Use the equation to answer the question.
H2O(l) + heat ⇄ H2O(g)
A sample of water is at equilibrium at 100°C. Which statement best describes what will happen if liquid water is added to the system?
(1 point)
All of the liquid water molecules that are added will become water vapor.
All of the liquid water molecules that are added will remain liquid water.
More liquid water molecules will change to water vapor until a new equilibrium is reached.
More water vapor molecules will change to liquid water until a new equilibrium is reached.
A system is at equilibrium. Which statement is correct?
(The rate of the forward reaction equals the rate of the reverse reaction)
H2O(i) + heat = H2O(g)
A sample of water is at equilibrium at 100°C. Which statement best describes what will happen if liquid water is added to the system?
(More liquid water molecules will change to water vapor until a new equilibrium is reached)
CO(H20)2* + 4CM + heat = CoCI,?- + 6H,0
Cobalt ions form complex ions with water and chloride. The Co(H20),2* ions are pink, and the CoCI,2-ions are blue. A scientist
creates a solution that is purple at equilibrium. How can the scientist make the solution more pink?
(by adding water h2O)
NaBr(s) = Na* (aq) + Br (aq)
A student adds hydrobromic acid (HBr) to a solution of sodium bromide at equilibrium. How does this change affect the system?
(The additional bromine ions cause the equilibrium to shift to the reactants)
A copper complex reacts with ammonia according to the following reaction, where the left side of the reaction is a pale sky-blue
color and the right side is dark blue
Cu(H,0)2* (ag) + 4NH,(8g) = Cu(NH3),2* (ag) + 4H;0(aq)
Which change to a solution at equilibrium will make the solution darker?
(removing water h2O)
1. The rate of the forward reaction equals the rate of the reverse reaction.
2. More liquid water molecules will change to water vapor until a new equilibrium is reached.
3. by adding water (H2O)
4. The additional bromine ions cause the equilibrium to shift to the reactants.
5. removing water (H2O)
[quizlet: captncrun]
Material gorl is 100% correct !! thank you <33
yup they were right i just got 100% thank you!!!
Man i love yall bruh.
Thanks babes <3
UGH TY <3
thanks guys, y’all always come through 😩
y’all really be comin thru
To answer this question, we need to understand the concept of equilibrium and how it relates to the given equation.
In the given equation: H2O(l) + heat ⇄ H2O(g), we see that liquid water (H2O(l)) can evaporate into water vapor (H2O(g)) when heat is applied. Conversely, water vapor can condense into liquid water when heat is removed.
Since the system is already at equilibrium at 100°C, it means that the rate of evaporation and condensation is balanced. At this temperature, the amount of water vapor and liquid water present in the system is constant.
Now, let's consider the scenario where liquid water is added to the system. Adding liquid water means an increase in the concentration of water molecules in the liquid phase. According to Le Chatelier's principle, a system at equilibrium will naturally shift in a direction that counteracts any disturbance.
In this case, the addition of liquid water will disrupt the balance between evaporation and condensation. To restore equilibrium, the system will need to counteract this disturbance. The system does this by increasing the rate of evaporation (water molecules changing to water vapor) until a new equilibrium is reached.
Therefore, the statement that best describes what will happen if liquid water is added to the system is: "More liquid water molecules will change to water vapor until a new equilibrium is reached."