Answer:
Mass of original sample = 100 g
Explanation:
Half life of cesium-137 = 30.17 years
Where, k is rate constant
So,
The rate constant, k = 0.02297 year⁻¹
Time = 90.6 years
Using integrated rate law for first order kinetics as:
Where,
is the concentration at time t
is the initial concentration
Initial concentration
= ?
Final concentration
= 12.5 grams
Applying in the above equation, we get that:-
![[A_0]=\frac{12.5}{e^{-0.02297\times 90.6}}\ g=100\ g](https://tex.z-dn.net/?f=%5BA_0%5D%3D%5Cfrac%7B12.5%7D%7Be%5E%7B-0.02297%5Ctimes%2090.6%7D%7D%5C%20g%3D100%5C%20g)
<u>Mass of original sample = 100 g</u>
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<span>A-U-G - G-C-A
Met - Ala
If AUG is going to be in the beginning of the chain, </span>A-U-G, also will mean a start codon. For eukaryotes, codon for Met means start of the amino acid chain.
Answer:
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Explanation:
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Explanation:

where,
R = Gas constant = 
T = temperature = ![600^oC=[273.15+600]K=873.15 K](https://tex.z-dn.net/?f=600%5EoC%3D%5B273.15%2B600%5DK%3D873.15%20K)
= equilibrium constant at 600°C = 0.900
Putting values in above equation, we get:


The ΔG° of the reaction at 764.85 J/mol is 764.85 J/mol.
Equilibrium constant at 600°C = 
Equilibrium constant at 1000°C = 
![T_1=[273.15+600]K=873.15 K](https://tex.z-dn.net/?f=T_1%3D%5B273.15%2B600%5DK%3D873.15%20K)
![T_2=[273.15+1000]K=1273.15 K](https://tex.z-dn.net/?f=T_2%3D%5B273.15%2B1000%5DK%3D1273.15%20K)
![\ln \frac{K_2}{K_1}=\frac{\Delta H^o}{R}\times [\frac{1}{T_1}-\frac{1}{T_2}]](https://tex.z-dn.net/?f=%5Cln%20%5Cfrac%7BK_2%7D%7BK_1%7D%3D%5Cfrac%7B%5CDelta%20H%5Eo%7D%7BR%7D%5Ctimes%20%5B%5Cfrac%7B1%7D%7BT_1%7D-%5Cfrac%7B1%7D%7BT_2%7D%5D)
![\ln \frac{0.396}{0.900}=\frac{\Delta H^o}{8.314 J/mol K}\times [\frac{1}{873.15 K}-\frac{1}{1273.15 K}]](https://tex.z-dn.net/?f=%5Cln%20%5Cfrac%7B0.396%7D%7B0.900%7D%3D%5Cfrac%7B%5CDelta%20H%5Eo%7D%7B8.314%20J%2Fmol%20K%7D%5Ctimes%20%5B%5Cfrac%7B1%7D%7B873.15%20K%7D-%5Cfrac%7B1%7D%7B1273.15%20K%7D%5D)

The ΔH° of the reaction at 600 C is -18,969.30 J/mol.
ΔG° = ΔH° - TΔS°
764.85 J/mol = -18,969.30 J/mol - 873.15 K × ΔS°
ΔS° = -22.60 J/K mol
The ΔS° of the reaction at 600 C is -22.60 J/K mol.

Partial pressure of carbon dioxide = 
Partial pressure of carbon monoxide = 
Where
mole fraction of carbon dioxide and carbon monoxide gas.
The expression of
is given by:








Mole fraction of carbon dioxide at 600°C is 0.474.