Answer the question below by filling in the blank spaces in the question. The ch

Question

Answer the question below by filling in the blank spaces in the question. The chromate and dichromate ions set up an equilibrium system as follows energy+2 Cr04(a)+2 H(a)r272 (ac) H20 p yellow orange State the equilibrium shift (eft, right, no shift) in the reaction for the following stress Equilibrium shift 1. Increase in [H*1 2. Increase in [CrO4 21 3. Increase in (Cr2072 4. Decrease in (H1 5. Decrease in [CrO4 2") 6. Increase in temperature 7. Decrease in temperature 8. Add HCI (aq) 9. Add NaOH 10. Add H2o

Explanation / Answer

The shift of the equilibrium position can be predicted by using LeChatelier's principle.

According to LeChatelier's principle, when a system at equilibrium is subjected to a change in either concentration or temperature or pressure then the equilibrium will shift in such a direction that it opposes or nullifies the change.

For example:In an equilibrium reaction, when concentration of species on the left hand side is increased,then the equilibrium will shift towards right and formation of products is favoured and vice-versa.

Example2:When an equilibrium reaction is endothermic in the forward direction, then increase in temperature favours the formation of products and equilibrium shift towards right.

The given reaction is endothermic in the forward direction.

1.H+ is in the left side of the equilibrium.If [H+] is increased, then equilibrium shift towards right that is towards the formation of products.

A------ right

2.Similarly chromate ion is in left side and increase in its concentration shifts the equilibrium towards right.

B----- right

3.Dichromate ion is in right side and increase in its concentration shifts the equilibrium towards left.

C------ left

4.Decrease in concentration of H+ ions will shift the equilibrium towards left.

D ---- left

5.Similarly decrease in concentration of chromate (reactant) leads to shift the equilibrium towards left means backward reaction is favoured.

E ---- left

6.The reaction is an endothermic reaction in the forward direction, so increase in temperature favours the forward reaction and equilibrium shift towards right.

F---- Right

7.Decrease in temperature favours the backward reaction and the equilibrium shift towards left.

G ----- Left

8.HCl is a strong acid and it dissociates completely into its respective ions.

H+ is in the left side.So increase in its concentration shifts the equilibrium towards right.

H------ Right

9. Addition of NaOH which is a base, shifts the equilibrium towards left.

Since NaOH reacts with the H+ ions which are in left side and their concentration decreases.So equilibrium shift towards left and favours the backward reaction.

I----- left

10.Adding water , increases the concentration on the right side so equilibrium shift towards left hand side that is it favours the formation of left hand side substrates.

J----- left

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