During an investigation, a scientist heated 2.76 g of silver carbonate until it decomposed to leave a silver residue. There was 2.16 g of silver residue formed. During this chemical reaction, 0.30g of CO2 and 0.30g of O2 were also produced.

Answer 1

To analyze the decomposition of silver carbonate (Ag2CO3), we can begin by using the law of conservation of mass. Let's break down the decomposition reaction and calculate the amounts.

Reaction of Silver Carbonate Decomposition

The decomposition reaction for silver carbonate is expressed as:

\[ 2 , \text{Ag}_2\text{CO}_3 \rightarrow 4 , \text{Ag} + 2 , \text{CO}_2 + \text{O}_2 \]

This equation tells us how silver carbonate decomposes into silver (Ag), carbon dioxide (CO2), and oxygen (O2).

Total Mass before and after Reaction

• Initial mass of silver carbonate (Ag2CO3): 2.76 g
• Mass of silver residue formed: 2.16 g
• Mass of CO2 produced: 0.30 g
• Mass of O2 produced: 0.30 g

Total Mass After Reaction

To find the total mass after the reaction, we can sum the masses of the remaining products:

\[ \text{Total mass after} = \text{mass of Ag} + \text{mass of CO}_2 + \text{mass of O}_2 \]

Substituting the known values:

\[ \text{Total mass after} = 2.16 , \text{g} + 0.30 , \text{g} + 0.30 , \text{g} = 2.76 , \text{g} \]

Conclusion

The total mass before the reaction (2.76 g) equals the total mass after the reaction (2.76 g), confirming that mass is conserved.

For further analysis or calculations, we can determine how the mass of the original silver carbonate relates to the masses of the products formed, or we could explore the stoichiometry of the decomposition. If you need any specific calculations or further insights based on this reaction, please let me know!

Answer 2

add them all together

Answer 3

Let's add the masses of all the components involved in the reaction to see the overall mass balance.

1. Mass of silver residue: \(2.16 , \text{g}\)
2. Mass of CO2 produced: \(0.30 , \text{g}\)
3. Mass of O2 produced: \(0.30 , \text{g}\)

Now, we will add these together:

\[ \text{Total mass after reaction} = \text{mass of Ag} + \text{mass of CO}_2 + \text{mass of O}_2 \] \[ \text{Total mass after} = 2.16 , \text{g} + 0.30 , \text{g} + 0.30 , \text{g} \] \[ \text{Total mass after} = 2.76 , \text{g} \]

Including the mass of silver carbonate that decomposed:

4. Mass of silver carbonate: \(2.76 , \text{g}\)

So, we can also represent the entire mass balance using the initial and the produced products:

\[ \text{Total initial mass} = 2.76 , \text{g} \quad (\text{mass of silver carbonate}) \]

Adding the masses of all the products:

\[ \text{Total mass of products formed} = 2.16 , \text{g} , (\text{Ag}) + 0.30 , \text{g} , (\text{CO}_2) + 0.30 , \text{g} , (\text{O}_2) = 2.76 , \text{g} \]

Final Summary

• Total mass initially: \(2.76 , \text{g}\) of silver carbonate
• Total mass after reaction (sum of products): \(2.76 , \text{g}\)

Both the initial mass and the total mass after the reaction match, confirming the law of conservation of mass holds true in this reaction. If you need further assistance or calculations, feel free to ask!