no
2.60 moles
how many moles are there in 56.0 grams of silver nitrate?
2,888.10e15 molecules of AgNO3 equal 0,48.10e-8 moles.
7 mol
As shown by the ionic equation of the reaction, Zn (s) + 2 Ag+ (aq) --> 2 Ag (s) + Zn2+ (aq), each mole of zinc produces two moles of silver. Therefore, 1.30 moles of zinc will displace 2.60 moles of silver.
2.60 moles
how many moles are there in 56.0 grams of silver nitrate?
2,888.10e15 molecules of AgNO3 equal 0,48.10e-8 moles.
2.0^25 moles of silver nitrate is .0301 moles.
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.)
7 mol
No. moles = mass/molecular mass mass of silver nitrate = 169.88 7.25/169.88 = 0.042 moles/l but this is per 100ml so we need to multiply by 10 = 0.42m
As shown by the ionic equation of the reaction, Zn (s) + 2 Ag+ (aq) --> 2 Ag (s) + Zn2+ (aq), each mole of zinc produces two moles of silver. Therefore, 1.30 moles of zinc will displace 2.60 moles of silver.
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.
Ag+ = 50 x 0.05 = 2.5 millimoles CrO4^2- = 100 x 0.06 = 6 millimoles Ag2CrO4 moles = 1.25 x 10^-3 moles formed.
It depends on the strength of the solution you want. 3.33g of AgNO3 is 0.0196 moles. Ish. So from there, you need to work out how much water is needed to create your required strength. 1.42 moles of silver nitrate is the maximum you can dissolve in 100g of water.
2,5 moles of silver is equal to 269,6705 g.