3. Beryllium Chloride reacts with potassium Nitrate to yield Beryllium Nitrate and Potassium Chloride
A Wite balanced chemical formula equation for this reaction

What type of reaction is this?

c. 71.2 grams of Beryllium Chloride is reacted with 161 grams of
Potassium Nitrate, identify the limiting and excess rentants

D. How many grams of the excess reactant romains when the
reaction is complete?
E. If the actual yield of Potassium Chloride produced is 105g what is
the percent yield?

n2(g) + 3h2-> 2nh3(g)   this is the balanced equation

note the mole ratio between n2, h2 and nh3.   it is 1 : 3 : 2   this will be important.

moles n2 present = 28.0 g n2 x 1 mole n2/28 g = 1 mole n2 present

moles h2 present = 25.0 g h2 x 1 mole h2/2 g = 12.5 moles h2 present

based on mole ratio, n2 is limiting in this situation because there is more than enough h2 but not enough n2.

moles nh3 that can be produced = 1 mole n2 x 2 moles nh3/mole n2 = 2 moles nh3 can be produced

grams of nh3 that can be produced = 2 moles nh3 x 17 g/mole = 34 grams of nh3 can be produced

note:   the key to this problem is recognizing that n2 is limiting, and therefore limits how much nh3 can be produced.

they are both synthetic elements

explanation:

d