removed, the position of equilibrium will shift back to reactants. Therefore, for an endothermic reaction, as the temper

[answerhappygod]

Removed The Position Of Equilibrium Will Shift Back To Reactants Therefore For An Endothermic Reaction As The Temper 1 (34.47 KiB) Viewed 29 times

Removed The Position Of Equilibrium Will Shift Back To Reactants Therefore For An Endothermic Reaction As The Temper 2 (9.88 KiB) Viewed 29 times

Removed The Position Of Equilibrium Will Shift Back To Reactants Therefore For An Endothermic Reaction As The Temper 3 (10.39 KiB) Viewed 29 times

Removed The Position Of Equilibrium Will Shift Back To Reactants Therefore For An Endothermic Reaction As The Temper 4 (17.75 KiB) Viewed 29 times

Removed The Position Of Equilibrium Will Shift Back To Reactants Therefore For An Endothermic Reaction As The Temper 5 (9.07 KiB) Viewed 29 times

Removed The Position Of Equilibrium Will Shift Back To Reactants Therefore For An Endothermic Reaction As The Temper 6 (9.46 KiB) Viewed 29 times

Removed The Position Of Equilibrium Will Shift Back To Reactants Therefore For An Endothermic Reaction As The Temper 7 (9.46 KiB) Viewed 29 times

removed, the position of equilibrium will shift back to reactants. Therefore, for an endothermic reaction, as the temperature increases, K will increase; as the temperature decreases, K will decrease. Procedure Video A: https:/lwww. youtube.com/watch?v=RjFW3sml1fy Click on the link above and watch the You Tube video. Record the data in the data tables below and answer the questions. The scientist in the video explains the shifts in the equilibria very well. Be sure to put these explanations in your own words with your answers to the questions below.  orange Cr2​O72​(aq)+H2​O(I)⇌​ yellow 2CrO42−​​(aq)+2H+(aq)
1) In terms of LeChâtelier's Principle, explain specifically why the reaction shifted when acid was added to the aqueous solution.
2) In terms of LeChâtelier's Principle, explain specifically why the reaction shifted when base was added to the aqueous solution.
Heat +N2​O4​( g)⟹2NO2​( g) colorless brown
3) In terms of LeChâtelier's Principle, explain specifically why the reaction shifted when the gas was heated.
4) In terms of LeChâtelier's Principle, explain specifically why the reaction shifted when the gas was cooled.
5) Based on the data above, does the equilibrium constant, K, for this process increase or decrease with an increase in temperature? Explain, clearly and concisely.