Calculate how much Carbon Dioxide IN GRAMS needs to be absorbed to release 500g of oxygen during photosynthesis.

687.5 g of CO2

Explanation:

We'll begin by writing the balanced equation for photosynthesis. This is illustrated below:

6CO2 + 6H2O —> C6H12O6 + 6O2

Next, we shall determine the mass of CO2 absorbed and the mass of O2 released from the balanced equation. This is illustrated below:

Mass of CO2 = 12 + (2 × 16) = 12 + 32

= 44 g/mol

Mass of CO2 from the balanced equation = 6 × 44 = 264 g

Molar mass of O2 = 2 × 16 = 32 g/mol

Mass of O2 from the balanced equation = 6 × 32 = 192 g

Summary:

From the balanced equation above,

264 g of CO2 were absorbed to release 192 g of O2.

Finally, we shall determine the mass of CO2 absorbed to release 500 g of O2. This can be obtained as follow:

From the balanced equation above,

264 g of CO2 were absorbed to release 192 g of O2.

Therefore, Xg of CO2 will be absorbed to release 500 g of O2 i.e

Xg of CO2 = (264 × 500)/192

Xg of CO2 = 687.5 g

Thus, 687.5 g of CO2 will be absorbed to release 500 g of O2.

"you start with 15.67 g mgco3-xh2o, when heated and all the water is removed, you are left with 7.58 g mgco3 only.

therefore, you had 15.67 - 7.58 = 8.09g h2o  

moles of each :

7.58g mgco3 = ? moles = 7.58g / 83.4g/mole = 0.09moles  

8 09g h2o = ? moles = 8.09g / 18g/mole = 0.44moles  

molar ratio between the two by dividing both numbers by the smallest number :

0.09 / 0.09 = 1  

0.44 / 0.09 = 4.8  

mgco3-5h2o"

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