9. when the [CO2] and [H2CO3] are both horizontal lines, the rate of the forward reaction is ____ The rate of the reverse reaction.
a. faster then
b. slower than
c. The same as
10. if you added molecules of H2CO3 into the liquid, what do you think will happen?
a.Since this would increase the concentration of CO2, the forward reaction would be favored
b. since this would increase the concentration of C02, the reverse reaction would be favored
c. since this would increase the concentration of H2CO3, The reverse reaction will be favored.
d. since this would increase the concentration of H2CO3, The forward reaction would be favored.
11. if CO2 is being produced and the solution at a faster rate than H2CO3, Then the rate of the _____ reaction is faster than the rate of the____ reaction.
a. forward/ reversed
b. reversed/ forward
c. neither a nor b is correct
12. which statement best describes why the equilibrium constant is larger number (greater than 1) in this simulation?
a. at equilibrium the concentration of product is equal to the concentration of reactants
b. at equilibrium there is significantly less product than reactant
c. at equilibrium there is significantly more product than reactant.
13. when the carbonator as CO2 to the solution, a _____ is added to the reaction, which pushes the reaction in the ____ direction.
a. product, forward
b. product, reverse
c. reactant, forward
d. reactants, reverse
14. for a given reaction, which statement is true?
a. The equilibrium constant is always the same number, but the concentration of reactants and products can vary at equilibrium.
b. The equilibrium constant it’s always the same number as long as the temperature is held constant.
c. The equilibrium constant is always the same number as long as the pressure is held constant.
d. The equilibrium constant is always the same number as long as the concentration of CO2 is held constant.
15. when the pressure increases, the concentration of CO2 gas and the solution at equilibrium____
a. increases
b. decreases
c. does not change
16. which of the following causes the concentration of H2co3 in the solution at equilibrium to increase?
a. increasing pressure, volume, or CO2
b. decreasing the pressure, volume, or CO2
c. increasing pressure, decreasing volume, or increasing CO2
d. decreasing pressure, increasing volume, or decreasing CO2
y’all please come in clutch bcc i can’t find these answers nowhere 🥲
Were you given notes before taking the test?
yea it’s like a lab report
9. To determine the rate of the forward reaction compared to the rate of the reverse reaction when both [CO2] and [H2CO3] are horizontal lines, you need to understand the concept of equilibrium. In a chemical reaction, equilibrium is reached when the rates of the forward and reverse reactions are equal. In this case, if both [CO2] and [H2CO3] are horizontal lines, it indicates that their concentrations are not changing over time. Therefore, the rate of the forward reaction is the same as the rate of the reverse reaction, so the answer is c. The same as.
10. Adding molecules of H2CO3 to the liquid will increase its concentration. To understand the effect on the reaction, recall that increasing the concentration of a reactant or product usually leads to a shift in the equilibrium position. In this case, since H2CO3 is a reactant, increasing its concentration would favor the forward reaction. Therefore, the answer is d. Since this would increase the concentration of H2CO3, the forward reaction would be favored.
11. If CO2 is being produced at a faster rate than H2CO3, it implies that the forward reaction is happening faster than the reverse reaction. The rate of the forward reaction is faster than the rate of the reverse reaction. Therefore, the answer is a. forward/reverse.
12. The equilibrium constant (K) is a measure of the ratio of product concentrations to reactant concentrations at equilibrium. In this case, if the equilibrium constant is greater than 1, it indicates that there is significantly more product than reactant at equilibrium. Therefore, the answer is c. at equilibrium, there is significantly more product than reactant.
13. When the carbonator adds CO2 to the solution, it is adding a product to the reaction. According to Le Chatelier's principle, adding a product to a reaction shifts the equilibrium position in the reverse direction (as the system tries to consume the added product). Therefore, the answer is b. product, reverse.
14. The equilibrium constant (K) is determined by the temperature and the relative concentrations of reactants and products at equilibrium. It is a constant value for a given reaction at a specific temperature. The equilibrium constant does not depend on the absolute concentrations of reactants and products, but rather on their ratio. Therefore, the answer is b. The equilibrium constant is always the same number as long as the temperature is held constant.
15. When the pressure increases, the concentration of CO2 gas and the solution at equilibrium do not change. Changes in pressure only affect the concentrations of gases, not solutions. Therefore, the answer is c. does not change.
16. Increasing the pressure, decreasing the volume, or increasing the concentration of CO2 would favor the forward reaction, leading to an increase in the concentration of H2CO3 at equilibrium. Therefore, the answer is c. increasing pressure, decreasing volume, or increasing CO2.
Is there anyway you could send it?
Here are the rules.
At equilibrium, the forward reaction rate = the reverse reaction rate.
According to Le Chatelier's principle, if we do something to a reaction at equilibrium, the reaction will shift to right, shift to the left, stay the same in order to UNDO what we did to it. With regard to the CO2/H2CO3 equilibrium you did not show in your post what reaction you are studying; i.e., H2CO3 ==> H2O + CO2 or H2O + CO2 ==> H2CO3.
If I assume the reaction is H2CO3 ==> CO2 + H2O and we add H2CO3 to the mixture, then the forward reaction will increase BECAUSE the reaction needs to get rid of the extra H2CO3 we added SO it produces more CO2 and H2O at the expense of the H2CO3 we added. If we add H2O or CO2 to the "closed" system, the reaction will move to the left producing more H2CO3 in order to use the CO2 or H2O that we added.
Now if you will use this information and my example to answer your lab report I will be happy to check your answers. If you run into one you have questions about just post it and explain exactly what you don't understand and I will help through that question. I'll bet you haven't had a better offer today.