Question

Calculate K at 298 K for the following reaction: SrSO₄(s) <--> Sr₂ +(aq) + SO₄₂-(aq) SCIENTIFIC NOTATION PLEASE

Comments : the answer K = 3.48 x 10⁻⁷ was wrong,it said

HInt: For any state function (G, H, or S) the change in the state function, F, for a reaction can be calculated from Delta F rxn= (sideways M)n x delta F (products) minus (sideways M) n x delta F (reactants), when n are the stoichiometric coefficients from the balanced chemical equation. Use this expression to calculate Delta G rxn. Use the expression that relates change in fuel energy of a reaction, Delta G rxn, to the equilibrium constant K.

p.s. (the ⁻⁷ power part was correct). I still get 2 more chances.

Answer 1

To calculate K at 298 K for the dissolution of SrSO4, standard free energy of formation values for the ions are needed to find ΔGorxn and apply the equation K = e(-ΔGorxn / RT), with the result in scientific notation.

Step-by-step explanation:

To calculate the equilibrium constant (K) for the dissolution of SrSO4 at 298 K, we need to determine the standard free energy change (ΔGorxn) and use the relationship ΔGorxn = -RTlnK, where R is the gas constant and T is the temperature in kelvins. Assuming standard state conditions, the activity for the solid SrSO4 is 1, and concentrations of the ions Sr2+ and SO42- are expressed in terms of molarity.

To find ΔGorxn, you need to know ΔGof values for the ions involved, which are Sr2+(aq) and SO42-(aq). With these values, you can then employ the previously mentioned equation to calculate ΔGorxn and ultimately K using the equation K = e(- ΔGorxn / RT). The result needs to be expressed in scientific notation.

Given the hint that the –7 power was correct, we assume that the order of magnitude for K is 10–7. However, to accurately determine K, you will need the specific standard free energy of formation (ΔGof) values for the products and reactants involved in the reaction.