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13 Dec 2019

If the ΔG0' of the reaction A→ B is -23 kJ.mol-1, under standard condition, which of the following is true?

-The entropy change (ΔS0') must be positive.

-The reaction will proceed rapidly

. -The enthalpy change (ΔH0') of this reaction must be negative.

-The reverse reaction B→A will not occur spontaneously.

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Tod Thiel
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17 Dec 2019

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Related questions

Part A: Using the heats of formation and standard entropy, calculate ΔH0 and ΔS0 then use these to calculate ΔG0 and determine if the reaction is spontaneous at 1000C. If not, under what temperature conditions will it become spontaneous? and K at the given temperature. Assume ΔH0 and ΔS0 are not affected by temperature.

O2(g) + 2F2(g) <----> 2F2O(g) T= 1000C

ΔHf0(kJ/mol) 0 0 24.7

S0(J/K-mol) 205.2 202.8 247.43

Part B: Calculate equilibrium constant (K) and state whether products or reactants are favored

The equilibrium constant under standard conditions (1 atm, 298 K, pH 7.0) for the reaction below, catalyzed by fumarase, is 4.00. At 310 K, the equilibrium constant is 8.00.

Fumarate(aq) + H2O ⇄ 1-malate (aq)

a. What is the standard Gibbs energy change ΔG0 for this reaction?

b. If [1-malate] = 0.01M and [fumarate] = 0.02 M, what is the Gibbs energy change at 298 K?

c. From b. above, how will this reaction proceed to equilibrium – that is: will more fumarate or Lmalate form?

d. Evaluate ΔH0 and ΔS0 for this reaction at 298K. State any assumptions you make.

a) {10} Calculate ΔH0, ΔS0, and ΔG0 at 300.0 0C b) {5} Calculate the equilibrium constant, Keq, for the rxn at 300.0 oC c) {1} is reaction goes forward or reverse at 300.0 oC? d) {2} Suggest two possible actions you could perform in the lab in order to change direction of this rxn. e) {2} Calculate temperature in Kelvins at which reaction will change direction substance ΔHof (kJ/mol) S (J/mol K) NH3 (g) -46.19 192.5 HNO3 (g) -134.3 266.4 NH4 NO3 (s) -365.6 151.0

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