What mass of potassium oxide is produced by the oxidation of 5 grams of potassium?
Here is an solved example of a stoichiometry problem. Just follow the steps.
http://www.jiskha.com/science/chemistry/stoichiometry.html
To determine the mass of potassium oxide produced by the oxidation of potassium, we need to balance the chemical equation for this reaction.
The balanced equation for the oxidation of potassium is as follows:
4K + O2 -> 2K2O
From the balanced equation, we can see that 4 moles of potassium (K) react with 1 mole of oxygen (O2) to produce 2 moles of potassium oxide (K2O).
First, we need to convert the mass of potassium (K) given in the question to moles. To do this, we use the molar mass of potassium, which is approximately 39.10 g/mol.
Number of moles of K = Mass of K / Molar mass of K
Number of moles of K = 5 g / 39.10 g/mol
Number of moles of K ≈ 0.128 moles
Now that we know the number of moles of potassium, we can calculate the number of moles of potassium oxide (K2O) using the stoichiometric ratio from the balanced equation.
According to the balanced equation, 4 moles of K react to produce 2 moles of K2O.
Number of moles of K2O = (Number of moles of K / 4) * 2
Number of moles of K2O = (0.128 moles / 4) * 2
Number of moles of K2O = 0.064 moles
Finally, we convert the moles of potassium oxide to grams using its molar mass. The molar mass of potassium oxide (K2O) is approximately 94.20 g/mol.
Mass of K2O = Number of moles of K2O * Molar mass of K2O
Mass of K2O = 0.064 moles * 94.20 g/mol
Mass of K2O ≈ 6.05 grams
Therefore, the mass of potassium oxide produced by the oxidation of 5 grams of potassium is approximately 6.05 grams.