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AgNO3 + NaCl ===> AgCl(s) + NaNO37 moles silver nitrate will produce 7 moles of silver chloride provided there is sufficient (at least 7 moles) of sodium chloride.
7 mol
.44 moles BeCl2
Since the four named compounds are the only reactants and products, this question can be answered from the law of conservation of mass: The amount of silver nitrate must be 14.35 + 8.5 - 5.85 or 17.0 grams.
no
Since both chloride anions and nitrate anions have a charge of -1, there will be the same number of moles of silver chloride produced as the moles of silver nitrate reacted. (Since both silver nitrate and silver chloride are ionic compounds, it would be preferable to call their "moles" "formula units" instead.)
AgNO3 + NaCl ===> AgCl(s) + NaNO37 moles silver nitrate will produce 7 moles of silver chloride provided there is sufficient (at least 7 moles) of sodium chloride.
7 mol
To determine the mass of silver chloride produced, we need to know the balanced chemical equation for the reaction between silver nitrate (AgNO3) and sodium chloride (NaCl) that produces silver chloride (AgCl) as a precipitate. Once we have the balanced equation, we can use the stoichiometry of the reaction to determine the number of moles of AgCl produced, and then convert that to mass using the molar mass of AgCl.
.44 moles BeCl2
6
Since the four named compounds are the only reactants and products, this question can be answered from the law of conservation of mass: The amount of silver nitrate must be 14.35 + 8.5 - 5.85 or 17.0 grams.
3,75 moles barium chloride
there are two moles produced in potassium nitrate.
2.0^25 moles of silver nitrate is .0301 moles.
no
2.60 moles