Zinc: Difference between revisions
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JeffEvarts (talk | contribs) (Created page with "{{Compound|name=Zinc|chemf=Zn|density=6.57|group=Transition Metals|num=30|stp_p=solid|stp_q=silver|mm=65.4|mp=419.5|bp=907|nfpa_h=2|nfpa_o=<s>W</s>}} ==Uses== ===Primary=== *...") |
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#: {{#Chem:Zn(v) { = ≤900°C } Zn(l) }} | #: {{#Chem:Zn(v) { = ≤900°C } Zn(l) }} | ||
# Gather the zinc from the lower (cooler) container | # Gather the zinc from the lower (cooler) container | ||
===Electrolysis=== | |||
====zinc sulfate==== | |||
Zinc sulfate can be electrolytically separated in [[sulfuric acid]], producing [[oxygen]] and ''excess sulfuric acid'' as a side stream. The reaction is fairly straightforward: | Zinc sulfate can be electrolytically separated in [[sulfuric acid]], producing [[oxygen]] and ''excess sulfuric acid'' as a side stream. The reaction is fairly straightforward: | ||
: {{#Chem: 2ZnSO4 + 2H2O { H2SO4 = 4.5v } 2Zn + 2H2SO4 + O2 }} | : {{#Chem: 2ZnSO4 + 2H2O { H2SO4 = 4.5v } 2Zn + 2H2SO4 + O2 }} | ||
Wikipedia offers some numbers on efficiency | Wikipedia offers some numbers on efficiency | ||
<blockquote>There are two common processes for electrowinning the metal. The former uses a 10% sulfuric acid solution as the electrolyte, with current density of 270–325 amperes per square meter. The latter uses 22–28% sulfuric acid solution as the electrolyte with a current density of about 1,000 amperes per square metre. The latter gives better purity and has higher production capacity per volume of electrolyte, but has the disadvantage of running hotter and being more corrosive to the vessel in which it is done. In either of the electrolytic processes, each metric ton of zinc production expends about 3.9 MW·h (14 GJ) of electric power.</blockquote> | <blockquote>There are two common processes for electrowinning the metal. The former uses a 10% sulfuric acid solution as the electrolyte, with current density of 270–325 amperes per square meter. The latter uses 22–28% sulfuric acid solution as the electrolyte with a current density of about 1,000 amperes per square metre. The latter gives better purity and has higher production capacity per volume of electrolyte, but has the disadvantage of running hotter and being more corrosive to the vessel in which it is done. In either of the electrolytic processes, each metric ton of zinc production expends about 3.9 MW·h (14 GJ) of electric power.</blockquote> | ||
====zinc chloride==== | |||
Zinc chloride can also be electrolyzed completely into zinc and [[chlorine]] | Zinc chloride can also be electrolyzed completely into zinc and [[chlorine]] | ||
: {{#Chem: ZnCl2 = Zn + Cl2 }} | : {{#Chem: ZnCl2 = Zn + Cl2 }} | ||
==Purification== | ==Purification== | ||
==Testing== | ==Testing== | ||
Latest revision as of 13:52, 25 June 2019
| Chemical formula | Zn |
|---|---|
| Atomic Number | 30 |
| OTP appearance | silver solid |
| Molar Mass(g/mol) | 65.4 |
| Density(g/cc) | 6.57 |
| Melting Point(°C) | 419.5 |
| Boiling Point(°C) | 907 |
| NFPA 704 |  0
2
0
|
Uses
Primary
- Essential element in brass
- Essential element for galvanizing steel
- Essential for multiple battery technologies
Secondary
- Sacrificial anode for boats
- -oxide as a skin protectant / cosmetic
Hazards
- Zinc and many of its compounds are toxic
Natural Sources
- Elemental zinc does occur naturally, but is exceedingly rare.
- The primary ores of zinc are hemimorphite, smithsonite, and sphalerite
- Nutritive zinc (sulfate, oxide, citrate, or ascorbate) is found in pumpkin, watermelon, and squash seeds.
Production
Extraction
India
- Gather two ceramic, one with a male and one with a female stem
- Place finely ground zinc ore in the male flask
- Place coarse charcoal in the male flask atop the zinc oxide
- (optional) place a small ceramic grate or porous plug in the male neck
- Join the male and female necks
- Arrange the flasks so that the male is above the female
- Heat the male flask to red heat while keeping the female flask cool
- ZnO + C{Zn(v) + CO + CO2800-1100°C}→
- Zn(v){Zn(l)≤900°C}→
- ZnO + C
- Gather the zinc from the lower (cooler) container
Electrolysis
zinc sulfate
Zinc sulfate can be electrolytically separated in sulfuric acid, producing oxygen and excess sulfuric acid as a side stream. The reaction is fairly straightforward:
- 2 ZnSO4 + 2 H2O{H2SO42 Zn + 2 H2SO4 + O24.5v}→
Wikipedia offers some numbers on efficiency
There are two common processes for electrowinning the metal. The former uses a 10% sulfuric acid solution as the electrolyte, with current density of 270–325 amperes per square meter. The latter uses 22–28% sulfuric acid solution as the electrolyte with a current density of about 1,000 amperes per square metre. The latter gives better purity and has higher production capacity per volume of electrolyte, but has the disadvantage of running hotter and being more corrosive to the vessel in which it is done. In either of the electrolytic processes, each metric ton of zinc production expends about 3.9 MW·h (14 GJ) of electric power.
zinc chloride
Zinc chloride can also be electrolyzed completely into zinc and chlorine
- ZnCl2 → Zn + Cl2