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Monica [59]
3 years ago
15

What mass of silver oxide, Ag2O is required to produce 25.0 g of silver sulfadiazine, AgC10H9N4SO2, from the reaction of silver

oxide and sulfadiazine?
2C10H10N4SO2 + Ag2O ? 2AgC10H9N4SO2 + H2O
Chemistry
1 answer:
Wittaler [7]3 years ago
4 0

Answer:

8.1107 g

Explanation:

The given reaction:

2C_{10}H_{10}N_4SO_2+Ag_2O\rightarrow 2AgC_{10}H_9N_4SO_2+H_2O

Given that:

Mass of silver sulfadiazine = 25.0 g

Molar mass of silver sulfadiazine = 357.14 g/mol

The formula for the calculation of moles is shown below:

moles = \frac{Mass\ taken}{Molar\ mass}

Thus,

Moles= \frac{25.0\ g}{357.14\ g/mol}

Moles= 0.07\ mol

From the reaction,

2 moles of silver sulfadiazine are formed from 1 mole of silver oxide

So,

1 mole of silver sulfadiazine are formed from 1/2 mole of silver oxide

0.07 mole of silver sulfadiazine are formed from 1/2*0.07 mole of silver oxide

Moles of silver oxide = 0.035 moles

Molar mass  of silver oxide = 231.735 g/mol

Mass = Moles * Molar mass = 0.035 moles * 231.735 g/mol = 8.1107 g

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according to this hydrocyanic acid is weak acid so the corresponding conjugate base i.e. cyanide ion is strongest conjugate base.

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3 years ago
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