Question

The reaction Co(H2O)6 + 4Cl– ⇌ CoCl4 + 6H2O is in equilibrium. If the products are increased which of the following is true?

increase the forward reaction, decrease the reverse reaction
This would not affect the rate of the reactions
increase the reverse reaction, decrease the forward reaction

Answer 1

@tranquility

Answer 2

He helped me yesterday thoo so um wut u talking about?

Answer 3

Defining some things beforehand
Reactants here are Co(H2O)6 + 4Cl–
Products here are CoCl4 + 6H2O
Forward reaction: Basic order of reaction, reactants lead to product
[\(\color{green}{Co(H_2O)_6 + 4Cl^–} \rightarrow \color{red}{CoCl_4 + 6H_2O} \)]

Reverse reaction: The opposite direction of the reaction, products going to reactants
[\(\color{green}{Co(H_2O)_6 + 4Cl^–} \leftarrow \color{red}{CoCl_4 + 6H_2O} \)]

A reaction will always want to stay at equilibrium
(Any change in products or reactants will affect the reaction, this eliminates the second option)

With that said, if you increase the products, then in order to stay at equilibrium youd want to have an increase in the reaction for its products to keep it equal

Another way of thinking about it: If you have too much of a product, then you'll want more reactants to keep them equal
[\(\color{green}{Co(H_2O)_6 + 4Cl^–} \color{red}{\leftarrow CoCl_4 + 6H_2O \uparrow}\)]
(This means we'll have a reverse reaction, trying to increase the amount of reactants to get to an equilibrium again)

Does this make sense? If it doesn't feel free to ask questions

Answer 4

Yeah

Answer 5

Yayyyy thank you!