When the balanced reaction equation is:
P4O10 + 6H2O→ 4 H3PO4
when we have the mass of P4O10 = 10 g and the molar mass of P4O10=284 g/mol & we have the molar mass of H3PO4 =98 g/mol so we can get the mass of H3PO4 by substitution by:
mass of H3PO4 = (mass of P4O10)/(molar mass of P4O10) * 4(mol of H3PO4)*molar mass of H3PO4
∴mass of H3PO4 = (10 / 284) * 4 * 98 = 13.8 g
No, 0.49 is greater than 0.72
Answer:
SO₄(aq) + Ba(aq) + ----> BaSO₄(s)
Explanation:
(aq) will always become 2 ions
balancing the equation
Na₂SO₄(aq) + BaCl₂(aq) ----> BaSO₄ + 2NaCl
note how there is the same amount of each element on both sides except for Na and Cl. the left side has 2 times the amount of the right side. All I needed to do to balance was add the 2 coefficient to NaCl product on right side since Na and Cl are together and not in separate compounds.
now rewriting (NaCl is aq since all compounds with Na are aqueous)
barium sulfate is the solid formed
rewriting the equation: (subscripts of single elements become coefficients, polyatomic subscripts stay)
2Na(aq) + SO₄(aq) + Ba(aq) + 2Cl(aq) ----> BaSO₄(s) + 2Na(aq) + 2Cl(aq)
net ionic: removing any substance seen on both sides
SO₄(aq) + Ba(aq) + ----> BaSO₄(s)