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The quantity of electricity required to liberate 112 cm3 of hydrogen at STP from acidified water is
- a)965 C
- b)1 Faraday
- c)0.1 F
- d)96500 C
Correct answer is option 'A'. Can you explain this answer?
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The quantity of electricity required to liberate 112 cm3 of hydrogen a...
Calculation of Quantity of Electricity Required
The liberation of hydrogen gas from acidified water involves the electrolysis of water, which can be represented by the following half-reaction:
2H2O(l) → 2H2(g) + O2(g)
Given Data:
Volume of hydrogen gas liberated = 112 cm3
Standard temperature and pressure (STP) conditions
Conversion of Volume to Moles of Hydrogen:
1 mole of any gas occupies 22.4 L at STP
112 cm3 = 112/1000 L = 0.112 L
0.112 L of hydrogen gas is equivalent to 0.112/22.4 = 0.005 moles of hydrogen gas
Calculation of Quantity of Electricity:
From the balanced equation, it is evident that 2 moles of electrons are required to liberate 1 mole of hydrogen gas.
Therefore, 1 mole of hydrogen gas requires 2 * 96485 C = 192970 C of electricity, which is equivalent to 1 Faraday.
Hence, 0.005 moles of hydrogen gas will require 0.005 * 192970 C = 965 C of electricity.
Therefore, the correct answer is 965 C.
The liberation of hydrogen gas from acidified water involves the electrolysis of water, which can be represented by the following half-reaction:
2H2O(l) → 2H2(g) + O2(g)
Given Data:
Volume of hydrogen gas liberated = 112 cm3
Standard temperature and pressure (STP) conditions
Conversion of Volume to Moles of Hydrogen:
1 mole of any gas occupies 22.4 L at STP
112 cm3 = 112/1000 L = 0.112 L
0.112 L of hydrogen gas is equivalent to 0.112/22.4 = 0.005 moles of hydrogen gas
Calculation of Quantity of Electricity:
From the balanced equation, it is evident that 2 moles of electrons are required to liberate 1 mole of hydrogen gas.
Therefore, 1 mole of hydrogen gas requires 2 * 96485 C = 192970 C of electricity, which is equivalent to 1 Faraday.
Hence, 0.005 moles of hydrogen gas will require 0.005 * 192970 C = 965 C of electricity.
Therefore, the correct answer is 965 C.
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The quantity of electricity required to liberate 112 cm3 of hydrogen at STP from acidified water isa)965 Cb)1 Faradayc)0.1 Fd)96500 CCorrect answer is option 'A'. Can you explain this answer?
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