Achieve HW #2

[JasmineReyes-2K]

Hi!,

Can someone tell me if I have to divide either 0.620 or 0.200 to find the initial concentration? I am not sure where to start

[Natalie Vu 1I]

Hi,

so first you would make an ice table with 0.620 being the initial concentration for SO3 (but remember to divide by 2.50 L!). You would also put 0.200 mol (divide by 2.50 L again) for the equilibrium O2. Then, you would fill in the +/- x for the C (change) part of the ice table. From there, you should be able to find the equilibrium constant from O2 and find Kc.

[Safwaan Khan 2K]

In this scenario, we are explicitly given the initial concentration of the reactant SO3, 0.620 moles/2.50L. Additionally, we are explicitly given the equilibrium concentration of one product O2, 0.200moles/2.50L. Thus, we know that the initial concentrations are as follows:

SO3: 0.620/2.50
SO2: 0
O2: 0

We also know that since there is only reactant that some amount of product will form during the reaction. Sine we are given the coefficients of the equilibrium reaction, we can assert that the changes in concentrations will be as follows.

SO3: -2x
SO2: +2x
O2: +x

Thus, our final/equilibrium concentrations based off given values, the initial concentration, and the change in concentration would be:

SO3: 0.620/2.50 - 2x
SO2: 2x
O2: 0.200/2.50 = x

Then, using our previous knowledge of how to solve for K given the products, reactants, and their coefficients, we would plug in the equilibrium concentrations to solve for Kc.

[405566265]

divide by the liter amount =. concentration is moles/liter, so if the container is not exactly equal to 1.00 L, then you need to divide by liters to obtain the concentrations and proceed with the problem

[Alekhya_Pantula_2E]

You would divide 0.620 by 2.50L to get the molar concentration of SO3. Then when you set up your ICE table, you would have the initial concentrations for SO3 be .620/2.5 and then 0 for the products as no product has been formed yet. We also know the equilibrium concentration of O2, so we plug that into the equilibrium concentrations. Then you can fill in the rest of the table to solve.

[Robert Nguyen 14B-3E]

As you want molarity, which equals moles / liters, you have to divide 0.620 mol by 2.50 L to start

[205282258]

In order to get the initial molarity of SO3 to put into the ICE table you divide 0.620 moles by 2.50 L. The other two initial values are 0. Then find the changes in concentration with x and divide 0.2 moles by 0.250 L to find the final molarity of O2. Use this O2 value and the ICE table to solve for K.

[Michelle Argueta 1E]

To get the initial molarity of SO3 to use an ICE table you divide 0.620 moles by 2.50 L and the other two initial values are 0. Then find the changes in concentration with x (make sure to look at the coefficients of the balanced reaction) and divide 0.2 moles by 0.250 L to find the final molarity of O2 since the final equilibrium molarity for O2 is provided. Use this O2 value and the ICE table to solve for K.