What will happen if more heat is applied to the following system at equilibrium?
X\(_2\)(g) + 3Y\(_2\)(g) ⇌ 2XY\(_3\)(g); ∆H = xKJmol\(^{-1}\)
the yield of XY 3 will decompose
more of XY3 will decompose
More of X2 will react
the forward reaction will remain static
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I don't think this is correct . the enthalpy change of that reaction is xkjmol-¹( that's shows it's endothermic)
increasing the temperature of an endothermic reaction will favour shift the equilibrium to the right. to annul it, more of the reactants will collide leading to the formation of more products.. please review.
X2(g) + 3Y2(g) ⇌ 2XY3(g); ∆H = xKJmol−1
As far as i can tell, the above reaction is clearly an exothermic reaction as such, increase in temperature favours the backward reaction.
Please @Myschool throw more light on this please
N² + 3H²=2NH³ an exothermic reaction
an increase in temperature would favour reactants formation
which is more N² and 3H² would react
there is no error it the same thing the equilibrum will shift to the right and what they choose
