calculate moles of both reagents given and the moles of FeS that each of them would form if they were in excess
moles = mass / molar mass
moles Fe = 7.62 g / 55.85 g/mol
= 0.1364 moles
1 mole Fe produces 1 mole FeS
Therefore 7.62 g Fe can form 0.1364 moles FeS
moles S = 8.67 g / 32.07 g/mol
= 0.2703 moles S
1 mole S can from 1 moles FeS
So 8.67 g S can produce 0.2703 moles FeS
The limiting reagent is the one that produces the least product. So Fe is limiting.
The maximum amount of FeS possible is from complete reaction of all the limiting reagent.
We have already determined that the Fe can form up to 0.1364 moles of FeS, so this is max amount of FeS you can get.
Convert to mass
hope this helps :)
The statements that are actually correct among the given options are:
<span>Valence electrons are transferred to the oxygen atom.
</span>The bond length <span>is less than the sum of the two atomic radii.
</span><span>Bonding electrons are stationary in the CO molecule
</span>So the correct option among all the options that are given in the question is the fourth option or option "D".
Photosynthesis in green plants during which CO2 is absorbed to form glucose
Answer:
2Al (s) + 6HCl (aq) → 2 AlCl3 (aq) + 3H2 (g)↑
Explanation:
- We can put an up arrow to H2 cause as it is a gas, it can be released to the atmosphere.
- Aluminum as metal must be solid.
- As we have two solutions, both are aqueous phase.
- The stoichiometry must match on both sides of the reaction to have the same amount of elements of each compound.}
Reactants : 2 Aluminun
6 Hydrogen
6 Chloride
Products:
2 Aluminun
2.3 = 6 Chloride
3.2 = 6 Hydrogen
I believe it has something to do with the H2O molecules, because a chemical compound is not a mixture.
