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2 years ago

Cu + 2AgNO3 → Cu(NO3)2 + 2Ag

Chemistry

1 answer:

Eva8 [605]2 years ago

4 0

Answer:

$m_{Ag}=135.8gAg$

$Y=88.4\%$

Explanation:

Hello there!

In this case, according to the described chemical reaction, it is possible to compute the theoretical mass of silver as mass via the 1:2 mole ratio of copper to silver and their atomic mass in the periodic table, in order to perform the following stoichiometric setup:

$m_{Ag}=40.gCu*\frac{1molCu}{63.55gCu}*\frac{2molAg}{1molCu}*\frac{107.87gAg}{1molAg}\\\\ m_{Ag}=135.8gAg$

Next, given the actual yield of 120 g, we compute the percent yield via:

$Y=\frac{120g}{135.8g}*100\%\\\\Y=88.4\%$

Regards!

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Answer:

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4Al(s) + 3O₂ (g) ⇄ 2Al₂O₃ (s)

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