What mass of Ag2O is required to produce 25.0 g of silver sulfadiazine from the reaction of silver oxide and sulfadiazine?
2C10H10N4SO2 + Ag2O ==> 2AgC10H9N4SO2 + H2O
8.11
1. Convert 25.0 g silver sulfadiazine to mols. Remember mols = g/molar mass.
2. Use the equation coefficients to convert mols silver sulfadiazine to mols Ag2O.
3. Convert mols Ag2O to grams using mols x molar mass = grams.
check my thinking.
Post your work if you get stuck.
8.110789883... 8.1
I got 8.11, don’t stay up the night before again !!
To find the mass of Ag2O required to produce 25.0 g of silver sulfadiazine, we need to use stoichiometry and the molar ratios present in the balanced chemical equation.
The balanced chemical equation is:
2C10H10N4SO2 + Ag2O → 2AgC10H9N4SO2 + H2O
From the equation, we can see that 1 mole of Ag2O reacts with 2 moles of AgC10H9N4SO2. This means the molar ratio between Ag2O and AgC10H9N4SO2 is 1:2.
1. Calculate the molar mass of AgC10H9N4SO2:
The molar mass can be calculated by adding up the atomic masses of each element in the formula:
Ag - 1 x 107.87 g/mol = 107.87 g/mol
C - 10 x 12.01 g/mol = 120.10 g/mol
H - 9 x 1.01 g/mol = 9.09 g/mol
N - 4 x 14.01 g/mol = 56.04 g/mol
S - 1 x 32.07 g/mol = 32.07 g/mol
O - 2 x 16.00 g/mol = 32.00 g/mol
Total: 357.17 g/mol
2. Calculate the number of moles of AgC10H9N4SO2 produced:
Divide the given mass (25.0 g) of AgC10H9N4SO2 by its molar mass (357.17 g/mol):
25.0 g / 357.17 g/mol = 0.070 moles
3. Determine the moles of Ag2O needed:
Using the mole ratio from the balanced equation, we know that 2 moles of AgC10H9N4SO2 are produced from 1 mole of Ag2O. Therefore, we need twice the moles of AgC10H9N4SO2 (0.070 mol) to find the moles of Ag2O required:
0.070 mol x 1 mol Ag2O / 2 mol AgC10H9N4SO2 = 0.035 mol Ag2O
4. Calculate the mass of Ag2O:
Multiply the moles of Ag2O by its molar mass (231.74 g/mol) to find the mass:
0.035 mol Ag2O x 231.74 g/mol = 8.11 g
Therefore, 8.11 g of Ag2O is required to produce 25.0 g of silver sulfadiazine.