a) 7.08g b) 55.5%
First, we set up the equation for the reaction.
Then we must balance it to get the correct molar ratios:
Next, we calculate the molar quantities in the actual reaction.
2.20g/31g/mole P = 0.071 mole
Our balanced reaction shows that we need 10 moles of
Because our balanced reaction shows that every 10 moles of
Converting that value back into grams gives us 0.034 mol x 208.25g/mol = 7.08g
If for part b) you mean only 3.93g are actually produced, the yield of the reaction is: (actual/theoretical) x 100 = % 3.93/7.08 x 100 =55.5%