Question

(part 1 of 3) Copper reacts with silver nitrate through a single replacement. If 1.29 g of silver are produced from the reaction, how much copper(II) nitrate is also produced? Answer in units of mol. (part 2 of 3) How much Cu is required in this reaction? Answer in units of mol. (part 3 of 3) 1.0 points How much AgNO3 is required in this reaction? Answer in units of mol.

Answer 1

See explanation.

Step-by-step 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`

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*(1molAg)/(107.87gAg)*(1molCu(NO_3)_2)/(2molAg)*(187.55gCu(NO_3)_2)/(1molCu(NO_3)_2) \\\\m_(Cu(NO_3)_2)=1.12gCu(NO_3)_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*(1molAg)/(107.87gAg)*(1molCu)/(2molAg)*(63.55gCu)_2)/(1molCu) \\\\m_(Cu)=0.380gCu`

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*(1molAg)/(107.87gAg)*(2molAgNO_3)/(2molAg)*(169.87gAgNO_3)/(1molAgNO_3) \\\\m_(AgNO_3)=2.03gAgNO_3`

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