Question

Consider this reaction: 6 CO2 + 6 H₂O + light
C6H12O6 + 6 02
If you actually produced 30g of C6H12O6 what would be the percent yield?
Calculate the theoretical yield from having 2.38 x 10² g of H₂O, 18.6 moles of CO₂.

Answer 1

531.2 grams of oxygen and 608.22 grams of C6H12O6 make up the potential yield.

What is a Moles?

• A mole is the amount of a substance that contains precisely 6.02214076 X 1023 of the substance's fundamental components.
• If a material has the same mass as 12.000 g of 12C and the same number of elementary particles as atoms, it is said to have a mole of that substance.
• The mole can be used to determine the simplest compound formula and calculate the quantities needed for chemical reactions. Molarity, a related concept, comes in handy when discussing reactions in solutions. Molarity is the measure of how many moles of a solute are present per liter of a solution (M).
• Molecular quantities are those that cannot be measured in terms of grams or milligrams. This way, a mole counts the number of atoms, ions, or molecules.

Determine the reaction's theoretical yield:

Given is the reaction: 6 CO2 + 6 H2O = C6H12O6 + 6 O2.

2.38 x 102 g of H2O are provided as the mass.

Given is 18.6 moles of CO2.

6 CO2 + 6 H2O →  C6H12O6 + 6 O2

6 moles of H2O  1 mole of C6H12O6

1 mole of water equals 0.6 moles of C6H12O6.

18gm of H2O = 276/6 gm of C6H12O6

2.38*10^2 gm of H2O = ? gm of C6H12O6

$=\frac{2.38*10^{2} *\frac{276}{6} }{18}$

$=608.22gms$ of C6H12O6

1 mole of  C6H12O6 = 276gms

? moles of C6H12O6 = 608.22gms

= 608.22/276

= 2.2 moles of C6H12O6

6 moles of CO2 = 6 moles of O2

1 mole of CO2 = 1 mole of O2

∴ 18.6 moles of CO2 = 18.6 moles of O2

1 mole of O2 = 32gms of O2

∴18.6 moles of O2 = ?  gm

= 18.6*32

= 531.2gms of O2

Hence 531.2 grams of oxygen and 608.22 grams of C6H12O6 make up the potential yield

To learn more about moles, refer to:

brainly.com/question/15356425

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