Answer:
The abundance of 35/17 Cl is 75% and 25% of 37/17Cl
Explanation:
The molar mass of an atom is defined as the sum of the masses of each isotope times its abundance, that is:
35.5amu = 35amu*X + 37amu*Y <em>(1)</em>
<em>Where X is the abundance of the 35/17Cl and Y the abundance of 37/17 Cl</em>
<em />
As there are just these 2 isotopes and the abundances of both isotopes = 1:
X + Y = 1 <em>(2)</em>
<em></em>
Replacing (2) in (1):
35.5 = 35X + 37(1-X)
35.5 = 35X + 37 - 37X
-1.5 = -2X
X = 0.75 = 75%
And Y = 100-75% = 25%
<h3>The abundance of 35/17 Cl is 75% and 25% of 37/17Cl</h3>
Answer:
Explanation:
It is possible to answer this question knowing Hess's law that says you can sum half-reactions enthalpy cahnge to obtain enthalpy change of the total reaction. Using the reactions:
<em>(1) </em>2NO(g) → N₂(g)+O₂(g) ΔH = -180,6 kJ
<em>(2) </em>N₂(g) + O₂(g) + Cl₂(g) → 2NOCl(g) ΔH = +103,4 kJ
The reverse reactions of (1) and (2) are:
<u>N₂(g)+O₂(g)</u> → 2NO(g) ΔH = +180,6 kJ
2NOCl(g) → <u>N₂(g) + O₂(g)</u> + Cl₂(g) ΔH = -103,4 kJ
The sum of these reactions is:
2NOCl(g) → 2NO(g) + Cl₂(g) ΔH = +180,6 kJ -103,4 kJ = <em>77,2 kJ</em>
<em />
I hope it helps!
Answer:
The approximate molar enthalpy of combustion of this substance is -66 kJ/mole.
Explanation:
First we have to calculate the heat gained by the calorimeter.
where,
q = Heat gained = ?
c = Specific heat = 
ΔT = The change in temperature = 3.08°C
Now put all the given values in the above formula, we get:
Now we have to calculate molar enthalpy of combustion of this substance :
where,
= enthalpy change = ?
q = heat gained = 8.2544kJ
n = number of moles methane = 
Therefore, the approximate molar enthalpy of combustion of this substance is -66 kJ/mole.
Answer:
B) Photosynthesis is the process in which light energy is transformed into food energy.
The narrator is a female
Hope this helps
