Suppose a 500.mL flask is filled with 1.6mol of NO3 and 1.2mol of NO2 . The following reaction becomes possible: +NO3gNOg 2NO2g The equilibrium constant K for this reaction is 8.01 at the temperature of the flask. Calculate the equilibrium molarity of NO3 . Round your answer to two decimal places.

At equilibrium, the concentration of is 1.60 M

Explanation:

Initial values

We have the balanced chemical reaction is:

+ ⇄2

:

:

Equilibrium values

and  are going to consume, while is going to be produced until equilibrium is reached.

By the ICE (initial, change, equilibrium) analysis:

I: []=3.2M   ;     []= 2.4M    ; []=0

C:  []=-x   ;     []= -x   ; []=+2x

E:  []=3.2-x  ;     []= 2.4-x    ; []=0+2x

Now we can use the constant information:

K=8.01

Solving for x we have 1.6 and 9.6 as possible results. But 9.6 has no sense because the concentration left can not be negative. So x=1.6

It means that at equilibrium, the concentration of is going to be 1.6 M

in 1783 cavendish was working with his hydrogen gas and found that when he burned it and condensed the vapor it was water. this was very significant since it disproved the greek theory of elements completely since water was not a simple substance but the product of two gases. it was lavoisier who hearing of the experiment gave cavendish's gas the name hydrogen ("water-producer") and added that hydrogen burned by combining with oxygen and that water was a hydrogen-oxygen combination.

explanation: