same masses of different metal carbonates are fully decomposed. why is the volume of carbon dioxide different for each metal carbonate?
mols = grams/molar mass
Molar masses are different so for constant grams the mols are different which makes mols CO2 different. For different number of mols there will be different volume since mols x 22.4L = volume @ STP
The volume of carbon dioxide produced during the decomposition of metal carbonates can vary depending on several factors, such as the nature of the metal, its valence, and the atomic mass of the metal involved.
To understand why the volume of carbon dioxide is different for each metal carbonate, we need to consider the chemical reactions involved in the decomposition process. When metal carbonates are heated, they undergo thermal decomposition, breaking down into metal oxides and carbon dioxide gas.
The general equation for the decomposition of a metal carbonate is:
Metal Carbonate (MCO3) → Metal Oxide (MO) + Carbon Dioxide (CO2)
The volume of carbon dioxide released during this reaction depends on the stoichiometry of the reaction, which is determined by the balanced chemical equation. The balanced equation gives us the molar ratio between the reactants (metal carbonate) and the products (metal oxide and carbon dioxide).
Let's take an example to illustrate this:
Suppose we have two metal carbonates, M1CO3 and M2CO3, with the same mass but different metals (M1 and M2) and atomic masses. When these carbonates are decomposed, they produce the respective metal oxides (M1O and M2O) and carbon dioxide (CO2).
The molecular weight of M1CO3 can be calculated by summing the atomic masses of its constituents (M1, C, and O). Similarly, we can calculate the molecular weight of M2CO3.
Now, let's assume that both carbonates are fully decomposed. Since the masses of the carbonates are the same, we can say that the moles of the two carbonates are equal (moles = mass / molecular weight). This means that the number of moles of carbon dioxide produced will be equal for both reactions.
However, since the molecular weights of M1CO3 and M2CO3 are different, the molar ratio between the metal carbonate and carbon dioxide will be different for each metal.
For example, let's say that M1 has a higher atomic mass compared to M2. This means that the molecular weight of M1CO3 will be higher than that of M2CO3. As a result, the ratio of moles of M1CO3 to moles of CO2 will be higher compared to the ratio of moles of M2CO3 to moles of CO2.
This difference in molar ratio translates to a difference in volume of carbon dioxide produced. Since gases occupy the same volume under the same conditions, the one with a higher molar ratio will result in more carbon dioxide by volume.
In conclusion, the volume of carbon dioxide produced during the full decomposition of metal carbonates can vary because of differences in the molar ratios between the metal carbonates and carbon dioxide, which are determined by the balanced chemical equation and the atomic masses of the metals involved.