Hey There!
p-aminophenol (109.13 g/mol) + Ac2O (102.09 g/mol) ---> acetominophen (151.16 g/mol)
next, since you already know your limiting reactant (p-aminophenol), convert it to mols :
0.130 g / (109.13 g/mol) = 0.00119 moles
now that's your theoretical max, since its a 1:1 mol ratio, so multiply by the new molecular weight. :
0.00119 * 151.16 = 0.180 g
Hope that helps!
Answer is: 15.30 kilojoules of heat are needed to completely vaporize C₄H₁₀<span>.
m(</span>C₄H₁₀) = 42.8 g.
M(C₄H₁₀) = 74.12 g/mol.
n(C₄H₁₀) = m(C₄H₁₀) ÷ M(C₄H₁₀).
n(C₄H₁₀) = 42.8 g ÷ 74.12 g/mol.
n(C₄H₁₀) = 0.577 mol.
Q = n(C₄H₁₀) · ΔHvap.
<span>Q = 0.577 mol </span>· 26.5 kJ/mol.
<span>Q = 15.30 kJ, heat of butane.
</span>
Answer:
Im pretty sure it is B. Earths temperature
Explanation:
Hello there!
1. Synthesis: 2H₂ + O₂ → 2H₂O
2. Decomposition: 2HBr → H₂ + Br₂
3. Single-Replacement: 2Al + 3H₂SO₄ → 3H₂ + Al₂(SO₄)₃
4. Double-Replacement: 2HCl + 2NaOH → 2H₂O + 2NaCl
5. Combustion: 2C₂H₆ + 7O₂ → 6H₂O + 4CO₂
I hope this helps!
Brady
