Respuesta :
The moles of silver nitrate required to form 0.854 mol silver ion has been 0.854 mol.
The balanced chemical equation for the dissolution of silver nitrate has been:
[tex]\rm AgNO_3\;\rightarrow\;Ag^+\;+\;NO_3^-[/tex]
The aqueous solution of silver nitrate has been dissociated into the constituent silver and nitrate ions.
In a balanced chemical equation, the coefficient has been equivalent to the moles of each reactant forming the moles of product.
From, the balanced equation,
[tex]\rm 1\;mol\;AgNO_3=1\;mol\;Ag[/tex]
The given moles of Silver has been 0.854 mol. Thus, the moles of silver nitrate required has been given as:
[tex]\rm 1\;mol\;Ag^+=1\;mol\;AgNO_3\\0.854\;mol\;Ag^+=0.854\;\times\;1\;mol\;AgNO_3\\0.854\;mol\;Ag^+=0.854\;mol\;AgNO_3[/tex]
The moles of silver nitrate required to form 0.854 mol silver ion has been 0.854 mol.
For more information about the moles produced, refer to the link:
https://brainly.com/question/10606802
