Silver sulfadiazine burn-treating cream creates a barrier against bacterial invasion and releases antimicrobial agents directly into the wound. If 20.0 g is reacted with 40.0 g , what mass of silver sulfadiazine, , can be produced, assuming 100% yield?

We will produce 57.1 grams of silver sulfadiazine

Explanation:

Silver sulfadiazine burn-treating cream creates a barrier against bacterial invasion and releases antimicrobial agents directly into the wound. If 20.0 g of Ag2O is reacted with 40.0 of C10H10N4SO2, what mass of silver sulfadiazine (AgC10H9N4SO2) can be produced assuming 100% yield?

Step 1: Data given

Mass of Ag2O = 20.0 grams

Molar mass of Ag2O = 231.735 g/mol

Mass of C10H10N4SO2 = 40.0 grams

Molar mass of C10H10N4SO2 = 250.277 g/mol

Step 2: The balanced equation

Ag2O + 2C10H10N4SO2 → 2AgC10H9N4SO2 + H2O

Step 3: Calculate moles Ag2O

Moles Ag2O = mass Ag2O / molar mass Ag2O

Moles Ag2O = 20.0 grams / 231.735 g/mol

Moles Ag2O = 0.0863 moles

Step 4: Calculate moles C10H10N4SO2

Moles C10H10N4SO2 = 40.0 grams / 250.277 g/mol

Moles C10H10N4SO2 = 0.160 moles

Step 5: Calculate the limiting reactant

For 1 mol Ag2O we need 2 moles 2C10H10N4SO2 to produce 2 moles AgC10H9N4SO2 and 1 mol H2O

C10H10N4SO2 is the limiting reactant. There will react 0.160 moles.

Ag2O is in excess. There will react 0.160/ 2 = 0.080 moles

There will remain 0.0863 - 0.080 = 0.0063 moles Ag2O

Step 5: Calculate moles AgC10H9N4SO2

For 1 mol Ag2O we need 2 moles 2C10H10N4SO2 to produce 2 moles AgC10H9N4SO2 and 1 mol H2O

For 0.160 moles C10H10N4SO2 we'll have 0.160 moles AgC10H9N4SO2

Step 6: Calculate mass AgC10H9N4SO2

Mass AgC10H9N4SO2 = moles * molar mass

Mass AgC10H9N4SO2 = 0.160 moles * 357.137 g/mol

Mass AgC10H9N4SO2 = 57.1 grams

We will produce 57.1 grams of silver sulfadiazine

the ideal gas law equation is as follows

pv = nrt

where p - pressure

v - volume

n - number of moles

r - universal gas constant

t - temperature

so if the pressure, volume and temperature are already known

we are left with n and r

since r is the universal gas constant that has a known fixed value then r too is known

so we are left with 'n'

once we know temperature volume and pressure

we can find the number of moles of gas present using the ideal gas law equation

this is not my own answer, this is an answer for the same question by the user blahblahmali. i do not claim ownership of this account.