Is this question actually solvable? It was on a quiz I just took and I couldn't figure it out...
Equation is 2I2+2H2S <-> 4HI+2S2. Given: KC=2.33x10-5, 0.250 mol HI in a 2L flask. Same with S2. Want: Equilibrium concentration of I2.
So I set up the ice table after putting everything in molarity.
2I2 + 2H2S <-> 4HI + S2
0 0 .125 .125
+2x +2x -4x -x
2x 2x .125-4x .125-x
Plugged it into ratios:
[HI]4[S2] / [I2]2[H2S]2 = ((.125-4x)4(.125-x)) / (16x4) = 2.33x10-5 I assumed the 4x and x in the numerator would be small so that changed it to (.1255)/(16x4). Plugging and chugging, I end up with a value of somewhere near 0.54 = x. So 2x= 1.06. Now, that just didn't look right, but I couldn't figure how else to do this. Any help?
Ammonia decomposes at high temperatures. In an experiment to explore this behavior, 3.00 moles of gaseous NH3 were sealed in a rigid 1.50 L vessel. The vessel is heated at 800K and some of the NH3 decomposes in the following reaction: NH3 (g) ---> N2 (g) + 3H2 (g)
The system eventually reaches equilibrium and is to contain 2.18 moles of NH3. What are the values of Kc and Kp for this reaction at 700K.
A solution was prepared such that the initial concentrations of Cu+2 and CN- were 0.0120 M and 0.0400 M, respectively. these ions react according to the following equation - Cu2+ + 4CN- > Cd(CN)4 ^2-. Kc = 1.0 x 10^25. What will be the concentration of CN- at equilibrium?
I made an ICE table and plugged everything into Kc,
so 1.0 x 10^25 = x / (0.0120 - x)((.04-4x)^4), is that right so far?
Submitted by Spinnerphoenix on Fri, 2014-04-18 11:29
Mixtures of propan-2-ol and propanone can be spearated by distllation due to their different boiling points. Explain why these compounds have such different boiling points even though they have very similar molar masses.
when we deal with the raoult's law equation for an ideal solution of 2 ideal liquids which are volatile, do we have to use the number of moles at equilibrium to calculate the mole fraction of solvent in the solution? or can we use the initial number of moles ?
What are the equilibrium concentrations of [H3O+], [CN-] and [HCN] if the concentration of HCN before equilibrium is 1.0 M? Also, what is the pH of the solution? (Ka = 6.3x10-10) Write out the entire ICE table for full credit.
I have no idea how to approach the problem when you need to find the values BEFORE equilibrium! I'm only familiar with how to find the values at equilibrium. Please help!!!