A) \[73.8\times {{10}^{10}}\]
B) \[7.38\times {{10}^{11}}\]
C) Both (a) and (b)
D) Zero
Correct Answer: C
Solution :
For the given reaction, \[\Delta {{n}_{g}}=2-3=-1\] \[{{K}_{p}}={{K}_{c}}{{(RT)}^{\Delta {{n}_{g}}}}\] or \[{{K}_{c}}={{K}_{p}}{{(RT)}^{-\Delta {{n}_{g}}}}\] or \[{{K}_{c}}={{K}_{p}}(RT)\] (After putting the value of \[\Delta {{n}_{g}}\]) \[=(2.0\times {{10}^{10}}ba{{r}^{-1}})(0.0821\,L\,bar\,{{K}^{-1}}\,mo{{l}^{-1}})\]\[\times (450K)\] \[=73.8\times {{10}^{10}}\,L\,\,mo{{l}^{-1}}\] or \[{{K}_{c}}=73.8\times {{10}^{11}}\,L\,\,mo{{l}^{-1}}\]
You need to login to perform this action.
You will be redirected in
3 sec
