For the balanced chemical reaction below: P4O10 (g) + 6 H2O (l) → 4 H3PO4 (aq)...
For the balanced chemical reaction below:
P4O10 (g) + 6 H2O (l) → 4 H3PO4 (aq)
(a) Calculate the moles of water if there are 9.19 grams of tetraphosphorus decoxide.
(b) Calculate the grams of water if there are 0.730 moles of tetraphosphorus decoxide.
(c) Calculate the grams of tetraphosphorus decoxide if there are 5.41 grams of H3PO4.
(d) Calculate the moles of H3PO4 if there are 0.604 moles of tetraphosphorus decoxide.
I am really just unsure how to set up the formula.
Homework Answers
a) molar mass of P4O10 = 283.889
gm/mol
moles of P4O10 = 9.19 gms
/ 283.889 gm/mol = 0.032371 mol of
P4O10
moles of water = 6*0.032371 = 0.19423 mol of
H2O
b) mol of P4O10 = 0.730 mol
moles of water = 6 * 0.730 = 4.38 moles of
H2O
grams of water = 4.38 mol of H2O * 18
gm/mol = 78.84 gm of H2O
c) molar mass of H3PO4 = 98 gm/mol
mol of H3PO4 = 5.41 gm / 98
gm/mol = 0.055204 mol
moles of P4O10 required =
(0.055204 mol / 4) *1 = 0.013801mol
grams of P4O10 required =
0.013801mol * 283.889 gm/mol = 3.91795 gms of
P4O10
d) moles of H3PO4 = 4*0.604 mol of
P4O10 = 2.416 mol of
H3PO4
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