Question

For an equilibrium reaction: А + В С +D the following graph was obtained. 90 80 70 6е 50 40 зе 20 10 -10 -20 e.002 0.01 0.004 0.006 0.008 1/T Ink -AHo RT ASO + R Given the above relationship, use the graph to identify which of the following statements are "true" or "false" in this specific case. All statements refer to the forward reaction (proceeding left to right, as given) corresponding to the equilibrium constant K. deltaSo for the reaction is positive The reaction is spontaneous at low temperatures but not at the highest temperatures. The reaction is exothermic. As the temperature is decreased, the equilibrium position shifts in favour of the products. false deltaG° is negative at low temperatures but becomes positive at higher temperatures. true true true true See Zumdahl, "Chemical Principles" 8th ed. Sec 10.11, p386 "The Temperature Dependence of K". Incorrect. Tries 4/8 Previous Tries Submit Answer

Answer 1

1) False, you have to:

ΔS = R * b; b is negative, therefore, ΔS is negative.

2) True, you have to:

ΔG = ΔH - T * ΔS

ΔH = - m * R

ΔH is negative, ΔS is negative. At low temperatures ΔG is negative and spontaneous, at high temperatures ΔG can be positive.

3) True, ΔH is negative, that is, the reaction is spontaneous.

4) True, the reaction is exothermic, if heat is removed from the medium, production of products is favored.

5) True, explained in response 2.

If you liked the answer, please rate it in a positive way, you would help me a lot, thank you.