Since 8x3=24 and since 12x3=36 you need to add 6oz of chemical B to have 24oz of chemical A and 36oz of chemical B. Take 1/3 of the total mixture...
1 Answers 1 viewsClearly, there are $6$ oxygen atoms on the left hand side of the equation; and, equally clearly, there are $6$ oxygen atoms on the right hand side of the equation,...
1 Answers 1 viewsAlumina is $Al_2O_3$, which is the product of aluminum oxidation. None of your equations shows the correct formulae. We can rewrite the correct equation as: $2Al(s)+ 3/2O_2(g) rarr Al_2O_3(s)$ This...
1 Answers 1 viewsCount how many $Fe$ and $O_2$ you have on both left and right sides: You are given: $4Fe+3O_2 -> 2Fe_2O_3$ $4:Fe:4$ $6:O_2:6$ You actually have the same number of $Fe$...
1 Answers 1 viewsAluminum is oxidized; oxygen is reduced. What are the elemental oxidation states in $Al_2O_3$?
1 Answers 1 views$4Al(s) + 3O_2(g) rarr 2Al_2O_3(g)$ This is a redox reaction, and represents the oxidation of aluminum metal by dioxygen gas to give alumina.
1 Answers 1 viewsTo check excess and limiting reactants, the number of moles has to be found, and then divided by the coefficient. For the sake of shortening the equations, let us say...
1 Answers 1 viewsAnd we could represent this by half-equations....CLEARLY iron metal is oxidized.... $FerarrFe^(3+) + 3e^(-)$ $(i)$ And meanwhile, the potent OXIDANT, dioxygen gas is reduced to $O^(2-)$... $O_2(g) + 4e^(-) rarr...
1 Answers 1 viewsWe have the balanced equation: $4Fe(s)+3O_2(g)->2Fe_2O_3(s)$ And so, $4$ moles of iron react with $3$ moles of oxygen, and therefore, $12.9 \ "mol"$ of iron would react with: $12.9color(red)cancelcolor(black)("mol" \...
1 Answers 1 viewsThis can be solved through dimensional analysis. Atomic Masses: $"Fe = 55.85 g/mol"$ $"O = 16.00 g/mol"$ Formula Mass: $"Fe"_2"O"_3 ="159.69 g/mol"$ $"Moles of Fe" =73.2cancel("g Fe") xx...
1 Answers 1 views