A) forward direction because \[Q>{{K}_{C}}\]
B) reverse direction because \[Q>{{K}_{C}}\]
C) forward direction because \[Q<{{K}_{C}}\]
D) reverse direction because \[Q<{{K}_{C}}\]
Correct Answer: B
Solution :
[b] \[\Delta G=\Delta {{G}^{o}}+RT\]In Q \[=249.2+8.314\times 300\] In 4 =Positive \[\Delta G=RT\]In \[\frac{Q}{K}\] Since, \[\Delta G\]is positive so Q>K, so reaction shifts in reverse direction.
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