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)⟶2AgC10H9N4S O2(s)+H2O(l)

The mass of produced is 21.13 grams

Explanation:

To calculate the number of moles, we use the equation:

    .....(1)

Given mass of silver (I) oxide = 3.024 g

Molar mass of silver (I) oxide = 102.1 g/mol

Putting values in equation 1, we get:

Given mass of = 50.0 g

Molar mass of = 250 g/mol

Putting values in equation 1, we get:

The chemical equation for the combustion of hexane follows:

By Stoichiometry of the reaction:

1 mole of silver (I) oxide reacts with 2 moles of

So, 0.0296 moles of silver (I) oxide will react with = of

As, given amount of is more than the required amount. So, it is considered as an excess reagent.

Thus, silver (I) oxide is considered as a limiting reagent because it limits the formation of product.

By Stoichiometry of the reaction:

1 mole of silver (I) oxide produces 2 moles of

So, 0.0296 moles of silver (I) oxide will produce = of

Now, calculating the mass of  from equation 1, we get:

Molar mass of  = 357 g/mol

Moles of  = 0.0592 moles

Putting values in equation 1, we get:

Hence, the mass of produced is 21.13 grams

pie chart because it is in percents ( % )

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