two substances are dissolved in water and start to react which statement accurately describes the appearance of the solution when it reaches equilibrium
a. the appearance Will continue to change as the forward reaction continues at a slow balanced rate
b. no changes will be apparent as the forward in reverse reactions continue
c. The appearance will continue to change as the forward and reverse reactions continue
d. no changes will be a parent as the reaction stop
1. which statement explains what it means for a chemical reaction to be at equilibrium? Answer: The rate of the forward and backward reactions are equal
2. Two substances are dissolved in water and start to react. Which statement accurately describes the appearance of the solution when it reaches equilibrium? Answer: No changes will be apparent, as the forward and reverse reactions continue.
3. Why is it not useful to talk about equilibrium in the context of baking? Answer: The reactions that happen in baking are not reversible reactions.
4. How can you tell that this process is not at equilibrium? Answer: The reaction mixture is not complete as reactants are still being added to the system.
5. In which step of the process is the person most likely at chemical equilibrium? Answer: in step 5 when the person returns to a healthy level of blood sugar and remains there.
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To determine the correct answer, let's review the process of reaching equilibrium in a chemical reaction.
When two substances dissolve in water and start to react, they undergo a forward reaction, where reactants combine to form the products. At the same time, a reverse reaction occurs, where products can react to produce reactants again. As the reaction progresses, the concentration of reactants decreases, while the concentration of products increases.
Eventually, the rates of the forward and reverse reactions become equal, and the system reaches a state called equilibrium. At this point, the concentrations of reactants and products stabilize, even though the reactions are still occurring.
Now let's consider the options:
a. The appearance Will continue to change as the forward reaction continues at a slow balanced rate.
This statement is inaccurate because when equilibrium is reached, both the forward and reverse reactions are occurring at the same rate, causing no net changes in the appearance of the solution.
b. No changes will be apparent as the forward and reverse reactions continue.
This statement accurately describes the appearance of the solution at equilibrium. The concentrations of reactants and products remain constant as the forward and reverse reactions are balanced.
c. The appearance will continue to change as the forward and reverse reactions continue.
This statement is inaccurate because the appearance of the solution does not change once equilibrium is achieved. The concentrations stabilize, resulting in no observable changes.
d. No changes will be apparent as the reaction stops.
This statement is also inaccurate because at equilibrium, the reactions are still occurring. Equilibrium is a dynamic state, where reactants are continuously converting to products and vice versa.
Therefore, the correct answer is b. No changes will be apparent as the forward and reverse reactions continue.