how do i calculate the number of potassium ions present in a 16.42 gram sample of k3p?

Answer 1

Calculate the molar mass of potassium phosphide

3 mol K * 39.10 g / mol = 117.3 g
1 mol P * 30.97 g / mol = 30.97 g
148.27 g / mol K3P

Calculate the number of moles in 16.42 g K3P

16.42 g * 1 mol/148.27 g = .111 mol K3P

Convert from moles of pottassium phosphide to moles of pottassium

(.111 mol K3P) * (3 mol K)/(1 mol K3P) = .333 mol K

Convert from moles of pottassium to atoms by multiplying by Avagadros number

.333 mol K * 6.022 X 10^23 atoms/1mol = 2.01 X 10^23 atoms K

Hope this helps!

Answer 2

if you mean Potassium phosphide then to calculate the number of potassium ions just do the following
16.42 grams of K3P is how many moles?
K = 39.10g x 3 = 117.3
P= 30.97
so 117.3 + 30.97 = 148.27g per mol
but you have 16.42 so to find the number of moles you have divided actual grams by the molar mass
16.42/148.27 = 0.111mol in your sample
so then do 0.111 times avogado's number to find out how many atoms you have in the entire sample
0.111 X 6.023 X10^23 = 6.685 x 10^22 atoms
now mulitple it by 3/4 since you have 3 K to one P.
6.685 X 10^22 times 3/4 = 5.01375 X 10^22 atoms of Potassium

Answer 3

first you find out how many moles of potassium are present and then you multiply the number of moles by Avogadro's number (6.02 *10^23). this will give you the number of ions.