Answer:
? the question isn't clear
Explanation:
Answer: it has full valence shells
Explanation: Hope this is it
One mole Hydrogen need 1/2mol O_2 .
Moles of Hydrogen
Moles of O_2
Answer:
The activation energy for this reaction = 23 kJ/mol.
Explanation:
Using the expression,
![\ln \dfrac{k_{1}}{k_{2}} =-\dfrac{E_{a}}{R} \left (\dfrac{1}{T_1}-\dfrac{1}{T_2} \right )](https://tex.z-dn.net/?f=%5Cln%20%5Cdfrac%7Bk_%7B1%7D%7D%7Bk_%7B2%7D%7D%20%3D-%5Cdfrac%7BE_%7Ba%7D%7D%7BR%7D%20%5Cleft%20%28%5Cdfrac%7B1%7D%7BT_1%7D-%5Cdfrac%7B1%7D%7BT_2%7D%20%5Cright%20%29)
Where,
![k_1\ is\ the\ rate\ constant\ at\ T_1](https://tex.z-dn.net/?f=k_1%5C%20is%5C%20the%5C%20rate%5C%20constant%5C%20at%5C%20T_1)
![k_2\ is\ the\ rate\ constant\ at\ T_2](https://tex.z-dn.net/?f=k_2%5C%20is%5C%20the%5C%20rate%5C%20constant%5C%20at%5C%20T_2)
is the activation energy
R is Gas constant having value = 8.314×10⁻³ kJ / K mol
![k_2=2.3\times 10^8](https://tex.z-dn.net/?f=k_2%3D2.3%5Ctimes%2010%5E8)
The conversion of T( °C) to T(K) is shown below:
T(K) = T( °C) + 273.15
So,
T = (280 + 273.15) K = 553.15 K
The conversion of T( °C) to T(K) is shown below:
T(K) = T( °C) + 273.15
So,
T = (376 + 273.15) K = 649.15 K
So,
![\left(\ln \left(\:\frac{4.8\times \:\:\:10^8}{2.3\times \:\:\:10^8}\right)\right)\:=-\frac{E_a}{8.314\times \:10^{-3}\ kJ/mol.K}\times \:\left(\frac{1}{649.15\ K}-\frac{1}{553.15\ K}\right)](https://tex.z-dn.net/?f=%5Cleft%28%5Cln%20%5Cleft%28%5C%3A%5Cfrac%7B4.8%5Ctimes%20%5C%3A%5C%3A%5C%3A10%5E8%7D%7B2.3%5Ctimes%20%5C%3A%5C%3A%5C%3A10%5E8%7D%5Cright%29%5Cright%29%5C%3A%3D-%5Cfrac%7BE_a%7D%7B8.314%5Ctimes%20%5C%3A10%5E%7B-3%7D%5C%20kJ%2Fmol.K%7D%5Ctimes%20%5C%3A%5Cleft%28%5Cfrac%7B1%7D%7B649.15%5C%20K%7D-%5Cfrac%7B1%7D%7B553.15%5C%20K%7D%5Cright%29)
![E_a=-\frac{10^{-3}\times \:8.314\ln \left(\frac{10^8\times \:4.8}{10^8\times \:2.3}\right)}{-\frac{96}{359077.3225}}\ kJ/mol](https://tex.z-dn.net/?f=E_a%3D-%5Cfrac%7B10%5E%7B-3%7D%5Ctimes%20%5C%3A8.314%5Cln%20%5Cleft%28%5Cfrac%7B10%5E8%5Ctimes%20%5C%3A4.8%7D%7B10%5E8%5Ctimes%20%5C%3A2.3%7D%5Cright%29%7D%7B-%5Cfrac%7B96%7D%7B359077.3225%7D%7D%5C%20kJ%2Fmol)
![E_a=-\frac{\frac{8.314\ln \left(\frac{4.8}{2.3}\right)}{1000}}{-\frac{96}{359077.3225}}\ kJ/mol](https://tex.z-dn.net/?f=E_a%3D-%5Cfrac%7B%5Cfrac%7B8.314%5Cln%20%5Cleft%28%5Cfrac%7B4.8%7D%7B2.3%7D%5Cright%29%7D%7B1000%7D%7D%7B-%5Cfrac%7B96%7D%7B359077.3225%7D%7D%5C%20kJ%2Fmol)
![E_a=22.87\ kJ/mol](https://tex.z-dn.net/?f=E_a%3D22.87%5C%20kJ%2Fmol)
<u>The activation energy for this reaction = 23 kJ/mol.</u>