A. To convert 2.33g of Na2CO3 to Ag2CO3, we first need to calculate the molar mass of Na2CO3 and Ag2CO3.
Molar mass of Na2CO3:
Na: 22.99 g/mol
C: 12.01 g/mol
O: 16.00 g/mol
Molar mass of Na2CO3 = (2 x 22.99) + 12.01 + (3 x 16.00) = 105.99 g/mol
Next, we need to 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 x 107.87) + 12.01 + (3 x 16.00) = 275.75 g/mol
Now we calculate the moles of Na2CO3:
moles = mass / molar mass
moles = 2.33g / 105.99 g/mol = 0.022 moles
Now, using the stoichiometry of the reaction, we see that 1 mole of Na2CO3 reacts with 2 moles of AgNO3 to form 1 mole of Ag2CO3. Therefore, the moles of AgNO3 needed to convert 0.022 moles of Na2CO3 to Ag2CO3 is 0.044 moles.
Finally, we calculate the mass of AgNO3 needed:
mass = moles x molar mass
mass = 0.044 moles x 169.87 g/mol (molar mass of AgNO3) = 7.47g
Therefore, 7.47g of AgNO3 is needed to convert 2.33g of Na2CO3 to Ag2CO3.
B. Once the reaction occurs, all of the AgNO3 will react to form Ag2CO3. Therefore, the mass of Ag2NO3 formed will be equal to the mass of AgNO3 used, which is 7.47g.
A.WHAT MASS OF AGNO3 IS NEEDED TO CONVERT THE 2.33g OF NA2CO3 TO AG2CO3.
B.WHAT MASS OF AG2NO3 WILL FORMED
1 answer