How muchmuch hydrogen gas evolvedwhen 1.5 current is passed through water for 1.5 hours?
1 answer:
0.042 moles of Hydrogen evolved
<h3>Further explanation</h3>Given
I = 1.5 A
t = 1.5 hr = 5400 s
Required
Number of Hydrogen evolved
Solution
Electrolysis of water ⇒ decomposition reaction of water into Oxygen and Hydrogen gas.
Cathode(reduction-negative pole) : 2H₂O(l)+2e⁻ ⇒ H₂(g)+2OH⁻(aq)
Anode(oxidation-positive pole) : 2H₂O(l)⇒O₂(g)+4H⁻(aq)+4e⁻
Total reaction : 2H₂O(l)⇒2H₂(g)+O₂(g)
So at the cathode H₂ gas is produced
Faraday : 1 mole of electrons (e⁻) contains a charge of 96,500 C
Q = i.t
Q = 1.5 x 5400
Q = 8100 C
mol e⁻ = 8100 : 96500 = 0.084
From equation at cathode , mol ratio e⁻ : H₂ = 2 : 1, so mol H₂ = 0.042
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<h2>The compound formed is NaCl and 
</h2>
Explanation:
PART 1:
- Atomic number of sodium is 11.
- Sodium(Na, Z = 11, Group 1A) will lose 1 electron to become
which is isoelectronic to Neon (Ne ,Z = 10).
- The symbol for the sodium ion is
.
- Chlorine atom (
, Z = 17, Group 7A or 17) gains 1 elecron to be isoelectronic to neon.
- The symbol for the compound formed is NaCl.
- PART 2:
- Atomic number of calcium is 20
- Calcium(Ca, Z = 20 ,Group 2A) will lose two electrons to become
which is isoelectronic to argon.
- The symbol for the ion is
- Two chlorine atoms (Cl, Z = 17, Group 7A or 17) each gains one electron to be isoelectronic to argon(Z = 18)
- The symbol for the compound formed is