Explain how stressing the system, Fe3+ + SCN1- ⇄ FeSCN2+, with the addition or removal of...
- Explain how stressing the system, Fe3+ + SCN1- ⇄ FeSCN2+, with the addition or removal of ions and temperature increased or decreased the concentration of the species. How did this affect the shift of the reaction in either the forward direction to produce more thiocyanato iron (III) ion or the reverse direction to remove thiocyanato iron (III) ion?
Homework Answers
According to Le Chatelier principal, if a reaction is in equilibrium and some changes are made with respect to concentration or environmental conditions the equilibrium reaction will shift toward a side such that the effect can be minimized.
Now in this reaction, if we increase the concentration of reactants ( Fe3+ or SCN1- ) , the reaction will go to form more products ( FeSCN2+ ) , hence the shift is in forward direction.
Moreover, this can also be obtained by removing the product. Hence the product will be formed more as it is less in amount. The reaction will shift in forward direction.
Whereas, if concentration of reactants is decreased or they are removed from solution the reaction will shift such that to form more reactants. Hence in backward direction. Similar case is when more product is added.
Further, this reaction is exothermic, hence addition of heat or increase in temperature will be same as adding more product. Therefore shifting the reaction to reactants side or reverse.
Also, if temperature is decreased, then the shift of reaction will be toward product side or forward.
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Explain how stressing the system, Fe3+ +
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FeSCN2+ (aq). The goal is to predict the color change (darker or
lighter) for test tubes 2-8. I have attached the supplemental
sheets given to help with the problem. The test tubes 2-8 are being
manipulated either by temperature or things being added which can
be seen by one of the pictures.
2. For reaction "UCTIONS are increased by the same amount. Fe3+ (aq) + SCN (aq) $...
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