According to the reaction below, how many grams of zinc, Zn, could react in 147.96 mL of 1.778 M AgNO3?
Zn(s) + 2 AgNO3(aq) → 2 Ag(s) + Zn(NO3)2(aq)
Molarity = 1.778 M
Volume = 147.96 mL = 0.14796 L
Moles = molarity X volume in L
n = 1.778 X 0.14796
n = 0.2631 mol
From the balanced equation given,
2 mol of silver nitrate needs 1 mol of zinc
Then,
0.2631 mol of silver nitrate needs 0.2631 / 2 = 0.1315 mol of zinc.
Moles of zinc = 0.1315 mol
Molar mass of zinc = 65.38 g/mol
Mass of zinc = moles X molar mass
m = 0.1315 X 65.38
m = 8.600 g.
Therefore,
Mass of zinc required = 8.600 g.
According to the reaction below, how many grams of zinc, Zn, could react in 147.96 mL...
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