Consider the reaction H2(g) + Cl2(g) <=> 2 HCl(g), which is exothermic as written. What would be the effect on the equilib

Question

vampirchik [111]

4 years ago

9

Consider the reaction H2(g) + Cl2(g) <=> 2 HCl(g), which is exothermic as written. What would be the effect on the equilib

rium position of decreasing the volume of the reaction container?

Chemistry

2 answers:

lilavasa [31] · Answer 1 · 2021-12-30T08:46:36+03:00

lilavasa [31]4 years ago

7 0

Answer:

no effect

good luck hun

Explanation:

kirill115 [55] · Answer 2 · 2021-12-30T06:53:51+03:00

Answer:

No effect

Explanation:

H2(g) + Cl2(g) <=> 2HCl(g)

Decreasing the volume of the re simply means increasing the pressure. As we can see from the above equation, the total number of moles of the reactants and products are the same. There decreasing the volume ( i.e increaing the pressure) will have no effect on the system and hence the equilibrium position is not affected.