How many grams of potassium sulfide are produced from the reaction of 1.23 moles of potassium with sulfur?
Write the equation and balance it.
16K + S8 ==> 8K2S
Convert mols K to mols K2S.
1.23 mols K x (8 mol K2S/16 mols K) = ?? mols K2S.
To find out how many grams of potassium sulfide are produced, we need to use the balanced chemical equation for the reaction between potassium and sulfur to determine the mole ratio. The balanced chemical equation for this reaction is:
2 K + S -> K2S
From the balanced chemical equation, we can see that the mole ratio between potassium sulfide (K2S) and potassium (K) is 1:2. This means that for every 1 mole of potassium used, 2 moles of potassium sulfide will be produced.
First, let's determine the number of moles of potassium sulfide produced from the given number of moles of potassium.
Given:
Moles of potassium (K) = 1.23 mol
Using the mole ratio from the balanced equation:
Moles of potassium sulfide (K2S) = 2 * Moles of potassium (K)
= 2 * 1.23 mol
= 2.46 mol
Now, to find the grams of potassium sulfide produced, we need to use the molar mass of potassium sulfide (K2S). The molar mass of K2S can be calculated by adding the atomic masses of potassium (K) and sulfur (S):
Molar mass of K2S = (Atomic mass of K) * 2 + Atomic mass of S
= (39.10 g/mol) * 2 + 32.06 g/mol
= 78.20 g/mol + 32.06 g/mol
= 110.26 g/mol
Finally, we can calculate the grams of potassium sulfide produced:
Grams of potassium sulfide = Moles of potassium sulfide * Molar mass of K2S
= 2.46 mol * 110.26 g/mol
= 270.89 g
Therefore, 270.89 grams of potassium sulfide are produced from the reaction of 1.23 moles of potassium with sulfur.