To solve this problem, we first need to calculate the molar mass of potassium oxide (K2O):
Molar mass of K2O = (2 x molar mass of K) + molar mass of O
Molar mass of K2O = (2 x 39 g/mol) + 16 g/mol
Molar mass of K2O = 78 g/mol + 16 g/mol
Molar mass of K2O = 94 g/mol
Now we can calculate the moles of K2O produced from 23.5 grams:
moles = mass / molar mass
moles = 23.5 g / 94 g/mol
moles = 0.25 mol
Since the balanced chemical equation shows that 4 moles of potassium are needed to produce 2 moles of K2O, we can calculate the moles of potassium needed:
moles of K = (4 moles of K / 2 moles of K2O) x moles of K2O
moles of K = (4 / 2) x 0.25 mol
moles of K = 0.5 mol
Finally, we can calculate the grams of potassium needed:
mass = moles x molar mass
mass = 0.5 mol x 39 g/mol
mass = 19.5 g
Therefore, 19.5 grams of potassium are needed in the reaction to produce 23.5 grams of potassium oxide (K2O). So the answer is 19.5 g.
Use the chemical equation to answer the question. 4K(s) + O2(g) → 2K2O(s) The molar mass of potassium (K) is 39 g/mol. The molar mass of oxygen (O) is 16 g/mol. How many grams of potassium are needed in the reaction to produce 23.5 grams of potassium oxide (K2O)? (1 point) Responses 23.5 g 23.5 g 19.5 g 19.5 g 9.75 g 9.75 g 0.50 g
1 answer