Enter your answer in the provided box. Before arc welding was developed, a displacement reaction involving aluminum and iron(III) oxide was commonly used to produce molten iron (the thermite process). This reaction was used, for example, to connect sections of iron railroad track. Calculate the mass of molten iron produced when 1.64 kg of aluminum reacts with 20.2 mol of iron(III) oxide.

grams of iron = 2262.4  g

Explanation:

The balanced chemical equation should be represented first.  

2Al + Fe2O3 → Al2O3 + 2Fe

find the limiting reactants by converting to moles.

covert 1.64 kg to grams = 1640 g

moles = mass/molar mass = 1640/27 = 60.7407407407  moles

60.7407407407 × 1 mol-rxn /2 = 30.37  mol-rxn

The limiting reactant is Fe2O3 Therefore it will determine the yield of Iron

2Al + Fe2O3 → Al2O3 + 2Fe

molar mass of Fe2O3 = 56 × 2 + 16 × 3 =  112 + 48 = 160 g

atomic mass of iron = 56

mass of iron in the reaction = 56 × 2 = 112 g

moles = mass/molar mass

mass = moles × molar mass

mass = 20.2 × 160 = 3232  g

if 160 g of Fe2O3  give 112 g of iron

3232 g of Fe2O3 will give ? grams of iron

grams of iron = 3232 × 112/ 160

grams of iron = 361984 /160

grams of iron = 2262.4  g

b..

is the correct one

explanation:

covalent bonds form as valence electrons are shared between two atoms. lewis structures and structural formulas are common ways of showing the covalent bonding in organic molecules. formal charge describes the changes in the number of valence electrons as an atom becomes bonded into a molecule.

a 20-cm-long, cylindrical graphite (pure carbon) rod is inserted into an oxidizing atmosphere at 1145 k and 1.013 x 105 pa pressure. the oxidizing process is limited by the diffu- sion of oxygen counterflow to the carbon monoxide that is formed on the cylindrical surface.