Equilibrium Constant Calculation and Naturally Occurring Potassium Isotopes
Equilibrium Constant Calculation
The equilibrium constant, K, for the reaction BaCl2 (aq) + K2SO4 (aq) â BaSO4 (s) + 2KCl (aq) can be calculated using the formula:
K = [BaSO4]*[2KCl]/[BaCl2]*[K2SO4}]
Plugging in the given mole values, we get:
K = [3.71 mol/L * (2*4.65 mol/L)] / (2.78 mol/L * 3.25 mol/L) = 8.24
Therefore, the equilibrium constant, K, for the reaction is 8.24 with 3 significant figures.
Naturally Occurring Potassium Isotopes
On Earth, naturally occurring potassium contains the isotopes 39K, 20K, and 41K. The following statements are true for a sample of naturally occurring potassium:
- A mole of naturally occurring potassium has a mass of 39.098 grams
- K-41 has 41 electrons
- All potassium isotopes have more neutrons than protons
- All potassium isotopes have an atomic number of 19
- Kâ39 is the most abundant potassium isotope
- A mole of K-39 atoms has a mass of 39.098 grams
- Potassium 41 has 19 protons and 22 neutrons
These characteristics define the composition and properties of naturally occurring potassium isotopes.