| The electrolysis of acetate solution produces ethane according to reaction: |
| \[2C{{H}_{3}}CO{{O}^{-}}\xrightarrow{{}}{{C}_{2}}{{H}_{6}}(g)+2C{{O}_{2}}(g)+2{{e}^{-}}\] |
| The current efficiency of the process is 80%. What volume of gases would be produced at \[\text{27}{}^\circ \text{C}\] and 740 torr, if the current of 0.5 A is passed through the solution for 96.45 min? |
A) 6.0 L
B) 0.60 L
C) 1.365 L
D) 0.91 L
Correct Answer: D
Solution :
| [d] Equivalents of \[C{{O}_{2}}\] produced \[=\frac{\left( I\times \eta \right)\times t}{96500}\] |
| \[=\frac{0.5\times 0.8\times 96.5\times 60}{96500}=0.024\] |
| Moles of \[C{{O}_{2}}(n=1)\] produced = 0.024 |
| Moles of \[{{C}_{2}}{{H}_{6}}\left( n=2 \right)\] produced |
| \[=\frac{0.024}{2}=0.012\] |
| Total moles of gases produced = 0.036 |
| \[{{V}_{gases}}=\frac{nRT}{P}=\frac{0.036\times 0.0821\times 300}{\left( \frac{740}{760} \right)}=0.91L\] |
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