Given the reaction system in a closed container at equilibrium and at a temperature of 298 k:
n2o4(g) < ==> 2no2(g)
the measurable quantities of the gases at equilibrium must be
(1) decreasing (3) equal
(2) increasing (4) constant

The measurable quantities of the gases at equilibrium must be constant

Explanation:

Measurable quantities for the gases at equilibrium includes rate of formation of , rate of formation of , pressure of and pressure of .

At equilibrium, rate of forward reaction is equal to rate of reverse reaction.

Rate of forward reaction infers rate of formation of and rate of backward reaction infers rate of formation of .

As rate of formations from both direction are equal therefore pressure of both gaseous species remains constant.

"you start with 15.67 g mgco3-xh2o, when heated and all the water is removed, you are left with 7.58 g mgco3 only.

therefore, you had 15.67 - 7.58 = 8.09g h2o  

moles of each :

7.58g mgco3 = ? moles = 7.58g / 83.4g/mole = 0.09moles  

8 09g h2o = ? moles = 8.09g / 18g/mole = 0.44moles  

molar ratio between the two by dividing both numbers by the smallest number :

0.09 / 0.09 = 1  

0.44 / 0.09 = 4.8  

mgco3-5h2o"