Question

9. The equilibrium constant for the reaction H2(g) + I2(g) 2HI(g) has a value of 54.6 at 699K. What are

the equilibrium concentrations of H2, I2, and HI if the initial concentrations at this temperature are 0.0800M

H2 and 0.0700 M I2.

10. Find the pH and pOH of a solution prepared by dissolving 9.85 grams of NaOH into a total aqueous solution

volume of 75.0 ml.

11. Using the data in Appendix B of your text, calculate the values of H

o

, S

o

, and G

o for the following

reaction at 25oC.

MgCO3(s)  MgO(s) + CO2(g)

9. The equilibrium constant for the reaction H:(g)+g)2HI(g) has a value of 54.6 at 699K. What are the equilibrium concentrations of H, , and Hl if the initial concentrations at this temperature are 0.0800M H2 and 0.0700 M 12 10. Find the pH and pOH of a solution prepared by dissolving 9.85 grams of NaOH into a total aqueous solution volume of 75.0 ml. 11. Using the data in Appendix B of your text, calculate the values of ΔΗ®. Δ. and ΔGo for the following reaction at 25°C. MgCO (s) MgO(s)+ CO.(g)

Answer 1

Tital (M) 0.07 =54,6 54. 6 )2 2 2. 2 50.6 8.19 ± 2.2 2X 50.6 竺(o, ogー0.0589-0.0215(H) (0.07-0.058s)=0.0115(M Lita.] ai equilibrum าร 2. 9.85 100o3.28 CM) 0 Mol eng Lo#7-10 a 140H14 5 14 3.28 5.16 5.16) = 8.84

={393-5-6017)-(-1095.8 чт ae avem for the Calculation ニ100.60 x100.0-298x174:94) J 4 ,847 x104 J = 48-47 KJ