The Reaction of Iron Nails with a Copper Solution
Mass of the empty dry beaker = 105.52 g
Initial mass of the beaker + CuCl2 (s) = 113.02 g
Initial mass of the two iron nails = 3.82 g
Final mass of the dry beaker and copper = 106.41 g
Final mass of the two iron nails = 3.04 g
1. What mass of CuCl2 (s) is used?
What mass of iron is consumed in the reaction?
How many moles of iron are consumed?
What mass of Cu is produced in the reaction?
How many moles of Cu are produced?
Find the ratio of the moles of copper produced to moles of iron consumed.
Determine the number of atoms of iron reacting and the number of atoms of copper produced.
The blue colour of the solution gets lighter as the reaction proceeds. What does this indicate? Explain your answer.
Write a balanced equation for the reaction. This is a single replacement reaction.
How many moles, how many atoms, and what mass of Cu (s) are produced by the reaction when 100. grams of iron completely reacts, assuming there is enough CuCl2 (aq)?
The reaction takes place is shown below.
`Fe_(s) + CuCl_(2(aq)) rarr Cu_(s) + FeCl_(3(aq))`
Here Fe is oxidized to `Fe^(3+)` and `Cu^(2+)` is reduced to Cu.
`2Fe_(s) + 3CuCl_(2(aq)) rarr 3Cu_(s) + 2FeCl_(3(aq))`
So in the beaker iron will dissolve and Cu will precipitate.
Cu = 63.5g/mol
Fe = 56g/mol
Mass of the empty dry beaker (M1)= 105.52 g
Initial mass of the beaker + CuCl2 (s) (M2)= 113.02 g
Initial mass of the two iron nails (M3)= 3.82 g
Final mass of the dry beaker and copper (M4)= 106.41 g
Final mass of the two iron nails (M5)= 3.04 g
Weight of `CuCl_2` used for reaction
Since i can answer one question as a editor i should omit the other parts.