3. Calculate the concentration of Fe in solution, if 5.00 mL of 0.20M Fe(NO)s wa

Question

3. Calculate the concentration of Fe in solution, if 5.00 mL of 0.20M Fe(NO)s was dispensed into a 50.0 mL volumetric flask and diluted with DI to the 50 mL mark. 4. Write the equilibrium constant expressions for the following reactions (a) CH:CO2H (aH20HO(aq) CH,CO2 (aq) (b) CaCO,(s) Ca2 (aa)+ CO (a) S)T 5. If the Keq value for (a) above was 14 would you expect there to be more reactants or products? 6. Determine the pressure-based Keq for the reaction: 2SO2(g) + O2(g) - 2SO3(g) given that 1.00x 10-2 moles of SO2 and 2.00× 10-2 moles of O2 were initially placed in a 2.00 L reaction chamber. The chamber contained 7.5x10 moles of SOs when equilibrium was established at 7278C. Since you need to calculate the pressure-based equilibrium constant, you will need to use the ideal gas equation (PV-nRT) to convert the moles of gas into pressure with units of atmospheres. (remember that one formulation of R is 0.0821 L atm/mol K)

Explanation / Answer

3) On dilution

M1V1 = M2 V2

5.00mL x 0.2 M = 50 x M2

Thus M2 = 0.02 M

the concentration of Fe+3 = 0.02 M

4)

a) K eq = [H3O+] [CH3COO-] / [CH3COOH]

as the concentration of pure liquids and solids = 1

b) Keq = [Ca+2] [Co3-2]

5)If Keq = 14 , it means the products oncentrations are more than reactants, thu s we expect more of products.

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