Gibb's free energy, ΔG°, is related to the equilibrium constant of the reaction, K, through the equation:
ΔG°= RT(ln K)
By definition, K is the ratio of the equilibrium partial pressure of the products to the reactants, raised to the power of their stoichiometric coefficients, respectively. For this reaction,
N₂ (g) + 3 H₂ (g) → 2 NH₃<span> (g)
the equilibrium constant is
K = [NH</span>₃]²/[N₂][H₂]³
Assuming that the given partial pressures are the equilibrium pressures, then we can substitute them directly:
K = [0.65 atm]²/[1.9 atm][1.6 atm]³
K = 0.05429 atm⁻²
Then, we can using this value to find ΔG. Note that R is the gas constant equal to 0.08206 L-atm/mol-K.
ΔG°= (0.08206 L-atm/mol-K)(298 K)(ln 0.05429 atm⁻²)
ΔG° = -71.244 L-atm/mol
From the image shown, the uncertainty in the weighing balance extends to the hundredth place.
<h3>What is a balance?</h3>
A balance is any device that is used for measuring the mass or weight of an object. The balance is a necessary instrument in every laboratory.
Looking at the image shown, the following are true;
- the uncertainty is in the hundredth place.
- a mass that falls between 1 gram and 9 grams measured on this balance will always have 3 significant figures.
Learn more about weighing balance: brainly.com/question/8902159
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Explanation:
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