textbook 5I25

[Isabelle Rieke-Wey 2G]

"A reaction mixture is prepared by mixing 0.100 mol SO2, 0.200 mol NO2, 0.100 mol NO, and 0.150 mol SO3 in a reaction vessel of volume 5.00 L. The reaction SO2(g) 1 NO2(g) ∆ NO(g) 1 SO3(g) is allowed to reach equilibrium at 460 8C, when Kc 5 85.0. What is the equilibrium concentration of each substance?"
Does anyone know how to set up this problem to find the concentrations? Thanks!

[Ayaan_Ekram_2J]

Hello!

For this problem, you should set up an ICE table where the reactants are on the left and the products are on the right. The process for completing the ICE table is the same as when we are only given reactants, however the initial concentrations are no longer zero for the products but the given values. You would then use the ICE tables and the equilibrium expressions to set the (products)/(reactants) equal to Kc and solve for the x. Once you get x, you can solve for the concentration of each substance at equilibrium. I hope this helps!

[405745446]

For this problem, you'll need to be careful on how you set up your ICE table, this is where my struggle with the problem came from with this problem. You're given the initial condition of all the products and reactants. So your I row should be filled. Next, the most important part, is determining what to put for the c row, the reactants should have a "-x" and the products should have a "+x", so your E row should look something like 0.02-x, 0.04 -x, 0.02 +x, 0.03 +x. The values are just the initial conditions converted into molarity. And then you solve the equation algebraically like any other problem with it set up like, (0.02+x)(0.03+x)/ (0.02-x)(0.04-x) = 85.0. Then solve for x. Hopefully this helps explaining how to set up the problem.