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xenn [34]
3 years ago
6

Examine the given reaction. NH4NO3(s) → NH4+(aq) + NO3–(aq) ΔH° = 25.45 kJ/mol ΔS° = 108.7 J/mol·K Which of the given is correct

about the ΔG° at 25 °C?
A)+4,360 J
B)−6,942 J
C)−4,360 J
D)+6,942 J
Chemistry
1 answer:
kobusy [5.1K]3 years ago
8 0

Answer:

B)−6,942 J /mol

Explanation:

At constant temperature and pressure, you cand define the change in Gibbs free energy, ΔG, as:

ΔG = ΔH - TΔS

Where ΔH is enthalpy, T absolute temperature and ΔS change in entropy.

Replacing (25°C = 273 + 25 = 298K; 25.45kJ/mol = 25450J/mol):

ΔG = ΔH - TΔS

ΔG = 25450J/mol - 298K×108.7J/molK

ΔG = -6942.6J/mol

Right solution is:

<h3>B)−6,942 J /mol</h3>

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When an arrhenius base is placed in h20 the only negative ion present in the solution is?
melamori03 [73]
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Need help please :'((((((((((
kati45 [8]

Answer:

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Explanation:

4.44

6 0
2 years ago
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