If a plant produces 3.21 mol of c6h12o6, how many moles of co2 are needed?

1 answer:

3 0

Photosynthesis is the process by which CO₂ is converted to an organic compound. The complete reaction is as follows;
6CO₂ + 6H₂O --> C₆H₁₂O₆ + 6O₂
stoichiometry of CO₂ to C₆H₁₂O₆ is 6:1
For 1 mol of C₆H₁₂O₆ to be formed - 6 mol of CO₂ is required
Therefore for 3.21 mol of C₆H₁₂O₆ to be formed - 6 x 3.21 mol of CO₂ required
Number of moles required are - 19.26 mol of CO₂

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Answer:

False

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Calculate the concentrations of h2so3, hso−3, so2−3, h3o+ and oh− in 0.025 m h2so3.

sammy [17]

We will use this two reaction equation:

H2SO3 + H2O ↔ H3O+ + HSO3- Ka1 = 1.3 x 10^-2

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we will use the ICE table for the first equation:

H2SO3 + H2O ↔ H3O+ + HSO3-

initial 0.025 0 0

change -X +X +X

Equ (0.025-X) X X

Ka1 = [H3O+] [HSO3-] / [H2SO3]

1.3 x 10^-2 = X^2 / (0.025 - X) by solving for X

∴ X = 0.0127

when [H3O+] = X

∴[H3O+] = 0.0127 M

and when [HSO3-] = X

∴[HSO3-] = 0.0127 M

and when [H2SO3] = 0.025 - X

∴[H2SO3] = 0.025 - 0.0127

= 0.0123 M

when Kw = [OH-][H3O+]

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- by using the ICE table for the second equation:

HSO3- + H2O ↔ H3O+ + SO3 2-

initial 0.0127 0.0127 0

change -X +X +X

Equ (0.0127-X) (0.0127+X) X

when Ka2 = [SO32-] [H3O+] / [HSO3-]

by substitution:

6.3 x 10^-8 = X(0.0127+X) / (0.0127-X)

as the Ka2 is so small so we can assume that (0.01271 + X) & (0.01271-X) = 0.01271 and neglect X

6.3 x 10^-8 = 0.0127X /0.0127

∴X = 6.3 x 10^-8

when [SO3 2-] = X

∴[SO32-] = 6.3 x 10^-8

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Explanation:

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A balanced chemical equation specifies the quantities of reactants and products required to meet the Law of Conservation of Mass. This signifies that there is the same number of each sort of atom on the left side of the equation as there are on the right side. The rule of a balanced chemical equation is used to determine if two weights put on opposing sides of the fulcrum will balance each other.

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allochka39001 [22]

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