This isn’t really a school related question. but can you workout with a belly piercing?
2 answers:
You might be interested in
Answer:
Chloroform is expected to boil at 333 K (60 ).
Explanation:
For liquid-vapor equilibrium at 1 atm, = 0.
We know, , where T is temperature in kelvin scale.
Here both and
are corresponding to vaporization process therefore T represents boiling point of chloroform.
So,
or, T = 333 K
So, at 333 K (60 ) , chloroform is expected to boil.
Answer: 1) Endothermic
2) Yes, absorbed.
3) 166.86 kJ will be absorbed.
Explanation:
1) To determine if a reaction is endothermic (heat is absorbed by the system) or exothermic (heat is released by the system), first calculate its change in Enthalpy, which is given by:
ΔH =
For the reaction 2Fe₂O₃(s) ⇒ 4FeO(s) + O₂(g):
<u />
<u>Enthalpy of Reagent (</u>Fe₂O₃(s)<u>)</u>
Enthalpy of formation for Fe₂O₃(s) is - 822.2 kJ/mol
The reaction needs 2 mols of the molecule, so:
H = 2(-822.2)
H = - 1644.4
<u />
<u>Enthalpy of Products (</u>4FeO(s) + O₂(g<u>))</u>
Enthalpy of formation of O₂ is 0, because it is in its standard state.
Enthalpy of formation of FeO is - 272.04 kJ/mol
The reaction produces 4 mols of iron oxide, so:
H = 4(-272.04)
H = -1088.16
<u>Change in Enthalpy</u>:
ΔH =
ΔH = - 1088.16 - (-1644.4)
ΔH = + 556.2 kJ/mol
The change in enthalpy is positive, which means that the reaction is absorving heat. Then, the chemical reaction is Endothermic.
2) When Fe₂O₃(s) reacts, heat is absorbed because it is an endothermic reaction.
3) Calculate how many mols there is in 94.2 g of Fe₂O₃(s):
n =
n =
n = 0.6 mols
In the reaction, for 2 mols of Fe₂O₃(s), 556.2 kJ are absorbed. Then:
2 mols --------------- 556.2 kJ
0.6 mols ------------- x
x =
x = 167 kJ
It will be absorbed 167 kJ of energy, when 94.2 g of Fe₂O₃(s) reacts.