Can someone help me figure out this problem...

Gaseous hydrogen bromide decomposes at elevated temperatures according to the following equation: 2HBr(g) yields H2(g) + Br2(g)
At a certain temperature a 2.00L flask is initially filled only with 0.600 of HBr. What is the value of Kc at that temperature if the flask contains 0.104 mol of H2 at equilibrium?

Question

Can someone help me figure out this problem...

Gaseous hydrogen bromide decomposes at elevated temperatures according to the following equation: 2HBr(g) yields H2(g) + Br2(g)
At a certain temperature a 2.00L flask is initially filled only with 0.600 of HBr. What is the value of Kc at that temperature if the flask contains 0.104 mol of H2 at equilibrium?

anonymous · Answer

(0.104/(0.600-2*0.104))^2
Solve this equation and you will get your answer.

anonymous · Answer

(0.104 / (0.600 - (2 * 0.104)))^2 =  0.0704?

anonymous · Answer

Thanks

anonymous · Answer

How did you go about setting up the problem?

anonymous · Answer

By the way, this question is in the wrong section.

anonymous · Answer

Isnt this the chemistry section?

anonymous · Answer

No, this is English.

anonymous · Answer

Sorry