Question

# The water is electrolysed in a cell , hydrogen is liberated at one electrode and oxygen is simultaneously liberated at the other . in a particular experiment hydrogen and oxygen so produced were collected together and the total volume measured 16.8 mL at NTP . How many coulombs were passed through the cell in the experiment ?

Solution

## $$W_{H_{2}} = Z_{H_{2}} Q...(1)$$$$W_{O2} =Z_{O2} Q...(2)$$$$(1)\Rightarrow W_{H_2} = \dfrac{gm\;eq\; wt\; of H_{2}}{96500}\times Q\dfrac{mole \;wt}{\dfrac{2}{96500}\times Q}$$ $$\Rightarrow \dfrac{W_{H2}}{M_{H2}}= \dfrac{Q}{2\times 96500} \Rightarrow n_{H2}=\dfrac{Q}{96500\times 2}$$$$\Rightarrow VH\times V_{H2}=\dfrac{2}{96500\times 2} \times 22400 ml$$$$for O_{2}$$$$WO_{2} = \dfrac{gm eg wt O_{2}}{96500}\times Q= \dfrac{mol wt O_{2}}{\dfrac{4}{96500}}\times Q$$$$\Rightarrow \dfrac{W_{02}}{MO_{2}} = \dfrac{Q}{96500\times 4} \therefore no_{2} = \dfrac{Q}{96500\times 4}$$$$\Rightarrow Vo_{2}=no_{2}\times 22400 ml =\dfrac{Q\times 22400}{96500\times 4}$$$$A/q , VH_{2}+VO_{2} = \times \dfrac{Q\times 22400}{96500\times 2}+\dfrac{Q\times 22400}{96500\times 4}$$$$16.8 = \dfrac{Q}{965} (112+56) =\dfrac{Q}{965}\times 168$$$$Q = \dfrac{16.8\times 965}{16.8} = 96.5 coulombs$$Chemistry

Suggest Corrections

0

Similar questions
View More

People also searched for
View More