Which law of chemical combination is illustrated by the fact that 168g fe reacts to from 232g Fe3 O4 and 8gH2
Plz give me the answer as am struck last to submit my assignment plz plzhelp me
The law of chemical combination that is illustrated by the fact you mentioned is the law of definite proportions.
The law of definite proportions states that a given compound always contains the same elements in the same proportion by mass. In other words, the chemical formula of a compound provides the ratio of the elements' masses in that compound.
To calculate the answer, we need to determine the ratio of the masses of Fe to Fe3O4 and H2. Here's how to do it:
1. Convert the given masses to moles using the molar mass of each element:
- Molar mass of Fe = 55.85 g/mol
- Moles of Fe = 168 g / 55.85 g/mol = 3.01 mol
- Molar mass of Fe3O4 = (3 x 55.85) g/mol + (4 x 16) g/mol = 231.52 g/mol
- Moles of Fe3O4 = 232 g / 231.52 g/mol = 1.00 mol
- Molar mass of H2 = 2 g/mol
- Moles of H2 = 8 g / 2 g/mol = 4.00 mol
2. Use the moles of Fe as a reference to find the ratio with Fe3O4 and H2:
- From the given equation, the balanced equation is: 4Fe + 3O2 → 2Fe2O3 (in which Fe2O3 is equivalent to Fe3O4)
- The ratio between Fe and Fe3O4 is 4:2 (or simplified: 2:1)
- The ratio between Fe and H2 is 4:4 (or simplified: 1:1)
In conclusion, based on the law of definite proportions, for every 168g of Fe reacting, you will form 232g of Fe3O4 and 8g of H2.