used to remove the exposed copper from the circuit board is $$ \mathrm{Cu}(s)+\mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{Cl}_{2}(a q)+4 \mathrm{NH}_{3}(a q) \underset{2 \mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{Cl}(a q)} $$ A plant needs to produce 5000 circuit boards, each with a surface area measuring $2.0$ in. $\times 3.0$ in. The boards are covered with a 0.65-mm layer of copper. In subsequent processing, $85 \%$ of the copper is removed. Copper has a density of $8.96 \mathrm{~g} / \mathrm{cm}^{3} .$ Calculate the masses of $\mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4}$ $\mathrm{Cl}_{2}$ and $\mathrm{NH}_{3}$ needed to produce the circuit boards, assuming that the reaction used gives a $97 \%$ yield.
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