The mass of silver produced by thermal decomposition of 5.52g Ag2CO3
To determine the mass of silver produced by thermal decomposition of Ag2CO3, we need to consider the chemical equation for the reaction. The thermal decomposition of Ag2CO3 can be represented by the following equation:
2 Ag2CO3(s) → 4 Ag(s) + 2 CO2(g) + O2(g)
From this equation, we can see that every 2 moles of Ag2CO3 will produce 4 moles of Ag.
Now, let's calculate the molar mass of Ag2CO3:
Ag2CO3:
Ag: 2 * atomic mass of silver (107.87 g/mol) = 215.74 g/mol
C: atomic mass of carbon (12.01 g/mol)
O: 3 * atomic mass of oxygen (16.00 g/mol) = 48.00 g/mol
Total molar mass of Ag2CO3 = 215.74 + 12.01 + 48.00 = 275.75 g/mol
Now, we can calculate the number of moles of Ag2CO3 using the given mass:
Number of moles = Mass / Molar mass
Number of moles of Ag2CO3 = 5.52 g / 275.75 g/mol = 0.02 mol
Since 2 moles of Ag2CO3 produce 4 moles of Ag, we can calculate the number of moles of Ag produced by multiplying the number of moles of Ag2CO3 by 2:
Number of moles of Ag = 0.02 mol * 2 = 0.04 mol
Finally, let's calculate the mass of Ag produced by multiplying the number of moles of Ag by the molar mass of Ag:
Mass = number of moles * molar mass
Mass of Ag produced = 0.04 mol * 107.87 g/mol = 4.31 g
Therefore, the mass of silver produced by thermal decomposition of 5.52 g Ag2CO3 is approximately 4.31 grams.
To find the mass of silver produced by the thermal decomposition of Ag2CO3, we need to determine the molar mass of Ag2CO3 and use stoichiometry to calculate the mass of silver.
Step 1: Find the molar mass of Ag2CO3
The molar mass of Ag (silver) is approximately 107.87 g/mol, and the molar mass of CO3 (carbonate) is approximately 60.01 g/mol. Ag2CO3 consists of two Ag atoms and one CO3 group.
Molar mass of Ag2CO3 = (2 x molar mass of Ag) + molar mass of CO3
= (2 x 107.87 g/mol) + 60.01 g/mol
= 215.74 g/mol + 60.01 g/mol
= 275.75 g/mol
Step 2: Use stoichiometry to calculate the mass of silver
From the balanced chemical equation for the thermal decomposition of Ag2CO3, we know that 1 mole of Ag2CO3 produces 2 moles of Ag.
2 Ag2CO3(s) -> 4 Ag(s) + 2 CO2(g) + O2(g)
Using the molar mass of Ag2CO3, we can calculate the number of moles present in 5.52 g by dividing it by the molar mass.
Number of moles of Ag2CO3 = mass of Ag2CO3 / molar mass of Ag2CO3
= 5.52 g / 275.75 g/mol
≈ 0.020 moles (approximately)
Since the stoichiometric ratio between Ag2CO3 and Ag is 1:2, we can determine the number of moles of Ag produced.
Number of moles of Ag = 2 x number of moles of Ag2CO3
= 2 x 0.020 moles
= 0.040 moles
Finally, we can calculate the mass of silver produced by multiplying the number of moles of Ag by its molar mass.
Mass of Ag = number of moles of Ag x molar mass of Ag
= 0.040 moles x 107.87 g/mol
= 4.31 g
Therefore, the mass of silver produced by the thermal decomposition of 5.52 g Ag2CO3 is approximately 4.31 grams.