Suppose you prepare a lessthanorequalto Chatelier standard for this experiment b

Question

Suppose you prepare a lessthanorequalto Chatelier standard for this experiment by mixing the amounts of reagents below. Using a approach, calculate the concentrations of KSCN and of Fe (NO_3)_3 by mixing the following solutions. Show all your work. Please note, there concentrations represent hypothetical initial concentration of KSCN and of Fe(NO_3)_3. the solutions have been mixed but before any reaction between KSCN and Fe (NO_3) has After the limiting Fe (NO_3)_3 and excess KSCN have been mixed, they react with each other to produce the colored Fe (SCN)^2 product. (Although the reaction may appear instantaneous the mixtures will be allowed several minutes for the reaction to come to completion and for the full color of the solutions to develop). Once the reaction mixture shown above has reached completion, what will be the concentration of the Fe (SCN)^1 product? In order to calculate K_eq, you will need to find the equilibrium concentrations of each of your reactants from initial concentrations of reactants and the equilibrium concentration of the product, using an ICE (Initial. Change, Equilibrium) table approach. Below is the data for concentrations and volume of reagents used for one of the equilibrium solutions which you will prepare. Calculate the initial concentrations of Fe (NO_3)_3 and of KSCN in the solution, where the initial concentrations represents hypothetical concentrations of each reactant after the stated volumes are mixed but before any reaction occurs.

Explanation / Answer

In above question 5 , I have to calculate the equlibirium concentration;

the formula for calculating concentration is total moles divided by mole fraction.

The molecular weight of Fe3O4 is 220 and when it is divided by 1 and multiplied by .0025 (as given in question) = 55.

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