Question

In the reaction shown below, 100 grams of H2CO3 decomposes to form 71 grams of CO2. Why is the amount of CO2 produced not equal to 100g?

Answer 1

H2CO3 yields H2O + CO2

Because some mass is converted to energy and then given off as heat in the reaction, the mass of the products will be less than the expected amount.
The chemical equation shown is not balanced. The amount of CO2 will equal 100g if the equation is balanced.
The chemical equation is balanced, but the amounts are in grams, not moles. The grams need to be converted to moles.
Decomposition reactions are unstable and almost immediately

Answer 2

@Abmon98 could you help me?

Answer 3

When elements and compounds react to form new products, mass cannot be lost or gained.
"The Law of Conservation of Mass" definition states that mass cannot be created or destroyed, but changed into different forms.
So, in a chemical change, the total mass of reactants must equal the total mass of products.
If you add up the mass of water and Carbon dioxide it would equal the mass of H2CO3
Number of Moles=Mass(g)/Molar Mass(g/mol)
100/62 moles of H2CO3
71/44 moles of CO2
Mole Ratio of H2CO3: CO2 : H2O
Are 1:1:1 So they share the same mole ration workout the number of moles and * by 18(molar Mass of Water and then add it to 71) it would equal 100
so i would go with option 3

Answer 4

absolutely, thank you! :3

Answer 5

Dont mention it :D