Question

Nitrogen dioxide gas is dark brown in color and remains in equilibrium with dinitrogen tetroxide gas, which is colorless.

2NO2(g) ⇌N2O4(g)

When the mixture was moved from room temperature to a higher temperature, the mixture turned darker brown. Which of the following conclusions about the mixture is true?

The forward reaction is exothermic.
The backward reaction has a negative net enthalpy.
The colorless gas has a higher enthalpy than the brown gas.
The equilibrium between the two forms of the gas is disturbed at high temperatures.

Answer 1

Is the answer A.) or D.)?

Answer 2

It's D. I'd assume. There's no way to prove that the reaction resulted in a release of heat, which would still constitute a chemical reaction. However, it's the most uncertain answer.

Answer 3

Nevermind. I completely overlooked the fact that it's shifted. It's A.

Answer 4

Ok you sure?

Answer 5

hey man forward reaction means it shifts to the right, the equilibrium shifted to the left?

Answer 6

well i guess its correct as well but id say D is better, cos if its exothermic that means it shifts to right

Answer 7

oh wait lol i read it wrong A is correct

Answer 8

cos if forward is exothermic n heat is added equili shift to right

Answer 9

Ight so its A.)