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Consider the following equilibrium system - HSC - SSCE Chemistry - Question 22 - 2021 - Paper 1
Question 22
Consider the following equilibrium system. 2CrO$_{4}^{2-}$(aq) ⇌ Cr$_2$O$_7^{2-}$(aq) + H$_2$O(l) ΔH = -895 kJ mol$^{-1}$ The solution is orange. Justify TWO way... show full transcript
Worked Solution & Example Answer:Consider the following equilibrium system - HSC - SSCE Chemistry - Question 22 - 2021 - Paper 1
Step 1
Justify TWO ways to shift the equilibrium to the left
Answer
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Reduce the concentration of hydrogen ions (H): By decreasing the concentration of H ions in the solution, the equilibrium will shift to the left. This is because the system seeks to counteract this change by producing more H ions and more yellow chromate ions (CrO), thus resulting in a more yellow solution.
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Heat the solution: Since the forward reaction is exothermic (it releases heat), increasing the temperature will drive the equilibrium to the left. This shift will increase the concentration of the yellow chromate ions, resulting in a color change towards yellow.