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blagie [28]
3 years ago
6

Silver is often extracted from ores such as k[ag(cn)2] and then recovered by the reaction 2k ⎡ ⎣ag(cn)2 ⎤ ⎦(aq) + zn(s) ⟶ 2ag(s)

+ zn(cn)2 (aq) + 2kcn(aq) (a) how many molecules of zn(cn)2 are produced by the reaction of 35.27 g of k[ag(cn)2]? (b) what mass of zn(cn)2 is produced?
Chemistry
1 answer:
lions [1.4K]3 years ago
5 0
Take note of the whole number beside each substance in the reaction because these will be used in the stoichiometric calculations below:

Molar mass of <span>k[ag(cn)2]:199 g/mol
Molar mass of Zn(Cn)2: 117.44 g/mol
Avogadro's number: 6.022</span>×10²³ molecules/mol

a.)

35.27 g*(1 mol/199 g)*(1 mol Zn(Cn)₂/ 2 mol K[Ag(CN)₂])*(6.022×10²³ molecules/mol) = <em>5.34×10²² molecules of Zn(Cn)₂</em>

b.)

35.27 g*(1 mol/199 g)*(1 mol Zn(Cn)₂/ 2 mol K[Ag(CN)₂])*(117.44 g/mol) = <em>10.41 g of Zn(Cn)₂</em>
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