<span> A compound <span>lens microscope. </span></span>
Answer:
it drifts through the atmosphere and the vapor absorbs heat then the warm air rises up therefore leaving the planet's surface and releasing the heat back into the upper part of the atmosphere
Answer:
The molecular formula is SO2F2
Explanation:
Step 1: Data given
Suppose the mass of compound = 100 grams
The compound contains:
31.42 % S = 31.42 grams S
31.35 % O = 31.35 grams O
100 - 31.42 - 31.35 = 37.23 F
Molar mass of S = 32.065 g/mol
Molar mass F = 19.00 g/mol
Molar mass O = 16.00 g/mol
Step 2: Calculate moles
Moles = mass / molar mass
Moles S = 31.42 grams / 32.065 g/mol
Moles S = 0.9799 moles
Moles 0 = 31.35 grams / 16.00 g/mol
Moles 0 = 1.959 moles
Moles F = 37.23 grams / 19.00 g/mol
Moles F = 1.959 moles
Step 3: Calculate mol ratio
We divide by the smallest amount of moles
S: 0.9799 / 0.9799 = 1
F: 1.959/ 0.9799 = 2
O : 1.959 / 0.9799 = 2
The empirical formula is SO2F2
This formula has a molecular mass of 102.06 g/mol
This means the empirical formula is also the molecular formula : SO2F2
Answer is: C₃H₃N₃O₃.
Chemical reaction: CₓHₓNₓOₓ + O₂ → aCO₂ + x/2H₂ + x/2N₂.
m(CₐHₓNₓ) = 5,214 g.
m(CO₂) = 5,34 g.
m(H₂) = 1,09 g.
m(N₂) = 1,70 g.
n(CO₂) = n(C) = 5,34 g ÷ 44 g/mol = 0,121 mol.
n(H₂O) = 1,09 g ÷18 g/mol = 0,06 mol.
n(H) = 2 · 0,0605 mol = 0,121 mol.
n(N₂) = 1,7 g ÷ 28 g/mol = 0,0607 mol.
n(N) = 0,0607 mol · 2 = 0,121 mol.
n(C) : n(H) : n(N) = 0,121 mol : 0,121 mol : 0,121 mol /: 0,121
n(C) : n(H) : n(N) = 1 : 1 : 1.
M(CHN) = 27 g/mol.
m(O₂) = 8,13 g - 5,214 g = 2,914 g.
n(O₂) = 2,914 g ÷ 32 g/mol = 0,09 mol.
n(CₓHₓNₓOₓ) = 5,214 g ÷ 129,1 g/mol = 0,0404 mol.
n(CₓHₓNₓOₓ) : n(CO₂) = 1 : 3.
