Question

1. A 2.00 g sample of silver nitrate is dissolved in water and then reacted with 0.250 g of copper metal, according to the reaction below. Answer the questions about this process.

2 AgNO₃ (aq) + Cu (s) --> Cu(NO₃)₂ (aq) + 2 Ag (s)

What mass of the excess reactant remains after the reaction goes to completion?

(I want to see if you guys get this correct because I have no idea how to approach because it doesn't tell us which reactant to solve for)

Answer 1

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Cucs? + 244 MOzcaq) → Cu (103) (02, + 2 Ag 0.250gm Giren agm molar mass of Cu = 63-5 gm/mol molar mass of AgNO3 = 170 gr/mol from reaction it is clear that 2x170gm AgNO3 reacts with 63-5 gm Cu so 2 gm AgNO3 reacts with 2x 63-5 grau 2 x 170 =0.37gmcu @ 63-5 gm Cu reacts with 2x170gm Agnoz So 0.250 gm Cu reacts with 2x170x0.250 gm AgNO3 here Cu is Limiting reagent = 1:34 gm Agno, 63.5 Im Agnoz mass of AgNO3 in excess = Given - Reached - mass mass mass of AgNO3 =2.0-1-34 in excess =10.66m