1No Spac. Heading 1 Heading 2 Title Subtitle Subtle Em... Emphasis Intense E Sty

Question

1No Spac. Heading 1 Heading 2 Title Subtitle Subtle Em... Emphasis Intense E Styles Which relationship regarding the quantities of reactants and products associated with the following reaction is NOT correct? Please provide an explanation 6H20(C) + P010 (s) 4 HPO(ag) 6 molecules +1 molecule 4 molecules 18mol + 6 mol 12mol 324 g + 852 g 1176 g d.6xmol+x mol4rmol e, y(27 g) + y(71 g) y(98 g) A uranium oxide compound is found to be 88.15% U by mass, what is the empirical formula for the compound? Please provide an explanation.

Explanation / Answer

6H2O + P4O10 = 4 H3PO4

Molecule or mole ratio is 6:1:4

6 molecules + 1 molecule = 4 molecules

C

6x mole + x mole = 4 x mole

This is correct because Molecule or mole ratio is 6:1:4

18 mole + 6 mole --- > 12 mole

3:1:2

This is wrong because molar ratio is wrong.

Y (27 g) + y (71 g)   ---- > y(98 g)

H2O = 27/18=1.5

P4O10 = 71 /283.88= 0.25

H3PO4= 98 / 97.9952= 1.00

THEN; 1.5 : 0.25 :1.00 = 6:1:4

6H2O + P4O10 = 4 H3PO4

This is correct because Molecule or mole ratio is 6:1:4

324 g +852 g= 1176 g

Molar mass of P4O10 = 283.889044 g/mol

Molar mass of H3PO4 is 97.9952 g/mol

Molar mass of H2O is 18.02 g/mol

6H2O + P4O10 = 4 H3PO4

H2O = 324/18=18

P4O10 = 852 /283.88= 3

H3PO4= 1176 / 97.9952= 12

THEN; 18:3:12= 6:1:4

6H2O + P4O10 = 4 H3PO4

This is correct because Molecule or mole ratio is 6:1:4

2.

Given that U = 88.15 %

The O = 100-88.15 = 11.85 %

Assume that the amount of oxide is 100 g, then U = 88.15 g

O = 11.85 g

Mole of U = 88.15 g / 238.0289 g/ mole= 0.370 mole

Mole of O = 11.85 g /15.99 g/ mole= 0.741 mole

Molar ratio in the oxide

U = 0.370 /0.370 = 1

O = 0.741/0.370= 2

Thus the empirical formula of uranium oxide is UO2.

Related Questions

Navigate

• Browse (All)
• Browse 1
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.