<h3>Answer:</h3>
Molecular Formula = S₂O₂ (Disulfur Dioxide)
<h3>Solution:</h3>
Molecular formula is calculated by using following formula,
Molecular Formula = n × Empirical Formula ---- (1)
Also, n is given as,
n = Molecular Weight / Empirical Formula Weight
Molecular Weight = 96.13 g.mol⁻¹
Empirical Formula Weight = 32.06 (S) + 16.0 (O) = 48.06 g.mol⁻¹
So,
n = 96.13 g.mol⁻¹ ÷ 48.06 g.mol⁻¹
n = 2.0002 ≈ 2
Putting Empirical Formula and value of "n" in equation 1,
Molecular Formula = 2 × SO
Molecular Formula = S₂O₂ (Disulfur Dioxide)
Answer:
Q:
What volume will 3.50 mol of Xe gas occupy at STP?
A:
78.4 L
Explanation:
Bond energy is basically how much energy it takes to break that molecule apart. The main things that affect bond energy is electronegativity and the number of bonds. I believe the correct answer is C=O. It <span>has the greatest bond energy, because it is harder to break apart a double bond than a single bond.</span>
