Answer:
2.35 *10^2 g
Explanation:
4.2 mol Fe *55.845 g/1 mol = 234.549 > 2.35 *10^2 g
Answer:
6.82 moles of Fe2O3
Explanation:
Step 1:
Determination of the number of mole of in 450g of CO2.
This is illustrated below:
Molar Mass of CO2 = 12 + (2x16) = 44g/mol
Mass of CO2 = 450g
Number of mole of CO2 =.?
Number of mole = Mass/Molar Mass
Number of mole of CO2 = 450/44 = 10.23 moles
Step 2:
Determination of the number of mole of Fe2O3 needed for the reaction. This is illustrated below:
2Fe2O3 + 3C—> 4Fe + 3CO2
From the balanced equation above,
2 moles of Fe2O3 reacted to produce 3 moles of CO2.
Therefore, Xmol of Fe2O3 will react to produce 10.23 moles of CO2 i.e
Xmol of Fe2O3 = (2x10.23)/3
Xmol of Fe2O3 = 6.82 moles
Therefore, 6.82 moles of Fe2O3 is required.
what is the question ? I don't see any question but a few words
Ideal gasses (ideal gas law)
This tells us that an atom of sodium contains 11 electrons which is balanced by 11 protons. The atomic mass of the atom is then the sum of the protons and neutrons. If you know the atomic mass of sodium, you can subtract 11 (protons) to get the number of neutrons.
