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rosijanka [135]
3 years ago
13

What we call "tin cans" are really iron cans coated with a thin layer of tin. The anode is a bar of tin and the cathode is the i

ron can. An electrical current is used to oxidize the Sn to Sn2+ in solution, which is reduced to produce a thin coating of Sn on the can.
Chemistry
1 answer:
UNO [17]3 years ago
6 0

Answer:

Fe (s) + Sn^{2+} (aq)\rightarrow Fe^{2+} (aq) + Sn (s)

Explanation:

Although the context is not clear, let's look at the oxidation and reduction processes that will take place in a Fe/Sn system.

The problem states that anode is a bar of thin. Anode is where the process of oxidation takes place. According to the abbreviation 'OILRIG', oxidation is loss, reduction is gain. Since oxidation occurs at anode, this is where loss of electrons takes place. That said, tin loses electrons to become tin cation:

Sn (s)\rightarrow Sn^{2+} (aq) + 2e^-

Similarly, iron is cathode. Cathode is where reduction takes place. Reduction is gain of electrons, this means iron cations gain electrons and produce iron metal:

Fe^{2+} (aq) + 2e^-\rightarrow Fe (s)

The net equation is then:

Sn (s) + Fe^{2+} (aq)\rightarrow Fe (s) + Sn^{2+} (aq)

However, this is not the case, as this is not a spontaneous reaction, as iron metal is more reactive than tin metal, and this is how the coating takes place. This implies that actually anode is iron and cathode is tin:

Actual anode half-equation:

Fe (s)\rightarrow Fe^{2+} (aq) + 2e^-

Actual cathode half-equation:

Sn^{2+} (aq) + 2e^-\rightarrow Sn (s)

Actual net reaction:

Fe (s) + Sn^{2+} (aq)\rightarrow Fe^{2+} (aq) + Sn (s)

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How many grams of sulfuric acid are needed to produce 57.0 grams of water? Show all steps of your calculation as well as the fin
antiseptic1488 [7]

Answer:

155.16 g.

Explanation:

  • Firstly, It is considered as a stichiometry problem.
  • From the balanced equation: 2NaOH + H₂SO₄ → 2Na₂SO₄ + 2H₂O
  • It is clear that the stichiometry shows that 2.0 moles of NaOH reacts with 1.0 mole of H₂SO₄ to give 2.0 moles of Na₂SO₄ and 2.0 moles of H₂O.
  • We must convert the grams of water (57.0 g) to moles <em>(n = mass/molar mass)</em>.
  • n = (57.0 g) / (18.0 g/mole) = 3.1666 moles.
  • Now, we can get the number of moles of H₂SO₄ that is needed to produce 3.1666 moles of water.
  • <em>Using cross multiplication:</em>
  • 1.0 mole of H₂SO₄ → 2.0 moles of H₂O, <em>from the stichiometry of the balanced equation</em>.
  • ??? moles of H₂SO₄ → 3.1666 moles of H₂O.
  • The number of moles of H₂SO₄ that will produce 3.1666 moles of H₂O <em>(57.0 g)</em> is (1.0 x 3.1666 / 2.0) = 1.5833 moles.
  • Finally, we should convert the number of moles of H₂SO₄ into grams <em>(n = mass/molar mass)</em>.
  • Molar mass of H₂SO₄ = 98.0 g/mole.
  • mass = n x molar mass = (1.5833 x 98.0) = 155.16 g.
6 0
3 years ago
Read 2 more answers
According to the Brönsted-Lowry theory, an acid is ___
Zigmanuir [339]

Answer:

is a substance which donates an H^+ or a proton

8 0
2 years ago
Read 2 more answers
→
marin [14]

Answer:

[A]²

Explanation:

Since the formation is independent of D, D is 0 order.

Since a quadruples when it is doubled it can be written as

2A^X= 4

To find the unknown power we can assume A= 1 to make the math simple. So When a = 2 (Because you doubled it) raised to X power it will equal 4

so the unknown power is 2

Making the rate law

[a]²[b]⁰

or simply just

[A]²

8 0
3 years ago
Suppose that 273 of a substance displaces 26ml of water what is the substance
Llana [10]
273g/25 mL = 10.92 (that's the density)
What has a density of 10.92 grams/mL?  I don't know but I bet it's in your notes or on the worksheet.
3 0
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19. I accidentally mixed bleach and ammonia when cleaning one day. It released 55 liters of deadly chlorine (CI) gas. How many g
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55,000 grams
Hope this helps you out :)
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