Based on the values you obtained for δh∘rxn, which of the reactions would you expect to be thermodynamically favorable and which would be unfavorable? no. reactions δh∘f (kj) 1 ag + (aq) + li (s) →ag (s) + li + (aq) - 384.4 2 fe (s) + 2na + (aq) →fe2 + (aq) + 2na (s) 392.3 3 2k (s) + 2h2o (l) →2koh (aq) + h2 (g) - 393.1

Question

Mateo Rogers

Chemistry

27 February, 10:33

Based on the values you obtained for δh∘rxn, which of the reactions would you expect to be thermodynamically favorable and which would be unfavorable? no. reactions δh∘f (kj) 1 ag + (aq) + li (s) →ag (s) + li + (aq) - 384.4 2 fe (s) + 2na + (aq) →fe2 + (aq) + 2na (s) 392.3 3 2k (s) + 2h2o (l) →2koh (aq) + h2 (g) - 393.1

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Selina Bowers · Answer 1

Following reactions are involved in present reaction

1) A g + (aq) + Li (s) → Ag (s) + Li + (aq) - 384.4kJ

2) 2Fe (s) + 2Na + (aq) → Fe2 + (aq) + 2Na (s) + 392.3kJ

3) 2K (s) + 2H2O (l) → 2KOH (aq) + H2 (g) - 393.1kJ

In above reaction, reaction 1 and 3 has negative value of δh∘f, while reaction 2 has posiyive value of δh∘f. As per the sign convention positive sign indicates that heat is given out during the reaction, while negative sign indicates heat is to be supplied for reaction to occur. In alternative words, product formed in reaction 2 is stable as compared to reactant. Hence, it is thermodynamically favorable.