Question

Consider this reaction: 6 CO2 + 6 H2O + light equation C6H12O6 + 6 O2 If there were 2.38 x 102 g of H2O, 18.6 moles of CO2, and plenty of light, what would be the theoretical yield of the reaction?

Answer 1

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Answer 2

Concept

Mole concept is the method used to express the amount of the substance.

Given

• The reaction given is  6 CO2 + 6 H2O →  C6H12O6 + 6 O2 .
• The mass of H2O given is 2.38 x 102 g.
• Moles of CO2 given is 18.6.

Find

We need to calculate the theoretical yield of the reaction

Solution

6 CO2 + 6 H2O →  C6H12O6 + 6 O2

6 moles of H2O  1 mole of C6H12O6

1 mole of H2O = 1/6th mole of C6H12O6

∴ 18gm of H2O = 276/6 gm of C6H12O6

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

$= \frac{2.38*10^2*276/6}{18} \\= 608.22gms$of C6H12O6

1 mole of  C6H12O6 = 276gms

? moles of C6H12O6 = 608.22gms

= 608.22/276

= 2.2 moles of C6H12O6

Similarly ,

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 the theoretical yield is 608.22 grams of C6H12O6 and 531.2 grams of O2

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