To answer this question, we need to know the molar masses of potassium (K) and oxygen (O).
The molar mass of potassium is approximately 39.10 g/mol.
The molar mass of oxygen is approximately 16.00 g/mol.
According to the law of conservation of mass, the mass of the reactants (potassium and oxygen) should be equal to the mass of the products (potassium oxide).
To find out how many grams of potassium oxide will be produced, we need to determine the limiting reactant. We can do this by converting the masses of potassium and oxygen to moles.
Moles of potassium (K):
2g K * (1 mol K / 39.10 g K) = 0.051 mol K
Moles of oxygen (O):
5g O * (1 mol O / 16.00 g O) = 0.313 mol O
Based on the balanced equation, the mole ratio between potassium and oxygen in the reaction is 4:1. Therefore, we can see that the 0.051 mol of potassium would require 0.051 mol O * (1 mol K / 4 mol O) = 0.013 mol K.
Since we have more moles of oxygen (0.313 mol) than the stoichiometric requirement for 0.051 moles of potassium (0.013 mol), oxygen is in excess and potassium is the limiting reactant.
Now, let's calculate the moles of potassium oxide produced.
Moles of potassium oxide (K2O):
0.051 mol K * (1 mol K2O / 2 mol K) = 0.0255 mol K2O
Finally, we can convert the moles of potassium oxide to grams.
Mass of potassium oxide:
0.0255 mol K2O * (94.20 g K2O / 1 mol K2O) = 2.40 g K2O
Therefore, according to the law of conservation of mass, 2 grams of potassium would react with 5 grams of oxygen to produce 2.40 grams of potassium oxide.
2 G of potassium would reacts with 5 G of oxygen according to the law of conservation of mass how many grams of potassium oxide will be produced
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