the same amount of current was passed through acidic water and copper sulphate solution. It liberates 203 ml of hydrogen at NTP and deposited 0.578g of copper . calculate the equivalent weight of copper
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Please find below the solution to the asked query:
2H+ + e- ----> H2
As we know that, 1 mole of any gas occupies 22400 ml of volume, hence in 203 ml of hydrogen we have = (1/22400) x 203 = 0.009 moles of hydrogen.
Moles of copper reduced = 0.578 g / 63.5 g mol-1 = 0.009 moles of copper
As we know that, 2 moles of hydrogen ions are required to obtain 1 mole of hydrogen gas, then in 0.009 moles of hydrogen gas, moles of hydrogen ions required = 0.018 moles
Now, since for 0.009 moles of copper, twice the moles i.e. 0.018 moles of hydrogen ion are used in the reaction. The equivalance factor for copper is 2.
Hence, equivalent weight of copper = 63.5 / 2 = 31.75 g
Hope this information will clear your doubts about Electrochemistry.
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Please find below the solution to the asked query:
2H+ + e- ----> H2
As we know that, 1 mole of any gas occupies 22400 ml of volume, hence in 203 ml of hydrogen we have = (1/22400) x 203 = 0.009 moles of hydrogen.
Moles of copper reduced = 0.578 g / 63.5 g mol-1 = 0.009 moles of copper
As we know that, 2 moles of hydrogen ions are required to obtain 1 mole of hydrogen gas, then in 0.009 moles of hydrogen gas, moles of hydrogen ions required = 0.018 moles
Now, since for 0.009 moles of copper, twice the moles i.e. 0.018 moles of hydrogen ion are used in the reaction. The equivalance factor for copper is 2.
Hence, equivalent weight of copper = 63.5 / 2 = 31.75 g
Hope this information will clear your doubts about Electrochemistry.
If you have any doubts just ask here on the ask and answer forum and our experts will try to help you out as soon as possible.
Best Wishes !