How many carbon dioxide (CO2) molecules are produced during the decomposition of 1.25 moles of Carbonic acid (H2CO3)

Answer 1

The decomposition of Carbonic Acid is: H₂CO₃ ----> H₂O + CO₂

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(***Always check to see if the chemical equation is balanced before making any further calculations***)

In this case the left side has 2 Hydrogens, 1 Carbon and 3 Oxygens. One the right there are 2 Hs, 1 C and 3 Os so the equation is balanced.

The right side of the chemical equation has one molecule of H₂O and one molecule of CO₂. Here is the solution in four steps or less.

(Another way of looking at, 1 molecule of H₂CO₃ decomposes into 1 molecule of H₂O and 1 molecule of CO₂.)

Based off the correction from J.R. S. the correct solution in four steps or less is:

1.25 mole of H₂CO₃ x ( 1 mole of CO₂ / 1 mole of H₂CO₃ ) x (6.0221409 x 10²³ molecules of

CO₂ / 1 mole of CO₂) = 7.53 x 10²³ molecules of CO₂

Answer 2

The balanced equation for this decomposition is...

H₂CO₃ ==> CO₂ + H₂O

1.25 moles H₂CO₃ ==> 1.25 moles CO₂ according to the stoichiometry of the balanced equation

Now we have to convert the 1.25 moles of CO₂ into the number of molecules. This is accomplished using Avogadro's number, 6.02x10²³ molecules/mole...

1.25 moles CO₂ x 6.02x10²³ molecules/mole = 7.5x10²³ molecules of CO₂