Silver sulfadiazine burn-treating cream creates a barrier against bacterial invasion and releases antimicrobial agents directly into the wound. If 25.0 g of Ag2O is reacted with 50.0 g of C10H10N4SO2, what mass of silver sulfadiazine (AgC10H9N4SO2) can be produced, assuming 100% yield?Ag2O(s)+2C10H10N4SO2(s)⟶2AgC10H9N4SO2(s)+H2O(l)

[tex]\text{ Moles of }C_{10}H_{10}N_4SO_2=\frac{\text{ Mass of }C_{10}H_{10}N_4SO_2}{\text{ Molar mass of }C_{10}H_{10}N_4SO_2}=\frac{50.0g}{250.3g/mole}=0.1998moles[/tex]

Now we have to calculate the limiting and excess reagent.

The balanced chemical reaction is,

[tex]Ag_2O(s)+2C_{10}H_{10}N_4SO_2(s)\rightarrow 2AgC_{10}H_9N_4SO_2(s)+H_2O(l)[/tex]

From the balanced reaction we conclude that

As, 2 mole of [tex]C_{10}H_{10}N_4SO_2[/tex] react with 1 mole of [tex]Ag_2O[/tex]

So, 0.1998 moles of [tex]C_{10}H_{10}N_4SO_2[/tex] react with [tex]\frac{0.1998}{2}=0.0999[/tex] moles of [tex]Ag_2O[/tex]

From this we conclude that, [tex]Ag_2O[/tex] is an excess reagent because the given moles are greater than the required moles and [tex]C_{10}H_{10}N_4SO_2[/tex] is a limiting reagent and it limits the formation of product.

Now we have to calculate the moles of [tex]AgC_{10}H_9N_4SO_2[/tex]

From the reaction, we conclude that

As, 2 mole of [tex]C_{10}H_{10}N_4SO_2[/tex] react with 2 mole of [tex]AgC_{10}H_9N_4SO_2[/tex]

So, 0.1998 mole of [tex]C_{10}H_{10}N_4SO_2[/tex] react with 0.1998 mole of [tex]AgC_{10}H_9N_4SO_2[/tex]

Now we have to calculate the mass of [tex]AgC_{10}H_9N_4SO_2[/tex]

[tex]\text{ Mass of }AgC_{10}H_9N_4SO_2=\text{ Moles of }AgC_{10}H_9N_4SO_2\times \text{ Molar mass of }AgC_{10}H_9N_4SO_2[/tex]

[tex]\text{ Mass of }AgC_{10}H_9N_4SO_2=(0.1998moles)\times (357.1g/mole)=71.35g[/tex]

Therefore, the mass of silver sulfadiazine produced can be, 71.35 grams.