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michelle10
 2 years ago
when will an equilibrium stop?
1.when we have more reactant than product. 2. when we have more production reactant 3. when the concentration of the product and reactant are equal 4 . when concentration of the reactant and product reach their equilibrium values 5. never
michelle10
 2 years ago
when will an equilibrium stop? 1.when we have more reactant than product. 2. when we have more production reactant 3. when the concentration of the product and reactant are equal 4 . when concentration of the reactant and product reach their equilibrium values 5. never

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michelle10
 2 years ago
Best ResponseYou've already chosen the best response.0Someone help me plz . Giving metals

JamesWolf
 2 years ago
Best ResponseYou've already chosen the best response.1do you mean, when will a chemical reaction stop?

michelle10
 2 years ago
Best ResponseYou've already chosen the best response.0@JamesWolf . Yes i need help with this asap. what would be the best answer?

JamesWolf
 2 years ago
Best ResponseYou've already chosen the best response.1if the concentration of product and reactant are equal, and the chemical process is reversable, then there is no preference to create product or reactant. So the reaction will be in equilibrium

michelle10
 2 years ago
Best ResponseYou've already chosen the best response.0So it would be #4 @JamesWolf

mos1635
 2 years ago
Best ResponseYou've already chosen the best response.04 or 5 4 is correct. that is correct in equilibrium. concentration of the reactant and product reach their equilibrium values and those values stay constant if nothing else change. but 5 is also corect due to the reaction continues with the same speed to both directions.... i would go with 5

thecuriousbud
 2 years ago
Best ResponseYou've already chosen the best response.0i would agree with the comment above me.

michelle10
 2 years ago
Best ResponseYou've already chosen the best response.0@thecuriousbud u would agree with #5 also?? & thank for ur help

thecuriousbud
 2 years ago
Best ResponseYou've already chosen the best response.0It is generally considered that the forward and reverse reactions both continue but at the same rate, so that "net reaction" stops which explains why 4 would be right, but not the microreactions which is why 5 is correct.
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