Submitted by Batman17 on Wed, 20140924 21:40
Is this question actually solvable? It was on a quiz I just took and I couldn't figure it out...
Equation is 2I_{2}+2H_{2}S <> 4HI+2S_{2}. Given: K_{C}=2.33x10^{5}, 0.250 mol HI in a 2L flask. Same with S_{2}. Want: Equilibrium concentration of I_{2}.
So I set up the ice table after putting everything in molarity.
2I_{2 }+ 2H_{2}S <> 4HI + S_{2}
0 0 .125 .125
+2x +2x 4x x
2x 2x .1254x .125x
Plugged it into ratios:
[HI]^{4}[S_{2}] / [I_{2}]^{2}[H_{2}S]^{2} = ((.1254x)^{4}(.125x)) / (16x^{4}) = 2.33x10^{5} I assumed the 4x and x in the numerator would be small so that changed it to (.125^{5})/(16x^{4}). 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?
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Submitted by wnterhorst on Sat, 20140920 11:20
Calculate [N2O4] at equilibrium when [NO2]=2.00×10−2mol/L.?
For the reaction N2O4(g)⇌2NO2(g), the value of K at 25∘C is 7.19×10−3.
i would like to see the math behind it so i can understand it better.
thanks in advance
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Submitted by Chemslayer on Thu, 20140731 17:19
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.
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Submitted by zig5151 on Sun, 20140727 17:09
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)((.044x)^4), is that right so far?
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Submitted by Spinnerphoenix on Fri, 20140418 11:29
Mixtures of propan2ol 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.

2propanol

Propanone

Boiling point(°C)

82

56

Molar mass(g/mol)

60

58

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Submitted by roshani on Fri, 20140411 07:25
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 ?
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Submitted by Spinnerphoenix on Mon, 20140407 11:10
Does production of a precipitate decrease concentration?
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Submitted by Spinnerphoenix on Sat, 20140329 13:04
I only need help with the last three dot points.
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Submitted by victoria126 on Sun, 20140323 23:48
What are the equilibrium concentrations of [H_{3}O^{+}], [CN^{}] and [HCN] if the concentration of HCN before equilibrium is 1.0 M? Also, what is the pH of the solution? (K_{a} = 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!!!
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Submitted by nicoked on Mon, 20140310 21:26
A gas has a volume of 2.0 L, and a pressure of 2.0 atm. If the pressure is increased to 4.0 atm, what is the new volume of the gas?
I really just don't know how to even set this problem up. Thats my problem. Dont know where to start. Help me please...
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