Can someone help me with finding the unknown element in this problem? I seriously need help!!!?

Let y be the atomic mass of E.

Molar mass of O = 16.00 g/mol
Molar mass of Cl = 35.45 g/mol
Molar mass of E = y g/mol

No. of moles of EO₂ reacted = (3.1985 g) / [(y + 16.00×2) g/mol] = 3.1985/(y + 32.00) mol
No. of moles of ECl₃ produced = (5.0573 g) / (y + 35.45×3) g/mol = 5.0573/(y + 106.35) mol

1 mole of EO₂ (containing 1 mole of E) reacts with Cl₂ to give 1 mole of ECl₃ (containing 1 mole of E).
3.1985/(y + 32.00) = 5.0573/(y + 106.35)
5.0573 × (y + 32.00) = 3.1985 × (y + 106.35)
5.0573y + 161.8336 = 3.1985y + 340.160475
1.8588y = 178.326875
y = 95.94

The atomic mass of E is 95.94.
Refer to the Periodic Table. The atomic mass of Mo (molybdenum) is 95.94.
Hence, E is Mo (molybdenum).

do u go to ucsd i need help too #hoeger

Write a balanced equation:
2EO2 + 3Cl2 → 2ECl3 + 2O2
1mol EO2 will produce 1 mol ECl3
Mass O in 1 mol EO2 = 32g
Mass Cl in 1 mol ECl3 = 106.35g
Let the molar mass of E = X g/mol
Then :
(X+106.35) / ( X + 32) = 5.0573 / 3.1985
(X+ 106.35) / (X + 32) = 1.5811
X + 106.35 = 1.5811( X + 32)
X + 106.35 = 1.5811X + 50.5967
1.5811X – X = 106.35 – 50.5967
0.5811X = 55.7533
X = 55.7533/0.5811
X = 95.94g/mol
Check on periodic table:
E is molybdenum

Maybe Helium? Just a random guess