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

first ans is wrong sorry, this question looked similar to one i answered a while ago

Answer 2

the ans is probably "The equilibrium between the two forms of the gas is disturbed at high temperatures."

Answer 3

because the gas gained a deeper color meaning the equilibrium shifted to the right when heated meaning it was disturbed

Answer 4

So D.)

Answer 5

well u never specified A B C or D

Answer 6

you only gave 4 options

Answer 7

The last option

Answer 8

yes

Answer 9

Ok thanks!