Iron is more reactive than silver.
Iron reacts with silver nitrate solution to form solid silver and an iron nitrate salt.
Two possible balanced equations for this reaction are:
Equation 1: Fe+2AgNO3→Fe(NO3)2+2Ag\text{Fe} + 2\text{AgNO}_3 \rightarrow \text{Fe}(\text{NO}_3)_2 + 2\text{Ag}Fe+2AgNO3→Fe(NO3)2+2Ag
Equation 2: Fe+3AgNO3→Fe(NO3)3+3Ag\text{Fe} + 3\text{AgNO}_3 \rightarrow \text{Fe}(\text{NO}_3)_3 + 3\text{Ag}Fe+3AgNO3→Fe(NO3)3+3Ag
In an experiment, 2.80 g of iron is reacted with an excess of silver nitrate solution. After the reaction is complete, the solid silver formed is filtered, dried, and weighed. The mass of silver obtained is 10.80 g.
Carry out a calculation, using this information, to show which equation represents the reaction taking place. (Relative atomic masses, ArA_rAr: Fe=56\text{Fe} = 56Fe=56, Ag=108\text{Ag} = 108Ag=108)
258 exam-style questions on Edexcel GCSE Chemistry Calculations involving masses. Each one has a worked solution and a mark scheme showing where the marks go.