Tarnishing of silver is caused by small amounts of hydrogen sulfide released into the atmosphere by decaying organic material and volcanic activity. Hydrogen sulfide's reaction with silver and atmospheric oxygen is as follows: 4 Ag (s) + 2 H2S (g) + O2 (g) -> 2 Ag2S (s) + 2 H2O (l) (tarnish) How many grams of Ag2S can be produced from 1.70g H2S if sufficient amounts of the other reactants are present?
Added by Santosh G.
Close
Step 1
The molar mass of hydrogen is approximately 1 g/mol and the molar mass of sulfur is approximately 32 g/mol. Therefore, the molar mass of H2S is (1*2) + 32 = 34 g/mol. Show more…
Show all steps
Your feedback will help us improve your experience
Anna D. and 56 other Chemistry 101 educators are ready to help you.
Ask a new question
Labs
Want to see this concept in action?
Explore this concept interactively to see how it behaves as you change inputs.
Key Concepts
Recommended Videos
Calculate the mass (g) of each product formed when 174 $\mathrm{g}$ of silver sulfide reacts with excess hydrochloric acid: $$ \mathrm{Ag}_{2} \mathrm{S}(s)+\mathrm{HCl}(a q) \longrightarrow \mathrm{AgCl}(s)+\mathrm{H}_{2} \mathrm{S}(g)[\text { unbalanced }] $$
Polishing Silver Silver tarnish is the result of silver metal reacting with sulfur compounds, such as $\mathrm{H}_{2} \mathrm{S}$, in the air. The tarnish on silverware $\left(\mathrm{Ag}_{2} \mathrm{S}\right)$ can be removed by soaking in a solution of $\mathrm{NaHCO}_{3}$ (baking soda) in a basin lined with aluminum foil. a. Write a balanced equation for the tarnishing of Ag to $\mathrm{Ag}_{2} \mathrm{S},$ and assign oxidation numbers to the reactants and products. How many electrons are transferred per mole of silver? b. Write a balanced equation for the reaction of $\mathrm{Ag}_{2} \mathrm{S}$ with Al metal, NaHCO $_{3},$ and water to produce Al(OH) $_{3}$ $\mathrm{H}_{2} \mathrm{S}, \mathrm{H}_{2},$ and $\mathrm{Ag}$ metal.
Silver sulfide, the tarnish on silverware, comes from the reaction of silver metal with hydrogen sulfide (H2S). The unbalanced equation is: Ag + H2S + O2 → Ag2S + H2O (unbalanced). If the reaction was used intentionally to prepare Ag2S, how many grams would be formed from 496 g of Ag, 80.0 g of H2S, and excess O2 if the reaction takes place in 90% yield?
Taimoor S.
Recommended Textbooks
Chemistry: Structure and Properties
Chemistry The Central Science
Chemistry
Transcript
18,000,000+
Students on Numerade
Trusted by students at 8,000+ universities
Watch the video solution with this free unlock.
EMAIL
PASSWORD