The answer is 236.5 J/K
According to Δ G formula:
ΔG = ΔH - TΔS
when ΔG is the change in free energy (KJ)
and ΔH is the change in enthalpy (KJ)= ΔHvap * moles
= 71.8 KJ/mol * 1.11 mol
= 79.7 KJ
and T is the absolute temperature (K)= 64 °C + 273°C = 337 K
Δ S is the change in entropy KJ/K
by substitution:
when at equilibrium ΔG = 0
∴ΔS = ΔH / T
=79.7 KJ/ 337 K
= 0.2365 KJ/K
= 236.5 J/K
D. photons it contains light but with zero mass
Answer:
C₆H₈O₆
Explanation:
First off, the<u> percent of oxygen by mass</u> of vitamin C is:
- 100 - (40.9+4.58) = 54.52 %
<em>Assume we have one mol of vitamin C</em>. Then we would have <em>180 grams</em>, of which:
- 180 * 40.9/100 = 73.62 grams are of Carbon
- 180 * 4.58/100 = 8.224 grams are of Hydrogen
- 180 * 54.52/100 = 98.136 grams are of Oxygen
Now we <u>convert each of those masses to moles</u>, using the <em>elements' respective atomic mass</em>:
- C ⇒ 73.62 g ÷ 12 g/mol = 6.135 mol C ≅ 6 mol C
- H ⇒ 8.224 g ÷ 1 g/mol = 8.224 mol H ≅ 8 mol H
- O ⇒ 98.136 g ÷ 16 g/mol = 6.134 mol O ≅ 6 mol O
So the molecular formula for vitamin C is C₆H₈O₆
The answer would be D. because when an acid and base mix the start to cancel each other out causing it to neutralize
A) The limiting reactant is Al
b) Br2 is the excess reactant
c) The amount moles of AlBr3 that get produced will be equal to the number of moles of Al to begin with.
d) 0
