Hey guys!
Does change in pressure have any effect on the equilibrium if NOT all the reactants and products are in gaseous states? (Answer is B)
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Hi!
1). Adding a catalyst doesn’t increases the yield, it just speeds up the time taken to reach equilibrium.
2).Adding more NH3 will cause the reaction to move forward to reduce the ammonia concentration; this will increase the yield of the salt.
3).By increasing the pressure the equilibrium will shift to the side with fewer gaseous moles which is the product side so, the yield will increase.
4).The reaction is exothermic in forward direction so, by increasing the temperature the equilibrium will shift to try and decrease the temperature by moving toward the endothermic direction, which is the backward direction. This will decrease the yield.
The answer is thus B only 2&3.
If in a particular reaction we have any component which is gaseous then the pressure will have it’s effect just like we saw here the salt was solid but the reactants were in gaseous phase. So, increasing the pressure had the effect on overall yield.
But let’s assume we have a reaction where every component involved is in solid state then increasing or decreasing the pressure will have no effect.
Hope it helps:)
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Thank you so much Ujjwal! I must remember that changing the pressure will affect the reaction if it contains any gases.
Btw, if we would have a reaction where 1 mol of gas reactant decomposes into 2 mols of solid product, would an increase in pressure cause formation of more solid product?
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Hi!
Yup it will favor the formation of these solid products on the R.H.S of the equation cuz they have fewer gaseous moles compared to the reactants:)
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