01-14-2020, 03:04 AM
write a balanced equation for the reaction between aluminium metal and potassium hydroxide in waterHi there! So you\'re given Aluminum metal, which has the oxidation state (almost always) of 3+. In play are: Al 3+ K+ OH- You have KOH(aq) + Al 3+ and they react to form a precipitate, creating Al(OH)3 and the potassium cation disperses into solution. In traditional symbols: 3 KOH (aq) + Al 3+(s) ----- Al(OH)3(s) + 3K+ (aq) That\'s 3 K+, 3 OH-, and 1 Al 3+. That carries for both sides! NIE would look like: 3 OH- + Al 3+ ----- Al(OH)3 (s) Most instructors don\'t mind if you leave off (aq) but pretty much all of them care about (s), so make sure you add those phase states! I hope I helped 
Potassium Aluminum HydroxideSo convert 27,8 g iron to moles, and convert that to a mass of aluminium 2. 3 CuNO3 + Fe3+ -- Fe(NO3)3 + 3 Cu+ 3. 2 Fe3+ + 3 O2- --- Fe2O3 So convert Fe2O3 from 20,8 grams to moles. Multiply this answer by two. Convert to a mass of Fe3+ 4. H2SO4 + 2 KOH -- K2SO4 + 2 H2O again, 150 grams of H2SO4 to moles, then convert that amount to an amount of mass of K2SO4 5. Na2CO3 + 2 H3O+ + Cl- --- CO2 + 3 H2O + NaClOther related question
Potassium Aluminum HydroxideSo convert 27,8 g iron to moles, and convert that to a mass of aluminium 2. 3 CuNO3 + Fe3+ -- Fe(NO3)3 + 3 Cu+ 3. 2 Fe3+ + 3 O2- --- Fe2O3 So convert Fe2O3 from 20,8 grams to moles. Multiply this answer by two. Convert to a mass of Fe3+ 4. H2SO4 + 2 KOH -- K2SO4 + 2 H2O again, 150 grams of H2SO4 to moles, then convert that amount to an amount of mass of K2SO4 5. Na2CO3 + 2 H3O+ + Cl- --- CO2 + 3 H2O + NaClOther related question