Answer:
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Explanation:
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Answer:
Explanation:
F Cl Br belongs to the Same group
Answer:
.
Start color: yellowish-green.
End color: dark purple.
Assumption: no other ion in the solution is colored.
Explanation:
In this reaction, chlorine gas
oxidizes iodine ions
to elemental iodide
. At the same time, the chlorine atoms are converted to chloride ions
.
Fluorine, chlorine, bromine, and iodine are all halogens. They are all found in the 17th column of the periodic table from the left. One similarity is that their anions are not colored. However, their elemental forms are typically colored. Besides, moving down the halogen column, the color becomes darker for each element.
Among the reactants of this reaction,
is colorless. If there's no other colored ion, only the yellowish-green hue of
would be visible. Hence the initial color of the reaction would be the yellowish-green color of
.
Similarly, among the products of this reaction,
is colorless. If there's no other colored ion, only the dark purple hue of
would be visible. Hence the initial color of the reaction would be the dark purple color of
.
<u>Answer:</u> The value of
for the surrounding when given amount of CO is reacted is 432.52 J/K
<u>Explanation:</u>
Entropy change is defined as the difference in entropy of all the product and the reactants each multiplied with their respective number of moles.
The equation used to calculate entropy change is of a reaction is:
![\Delta S^o_{rxn}=\sum [n\times \Delta S^o_{(product)}]-\sum [n\times \Delta S^o_{(reactant)}]](https://tex.z-dn.net/?f=%5CDelta%20S%5Eo_%7Brxn%7D%3D%5Csum%20%5Bn%5Ctimes%20%5CDelta%20S%5Eo_%7B%28product%29%7D%5D-%5Csum%20%5Bn%5Ctimes%20%5CDelta%20S%5Eo_%7B%28reactant%29%7D%5D)
For the given chemical reaction:

The equation for the entropy change of the above reaction is:
![\Delta S^o_{rxn}=[(2\times \Delta S^o_{(CO_2(g))})]-[(1\times \Delta S^o_{(O_2(g))})+(2\times \Delta S^o_{(CO(g))})]](https://tex.z-dn.net/?f=%5CDelta%20S%5Eo_%7Brxn%7D%3D%5B%282%5Ctimes%20%5CDelta%20S%5Eo_%7B%28CO_2%28g%29%29%7D%29%5D-%5B%281%5Ctimes%20%5CDelta%20S%5Eo_%7B%28O_2%28g%29%29%7D%29%2B%282%5Ctimes%20%5CDelta%20S%5Eo_%7B%28CO%28g%29%29%7D%29%5D)
We are given:

Putting values in above equation, we get:
![\Delta S^o_{rxn}=[(2\times (213.74))]-[(1\times (205.14))+(2\times (197.674))]\\\\\Delta S^o_{rxn}=-173.008J/K](https://tex.z-dn.net/?f=%5CDelta%20S%5Eo_%7Brxn%7D%3D%5B%282%5Ctimes%20%28213.74%29%29%5D-%5B%281%5Ctimes%20%28205.14%29%29%2B%282%5Ctimes%20%28197.674%29%29%5D%5C%5C%5C%5C%5CDelta%20S%5Eo_%7Brxn%7D%3D-173.008J%2FK)
Entropy change of the surrounding = - (Entropy change of the system) = -(-173.008) J/K = 173.008 J/K
We are given:
Moles of CO gas reacted = 2.25 moles
By Stoichiometry of the reaction:
When 2 moles of CO is reacted, the entropy change of the surrounding will be 173.008 J/K
So, when 2.25 moles of CO is reacted, the entropy change of the surrounding will be = 
Hence, the value of
for the surrounding when given amount of CO is reacted is 432.52 J/K