Answer:
See explanation.
Explanation:
Hello there!
In this case, according to the described chemical reaction, we first write the corresponding equation to obtain:
![Cu+2AgNO_3\rightarrow 2Ag+Cu(NO_3)_2](https://tex.z-dn.net/?f=Cu%2B2AgNO_3%5Crightarrow%202Ag%2BCu%28NO_3%29_2)
Thus, we proceed as follows:
Part 1 of 3: here, since the molar mass of silver and copper (II) nitrate are 107.87 and 187.55 g/mol respectively, and the mole ratio of the former to the latter is 2:1, we can set up the following stoichiometric expression:
![m_{Cu(NO_3)_2}=1.29gAg*\frac{1molAg}{107.87gAg}*\frac{1molCu(NO_3)_2}{2molAg}*\frac{187.55gCu(NO_3)_2}{1molCu(NO_3)_2} \\\\m_{Cu(NO_3)_2}=1.12gCu(NO_3)_2](https://tex.z-dn.net/?f=m_%7BCu%28NO_3%29_2%7D%3D1.29gAg%2A%5Cfrac%7B1molAg%7D%7B107.87gAg%7D%2A%5Cfrac%7B1molCu%28NO_3%29_2%7D%7B2molAg%7D%2A%5Cfrac%7B187.55gCu%28NO_3%29_2%7D%7B1molCu%28NO_3%29_2%7D%20%20%20%5C%5C%5C%5Cm_%7BCu%28NO_3%29_2%7D%3D1.12gCu%28NO_3%29_2)
Part 2 of 3: here, the molar mass of copper is 63.55 g/mol and the mole ratio of silver to copper is 2:1, the mass of the former that was used to start the reaction was:
![m_{Cu}=1.29gAg*\frac{1molAg}{107.87gAg}*\frac{1molCu}{2molAg}*\frac{63.55gCu)_2}{1molCu} \\\\m_{Cu}=0.380gCu](https://tex.z-dn.net/?f=m_%7BCu%7D%3D1.29gAg%2A%5Cfrac%7B1molAg%7D%7B107.87gAg%7D%2A%5Cfrac%7B1molCu%7D%7B2molAg%7D%2A%5Cfrac%7B63.55gCu%29_2%7D%7B1molCu%7D%20%20%20%5C%5C%5C%5Cm_%7BCu%7D%3D0.380gCu)
Part 3 of 3: here, the molar mass of silver nitrate is 169.87 g/mol and their mole ratio 2:2, thus, the mass of initial silver nitrate is:
![m_{AgNO_3}=1.29gAg*\frac{1molAg}{107.87gAg}*\frac{2molAgNO_3}{2molAg}*\frac{169.87gAgNO_3}{1molAgNO_3} \\\\m_{AgNO_3}=2.03gAgNO_3](https://tex.z-dn.net/?f=m_%7BAgNO_3%7D%3D1.29gAg%2A%5Cfrac%7B1molAg%7D%7B107.87gAg%7D%2A%5Cfrac%7B2molAgNO_3%7D%7B2molAg%7D%2A%5Cfrac%7B169.87gAgNO_3%7D%7B1molAgNO_3%7D%20%20%20%5C%5C%5C%5Cm_%7BAgNO_3%7D%3D2.03gAgNO_3)
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