Answer:
see explanation
Explanation:
To determine limiting reactant divide mole quantities of reactants by the respective coefficient in the balanced equation. The smaller value is the limiting reactant.
P₄ + 5O₂ => 2P₂O₅
12/1 = 12 15/5 = 3
O₂ is the limiting reactant. P₄ will be in excess when rxn stops.
Answer:
Umm i dont know but i think atomic nucleus
Explanation:
Answer:
All are correct
Explanation:
This might be a little deceptive. The question shows H, O and N which would designate ELEMENTS.
However, all of these can also be considered compounds and molecules as well. BUT, they are H₂, O₂ and N₂ when they are molecules and compounds.
So it depends on the whether the question is being literal or not.
Ksp for FeCO₃ is 3.07 x 10⁻¹¹
Ksp for MgCO₃ is 6.82 x 10⁻⁶
So Fe²⁺ will precipitated first as solubility product of FeCO₃ is lower than solubility product of MgCO₃
Ksp FeCO₃ = [Fe²⁺][CO₃²⁻]
3.07 x 10⁻¹¹ = (2.3 x 10⁻²) [CO₃²⁻]
[CO₃²⁻] = 1.33 x 10⁻⁹ M to precipitate Fe²⁺ ions
Ksp MgCO₃ = [Mg²⁺][CO₃²⁻]
6.82 x 10⁻⁶ = (2.0 x 10⁻²) [CO₃²⁻]
[CO₃²⁻] = 3.4 x 10⁻⁴ M to precipitate the Mg²⁺ ions
Ksp FeCO₃ = [Fe²⁺][CO₃²⁻]
3.07 x 10⁻¹¹ = [Fe²⁺] (3.4 x 10⁻⁴)
[Fe²⁺] = 9 x 10⁻⁸ M when Mg²⁺ ions precipitate
To predict the theoretical yield we would have to know the amount we of product we actually produced in a reaction, and the amount that should have been produced based on calculations involving the balanced equation for the reaction.
For instance, suppose we made water from hydrogen and oxygen. Starting with 2 moles of hydrogen and 1 mole of oxygen we should produce 2 moles of water (or 36 gram). But suppose we actually ran the reaction in the lab and collected only 34g of water.
The percent yield would be 34g / 36g x 100 =94.4%
So, if I'm reading your question correctly, 20g is the experimental yield and 10% is the percent yield.
Plugging in gives us 10/100 = 20/x
The theoretical yield must be 200g.
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I HOPE THAT HELP MY FRIEND :)
