Answer:
answer of first question is <u>Chlorine</u>
answer of second question is <u>Group </u><u>1</u><u>4</u>
<h3>
<u>PLEASE</u><u> MARK</u><u> ME</u><u> BRAINLIEST</u></h3>
<u>Answer:</u> The initial concentration of
are 0.0192 M and 0.0192 M respectively.
<u>Explanation:</u>
We are given:
Equilibrium concentration of HI = 0.030 M
Moles of hydrogen gas = Moles of iodine gas (concentration will also be the same)
For the given chemical equation:

<u>Initial:</u> x x -
<u>At eqllm:</u> x-c x-c 2c
Calculating the value of 'c'

The expression of
for above reaction follows:
![K_{eq}=\frac{[HI]^2}{[H_2]\times [I_2]}](https://tex.z-dn.net/?f=K_%7Beq%7D%3D%5Cfrac%7B%5BHI%5D%5E2%7D%7B%5BH_2%5D%5Ctimes%20%5BI_2%5D%7D)
We are given:

![[H_2]=(x-c)=(x-0.015)](https://tex.z-dn.net/?f=%5BH_2%5D%3D%28x-c%29%3D%28x-0.015%29)
![[I_2]=(x-c)=(x-0.015)](https://tex.z-dn.net/?f=%5BI_2%5D%3D%28x-c%29%3D%28x-0.015%29)
Putting values in above equation, we get:

Neglecting the value of x = 0.0108 M, because the initial concentration cannot be less than the equilibrium concentration.
x = 0.0192 M
Hence, the initial concentration of
are 0.0192 M and 0.0192 M respectively.
I believe this would be Avogadro's law which states ''Equal volumes of all gases, at the same temperature and pressure, have the same number of molecules regardless of their chemical nature and physical properties.''
Answer:
Cretaceous Period
Explanation:
Dinosaurs went extinct about 65 million years ago (at the end of the Cretaceous Period), after living on Earth for about 165 million years.
<u>Answer:</u> The Gibbs free energy of the given reaction is -40 kJ
<u>Explanation:</u>
The given chemical equation follows:

The equation for the standard Gibbs free change of the above reaction is:
![\Delta G^o_{rxn}=[(2\times \Delta G^o_f_{(NH_3(g))})]-[(1\times \Delta G^o_f_{(N_2(g))})+(3\times \Delta G^o_f_{(H_2(g))})]](https://tex.z-dn.net/?f=%5CDelta%20G%5Eo_%7Brxn%7D%3D%5B%282%5Ctimes%20%5CDelta%20G%5Eo_f_%7B%28NH_3%28g%29%29%7D%29%5D-%5B%281%5Ctimes%20%5CDelta%20G%5Eo_f_%7B%28N_2%28g%29%29%7D%29%2B%283%5Ctimes%20%5CDelta%20G%5Eo_f_%7B%28H_2%28g%29%29%7D%29%5D)
We are given:

Putting values in above equation, we get:
![\Delta G^o_{rxn}=[(2\times (-16.45))]-[(1\times (0))+(3\times (0))]\\\\\Delta G^o_{rxn}=-32.9kJ/mol](https://tex.z-dn.net/?f=%5CDelta%20G%5Eo_%7Brxn%7D%3D%5B%282%5Ctimes%20%28-16.45%29%29%5D-%5B%281%5Ctimes%20%280%29%29%2B%283%5Ctimes%20%280%29%29%5D%5C%5C%5C%5C%5CDelta%20G%5Eo_%7Brxn%7D%3D-32.9kJ%2Fmol)
The equation used to Gibbs free energy of the reaction follows:

where,
= free energy of the reaction
= standard Gibbs free energy = -32.9 kJ/mol = -32900 J/mol (Conversion factor: 1 kJ = 1000 J)
R = Gas constant = 8.314J/K mol
T = Temperature = ![25^oC=[273+25]K=298K](https://tex.z-dn.net/?f=25%5EoC%3D%5B273%2B25%5DK%3D298K)
= Ratio of concentration of products and reactants at any time = 



Putting values in above equation, we get:

Hence, the Gibbs free energy of the given reaction is -40 kJ