Use the tabulated thermodynamic values of Delta H degree f and S degree to calcu

Question

Use the tabulated thermodynamic values of Delta H degree f and S degree to calculate the value of Kp at 25 degree C for the gas-phase reaction CO + H2O CO2 + H2 Calculate the value of Kp for this reaction at 200. Degree C, by the same method as in part (a), (c) Repeat the calculation of part (a) using tabulated values of Delta G degree f. The equilibrium constant Kc for the reaction H2(g) + Br2(g) 2HBr(g) is 1.6 Times 105 at 1297 K and 3.5 Times 104 at 1495 K. ( a ) Is Delta H degree for this reaction positive or negative? (b) Find Kc for the reaction ½ H2(g) + ½ Br2(g) HBr(g) at 1297 K. (c) Pure HBr is placed in a container of constant volume and heated to 1297 K. What percentage of the HBr is decomposed to H2 and Br2 at equilibrium? The air pollutant sulfur dioxide can he partially removed from stack gases in industrial processes and converted to sulfur trioxide, the acid anhydride of commercially important sulfuric acid. Write the equation for the reaction, using the smallest whole-number coefficients. Calculate the value of the equilibrium constant for this reaction at 25 degree C from values of Delta G degree f in Appendix K. The value of Delta H degree for the reaction in Exercise 86 is - 197.6 kJ/mol. (a) Predict qualitatively (i.e., without calculation) whether the value of KP for this reaction at 500 degree C would be greater than, the same as, or less than

Explanation / Answer

(a)In(3.5 x 10^4 / 16 x 10^4) = -((delta H)/R) [1/1495 - 1/1297]

delta H = -123.743 kJ/mol

delta H is negative.

(b) Kc = (1.6 x 10^5)^2 = 2.56 x 10^10

(c) Percentage of HBr decomposed = 100/(2.56 x 10^10) = 3.91 x 10^-9 %

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