Sapling Week 1 #3

[Sean Phen]

At a certain temperature, the equilibrium constant, Kc, for this reaction is 53.3.

H2(g)+I2(g)↽−−⇀2HI(g)Kc=53.3

At this temperature, 0.600 mol H2 and 0.600 mol I2 were placed in a 1.00 L container to react. What concentration of HI is present at equilibrium?

[Sydney Lam_2I]

Hi! So you would need to create an ice table in order to solve for this. First calculate the initial concentrations of the reactants and products for I. For the change, due to us know it shift to the right (no products initially) the change for the reactants would be -x and the change for the product would be +2x. So, the equilibrium concentrations would be the initial plus the change. From there use the K equation to solve for x and input x back into the equilibrium concentrations equations to solve for the concentrations!

[Simran Bains 2C]

I had trouble on this one for a while because I didn't multiply my x by 2 at the end, so remember to do that.

[Kaiya_PT_1H]

Not sure if this helps, but I spent a long time on this trying to do the quadratic formula when you can just square root the Kc formula and the value for Kc to solve for x.

[Sana Nagori 2H]

Not sure if this helps, but I spent a long time on this trying to do the quadratic formula when you can just square root the Kc formula and the value for Kc to solve for x.

I wish I saw this beforehand. I also did the whole quadratic formula out haha

[FrancescaHawkins2H]

I also did the whole quadratic formula without realizing I could use a square root! Good tip to be on the lookout for for next time though.

[Tobie Jessup 2E]

remember to account for the stoichiometric coefficients! Thats why I had problems with this problem.

[Nick Saeedi 1I]

I used an ICE table to solve this question. You know the initial concentrations by dividing moles/Liters and you have the coefficients which will give u the change. Then you can set up an expression that you can set equal to Kc which is [HI]^2/[H2][I2]

[Presley Gao 2C]

For this question, you would have to set up an ICE table. One tip is that you can just take the square root the Kc formula and the value for Kc to solve for x. Although this is a shortcut, I would not recommend using this and instead solve the entire quadratic formula since taking the square root of something results in both a positive and a negative value, but it depends on the situation.

[Neel Sharma 3F]

Create an ICE table. Plug in the given values. Designate unknowns with a variable. Plug in equilibrium values into the equilibrium expression and solve the resultant algebraic expression. Often times you can find ways to simplify it before things get too messy. Hope this helps!