For the chemical equilibrium...

For the chemical equilibrium:
H2(g) + I2(g) <---> 2HI(g) K= 80 at 700 degrees celcius K= 64 at 800 degrees celcius

For this equilibrium:
a) The forward reaction is endothermic
b) An increase in the container volume increases the relative amount of HI
c) Removing I2 from the equilibrium system would icrease the relative amount of H2
d) if Q = 90 for an initial mix of H2, I2 and HI at 800 degrees celcius; more HI will be produced
e) none of the above is true.

The value of the equilibrium is higher at a lower temperature. That means increasing the temperature favors the reverse reaction. Therefore, the reverse reaction is endothermic and the forward reaction is exothermic. So a is incorrect.

This reaction has two gas molecules in the products and two gas molecules in the reactants. Changes in pressure/volume will not shift the equilibrium of this reaction, and b is incorrect.

C is correct. If you remove I2 from the equilibrium system, the forward reaction will be slowed. The reverse reaction will dominate for a while, replacing some of the I2 that was removed and increasing the relative amount of H2 as equilibrium is gradually re-established.

D is false. If Q>K, then the reverse reaction will dominate until equilibrium is established.