Calculate the volume of Hydrogen liberated when 0.75 amp of current flows for 45 mins through a metallic salt at NTP
Answers
Answer : The volume of hydrogen gas obtained at STP is 0.0836 L or 83.6 mL
Explanation :
When a current is passed through acidified water, it causes decomposition of water into H2 and O2.
The decomposition equation is given below.
Reaction at Cathode :
Reaction at Anode :
Overall reaction :
Step 1 : Find the amount of charge passed through the solution.
The number of coulombs can be calculated using following equation.
Step 2 : Find moles of electrons transferred using the coulomb value
According to Faraday's law, 1 mole of electrons carry a charge of 96485 coulombs.
Let us use this to find the moles of electrons carrying a charge of 720 coulombs.
Moles of electrons transferred is 0.00746
Step 3 : Use the mole ratio of electrons and H2 gas to find the number of moles of the gas released
The mole ratio of H2 and electrons is 1 : 2 according to the reduction reaction that occurs at the cathode
Step 4 : Use Ideal gas law and STP conditions to find the volume of the gas.
At STP, 1 mole of any gas occupies 22.4 L of volume.
We have 0.00373 mol.
The volume of hydrogen gas obtained at STP is 0.0836 L or 83.6 mL
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