contestada

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?

Respuesta :

kenmyna
step  one write  the chemical   equation  for  reaction
=  Ag2O  +  2(C10H10N4SO2)---> 2 ( AgC10H9N4SO2)

The   reacting  ratio  of  Ag2O  to  AgC10H9N4SO2  is  1:2  from   the  reaction  above
    
step  2;  find  the  number  of  moles  of  AgC10H9N4SO2
that is  mass/molar  mass
The  molar  mass  of  AgC10H9N4SO2  =  107.86  +(12 x10) + (1 x 9) +  (4 x  14) +32 +(16 x2) =356.86g/mol
moles  is  therefore=  25g/356.86g/mol=  0.07moles

by  use  of  mole  ratio  the  moles   of  Ag2O=  0.0702=0.035moles
mass  =  moles x  molar  mass
the  molar  mass  of  Ag2O=231.72 g/mol
mass  is therefore=  231.72g/mol  x  0.035moles= 8.11grams

Eduard22sly

The mass of Ag₂O required to produce 25 g of silver sulfadiazine, AgC₁₀H₉N₄SO₂ is 8.12 g.

We'll begin by writing the balanced equation for the reaction. This is given below:

Ag₂O + 2C₁₀H₁₀N₄SO₂ → 2AgC₁₀H₉N₄SO₂ + H₂O

Molar mass Ag₂O = (108×2) + 16 = 232 g/mol

Mass of Ag₂O from the balanced equation = 1 × 232 = 232 g

Molar mass of AgC₁₀H₉N₄SO₂ = 108 + (12×10) + (1×9) + (14×4) + 32 + (16×2)

= 357 g/mol

Mass of AgC₁₀H₉N₄SO₂ from the balanced equation = 2 × 357 = 714 g

From the balanced equation above,

232 g of Ag₂O reacted to produce 714 g of AgC₁₀H₉N₄SO₂

  • With the above information, we can obtain the mass of Ag₂O required to 25 g of AgC₁₀H₉N₄SO₂. This can be obtained as follow:

From the balanced equation above,

232 g of Ag₂O reacted to produce 714 g of AgC₁₀H₉N₄SO₂

Therefore,

X g of Ag₂O will react to produce 25 g of AgC₁₀H₉N₄SO₂ i.e

X g of Ag₂O = [tex]\frac{232 * 25}{714} \\\\[/tex]

X g of Ag₂O = 8.12 g

Thus, the mass of Ag₂O required to produce 25 g of AgC₁₀H₉N₄SO₂ is 8.12 g.

Learn more: https://brainly.com/question/25248271

Otras preguntas