Silver tarnishes in the presence of hydrogen sulfide according to the given balanced equation. What mass (g) of "tarnish" (Ag2S) is produced when 205.96 g of Ag react completely
Silver tarnishes in the presence of hydrogen sulfide according to the given balanced equation. What mass (g) of "tarnish" (Ag2S) is produced when 205.96 g of Ag react completely
Chapter3: Stoichiometry
Section: Chapter Questions
Problem 164CP: Nitric acid is produced commercially by the Ostwald process, represented by the following equations:...
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Silver tarnishes in the presence of hydrogen sulfide according to the given balanced equation. What mass (g) of "tarnish" (Ag2S) is produced when 205.96 g of Ag react completely? Give your answer to 2 decimal places.
4 Ag + 2 H2S + O2 ==> 2 Ag2S + 2 H2O
Molar Mass, g/mol | |
Ag | 107.9 |
H2S |
34.08 |
O2 |
32.00 |
Ag2S |
247.80 |
H2O |
18.02 |
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