How many carbon dioxide (CO2) molecules are produced during the decomposition of 1.25 molecules of carbonic acid (H2CO3)? Remember to use the balanced equation!

7.5×10^23 molecules of carbon dioxide

Explanation:

H2CO3 → CO2 + H2O

From the balanced reaction equation, one mole of carbonic acid produces one mole of carbon IV oxide.

1.25 moles of carbonic acid will produce 1.25 moles of carbon dioxide

If 1 mole of carbon dioxide contains 6.02×10^23 molecules

1.25 moles of carbon dioxide contains 1.25×6.02×10^23= 7.5×10^23 molecules of carbon dioxide

1.25 molecules of CO2 will be produced

Explanation:

Step 1: data given

Number of molecules carbonic acid (H2CO3) = 1.25 molecules

Molar mass carbonic acid (H2CO3) = 62.03 g/mol

Number of Avogadro = 6.022 * 10^23 / moles

Step 2: Calculate moles of H2CO3

Moles H2CO3 = 1.25 molecules / 6.02 *10^23

Moles H2CO3 = 2.076 * 10^-24 moles

Step 3: The equation

H2CO3 → H2O + CO2

For 1 mol H2CO3 we'll have 1 mol H2O and 1 mol CO2

For  2.076 * 10^-24 moles H2CO3 we'll have  2.076 * 10^-24 moles CO2

Step 4: Calculate molecules CO2

Molecules CO2 = moles CO2 * number of Avogadro

Molecules CO2 =  2.076 * 10^-24 moles * 6.02 * 10^23

Molecules CO2 = 1.25 molecules

1.25 molecules of CO2 will be produced

answer

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