To calculate the mass of AgNO3 needed to convert 2.33g of Na2CO3 to Ag2CO3, we first need to determine the molar mass of Na2CO3 and Ag2CO3.
1. Calculate the molar mass of Na2CO3:
Na: 22.99 g/mol
C: 12.01 g/mol
O: 16.00 g/mol
Molar mass of Na2CO3 = 2(22.99) + 12.01 + 3(16.00) = 45.98 + 12.01 + 48.00 = 105.99 g/mol
2. Calculate the molar mass of Ag2CO3:
Ag: 107.87 g/mol
C: 12.01 g/mol
O: 16.00 g/mol
Molar mass of Ag2CO3 = 2(107.87) + 12.01 + 3(16.00) = 215.74 + 12.01 + 48.00 = 275.75 g/mol
3. Calculate the molar mass of AgNO3:
Ag: 107.87 g/mol
N: 14.01 g/mol
O: 16.00 g/mol
Molar mass of AgNO3 = 107.87 + 14.01 + 3(16.00) = 107.87 + 14.01 + 48.00 = 169.88 g/mol
4. Use the stoichiometry of the reaction to calculate the mass of AgNO3 needed:
Na2CO3 + 2AgNO3 -> Ag2CO3 + 2NaNO3
From the balanced chemical equation, 1 mole of Na2CO3 reacts with 2 moles of AgNO3 to form 1 mole of Ag2CO3.
Number of moles of Na2CO3 = 2.33 g / molar mass of Na2CO3 = 2.33 g / 105.99 g/mol ≈ 0.022 moles
According to the stoichiometry, this would require 0.022 moles of AgNO3 to react with the Na2CO3.
Mass of AgNO3 needed = 0.022 moles x 169.88 g/mol ≈ 3.74 g
Therefore, 3.74 grams of AgNO3 is needed to convert 2.33 grams of Na2CO3 to Ag2CO3.
WHAT MASS OF AGNO3 IS NEEDED TO CONVERT THE 2.33g OF NA2CO3 TO AG2CO3
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