Small respiration task in class

[Chen22]

Hi, we did a small respiration task in class and now I need to calculate a few things.

I placed a bottle of NaOH in another bottle, together with a bottle of yeast and glucose. I did the same with another bottle, but without the yeast/glucose. Amount of glucose 0.2g.

Now I need to calculate how much CO2 has been produced and how much maximum can be produced.

I also need to know if there was enough O2 in the bottle to let the glucose react completely (bottle is 440ml). And if there wasn't to much CO2 in the bottle which gives a false result.

I also needed to know how much NaOH has been used.

What I have so far:
Titer of NaOH of bottle yeast/glucose: 0.089N
Titer of NaOH whithout yeast/glucose: 0.071N
NaOH used: 0.089N - 0.071N = 0.027N

Reaction of glucose with O2
C6H12O6+O2->6CO2+4H2O

I'm not sure if those are right :uhh:

Thanks

 

[Ouabache]

Reaction of glucose with O2
C6H12O6+O2->6CO2+4H2O
I'm not sure if those are right :uhh:

You're equation needs some fixing, check the number of elements on each side and see if they balance.
(Ex: left side H = 12, right side H = 8)

As far as the rest of your question, I don't follow your description. You placed a bottle of NaOH in another bottle, together with a bottle of yeast and glucose. It sounds like you have a big bottle with two little bottles sitting inside it, one with NaOH in it and the other with yeast/glucose. Is the big bottle then sealed or open? Are the small bottles sealed or open? Did I describe your setup correctly?

I don't know if your NaOH or your 'yeast/glucose' are all solid or if they are solutions. If they are solutions, what volume of liquid is there in each? You mentioned that the bottle is 440ml. Is that its capacity? The reason we need to be clear on this is because you are then given values of normality for two titers. Do you know what normality is?

 

[Blueshift5]

Hello, it sounds like you have conducted an interesting respiration experiment in class! Let's go through the calculations together to make sure everything is correct.

First, to calculate the amount of CO2 produced, we need to use the balanced equation for the reaction of glucose with O2. Based on the given amounts, we can see that 0.2g of glucose was used in the reaction. Using the molar mass of glucose (C6H12O6), we can convert the mass of glucose to moles. This comes out to be 0.0011 moles of glucose. According to the equation, for every mole of glucose, 6 moles of CO2 are produced. Therefore, we can calculate that 0.0066 moles of CO2 were produced in the reaction.

Next, to find the maximum amount of CO2 that can be produced, we need to consider the amount of O2 present in the bottle. The bottle has a volume of 440ml, so we need to convert that to liters (0.44L). Using the ideal gas law, we can calculate that there was approximately 0.019 moles of O2 present in the bottle. Since the reaction of glucose with O2 has a 1:1 ratio, this means that the maximum amount of CO2 that can be produced is also 0.019 moles.

Now, to determine if there was enough O2 in the bottle for the reaction to occur completely, we need to compare the amount of O2 present (0.019 moles) to the amount needed for the reaction (0.0011 moles). Since there was more than enough O2 present, we can conclude that the reaction was able to occur completely.

Lastly, to calculate the amount of NaOH used, we can use the titer values given. The difference between the two titer values (0.089N - 0.071N) is 0.018N. This means that 0.018 moles of NaOH were used in the reaction.

Overall, it seems like your calculations are correct! Just make sure to double check your units and conversions to ensure accuracy. Keep up the good work in your science class!