A) low pressure
B) high pressure
C) high temperature
D) low temperature
Correct Answer: A
Solution :
For a reaction, we know that \[{{K}_{p}}={{K}_{c}}{{(RT)}^{\Delta {{n}_{g}}}}\] where \[\Delta {{n}_{g}}\]= Number of gaseous moles of product - Number of gaseous moles of reactant Hence, if \[{{K}_{p}}>{{K}_{c}}\], then An must be positive. It means that there is a decrease in volume of reaction, hence low pressure will favour the forward reaction.You need to login to perform this action.
You will be redirected in
3 sec