Which of the following statements about the equilibrium is false?

H2(g) + I2(s) = 2HI + 68.0 kJ/mol


[A] If the system is heated, the right side is favored.


[B] This is a heterogeneous equilibrium.


[C] If the pressure on the system is increased by changing the volume, the left side is favored.


[D] Adding more H2(g) increases the equilibrium constant.


[E] Removing HI as it forms forces the equilibrium to the right.Which of the following statements about the equilibrium is false?
The reaction is exothermic (left to right) so increasing the temperature overall would tend to favour the reverse endothermic (right to left) reaction since it must absorb a net amount of energy equal to 68.0 kJ/mol to complete, although this is complicated further when considering how the reverse mechanism, specifically, may proceed.Which of the following statements about the equilibrium is false?
We've just been doing this in chemistry sooo I think C is false.





Because increasing the pressure would cause the equilibrium to swing to the right to try to decrease the pressure. (As there are more gaseous atoms on the left side).
A. Adding heat will cause the reaction's equilibrium possition to shift to the left, by le chatelier;s principle.
A, C and D

computer security