<u>Answer:</u> The fractional abundance of Ir-191 is 0.372
<u>Explanation:</u>
Average atomic mass of an element is defined as the sum of masses of each isotope each multiplied by their natural fractional abundance.
Formula used to calculate average atomic mass follows:
.....(1)
Let the fractional abundance of Ir-191 be x and that of Ir-193 isotope be (1-x)
<u>For isotope 1 (Ir-191):</u>
Mass of isotope 1 = 190.96058 amu
Fractional abundance of Ir-191 = x
<u>For isotope 1 (Ir-193):</u>
Mass of isotope 1 = 192.96292 amu
Fractional abundance of Ir-193 = (1 - x)
Average atomic mass of iridium = 192.217 amu
Putting values in equation 1, we get:
![192.217=[(190.96058\times x)+(192.96292\times (1-x))]\\\\x=0.372](https://tex.z-dn.net/?f=192.217%3D%5B%28190.96058%5Ctimes%20x%29%2B%28192.96292%5Ctimes%20%281-x%29%29%5D%5C%5C%5C%5Cx%3D0.372)
Hence, the fractional abundance of Ir-191 is 0.372
I believe it is d. scientific law
Answer:
0,051g of O₂
Explanation:
The reaction of precipitation of Fe is:
4Fe(OH)⁺(aq) + 4OH⁻(aq) + O₂(g) + 2H₂O(l) → 4Fe(OH)₃(s)
<em>-Where the Fe(OH)⁺ is Fe(II) and Fe(OH)₃ is Fe(III)-</em>
This reaction is showing you need 1 mol of O₂(g) per 4 moles of Fe(II) for a complete reaction.
85mL= 0,085L of 0,075M Fe(II) are:
0,085L*0,075M = 6,34x10⁻³ moles of Fe(II)
For a complete reaction of 6,34x10⁻³ moles of Fe(II) you need:
6,34x10⁻³ moles of Fe(II)×
=
1.59x10⁻³ moles of O₂. In grams:
1.59x10⁻³ moles of O₂×
= <em>0,051g of O₂</em>
<em></em>
I hope it helps!
Answer:
The system makes the transition from nonspontaneous to spontaneous at a temperature of 954.7 K.
Under 954.7 K the reaction is nonspontaneous; more than 954.7 K is the reaction spontaneous.
Explanation:
CH4(g) + 2H2O(g) ⇆ CO2(g) + 4H2(g)
CH4(g) H2O(g) CO2(g) H2(g) ΔH°f (kJ/mol): –74.87 –241.8 –393.5 0
ΔG°f (kJ/mol): –50.81 –228.6 –394.4 0
S°(J/K·mol): 186.1 188.8 213.7 130.7
ΔG<0 to be spontaneous
ΔG = ΔH- TΔS <0
ΔH = ∑nΔH(products) - ∑nΔH(reactant)
ΔH = (-393.5) - (–74.87 + 2*–241.8)
ΔH = 164.97 kJ = 164970 J
ΔS = ∑nΔS(products) - ∑nΔS(reactant)
ΔS = (213.7 + 4*130.7) - (186.1 + 2*188.8)
ΔS = 172.8 J
0 > 164970 J - T* 172.8 J
-164970 J > - T* 172.8 J
954.7< T
The system makes the transition from nonspontaneous to spontaneous at a temperature of 954.7 K.
Under 954.7 K the reaction is nonspontaneous; more than 954.7 K is the reaction spontaneous.
it’s C
i hope i help you but if not DO NOT FORGET STAY SAFE AT HOME