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Andre45 [30]
3 years ago
7

Based on the standard free energies of formation, which of the following reactions represent a feasible way to synthesize the pr

oduct?
A. 2C(s)+H2(g)→C2H2(g); ΔG∘f=209.2 kJ/mol
B. N2(g)+3H2(g)→2NH3(g); ΔG∘f=−33.30 kJ/mol
C. 2C(s)+2H2(g)→C2H4(g); ΔG∘f=68.20 kJ/mol
D. 2SO(g)+O2(g)→2SO2(g); ΔG∘f=−600.4 kJ/mol
Chemistry
1 answer:
Lyrx [107]3 years ago
5 0

Answer:

The correct answer are option B and D.

Explanation:

ΔG° = ΔH° - TΔS°

Where:

ΔG° = Gibbs's free energy of the reaction at temperature T.

ΔH° = Enthalpy of the reaction at temperature T.

ΔS° = Change in entropy of the reaction at temperature T.

  • If the vales of Gibb's free energy is less than zero or negative than the reaction is said to be spontaneous that is feasible under given conditions.
  • If the vales of Gibb's free energy is greater than zero or positive than the reaction is said to be non spontaneous that is non feasible under given conditions.

From the given reaction, the reaction with value of \Delta G_{f}^o  represents the a feasible way to synthesize the product. So, the correct answer are option B and D.

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kolbaska11 [484]

Answer:

P_{air}=1.02atm

Explanation:

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In this case, since the Dalton's law help us to realize that the total pressure of a gas mixture is computed by adding the partial pressure of each composing gas, for the mixture formed by carbon dioxide, oxygen sulfide (should be hydrogen sulfide instead) and air, we can write:

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Thus, given the total pressure and the partial pressures of both carbon dioxide and hydrogen sulfide, the partial pressure of the remaining air would be:

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