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Elza [17]
2 years ago
15

The free energy of formation of nitric oxide, NO, at 1000 K (roughly the temperature in an automobile engine during ignition) is

about 78 kJ/mol. Calculate the equilibrium constant Kp for the reaction N2(g) + O2(g) 2NO(g) at this temperature.
Chemistry
1 answer:
Assoli18 [71]2 years ago
4 0

<u>Answer:</u> The value of K_p for the chemical equation is 8.341\times 10^{-5}

<u>Explanation:</u>

For the given chemical equation:

N_2(g)+O_2(g)\rightarrow 2NO(g)

To calculate the K_p for given value of Gibbs free energy, we use the relation:

\Delta G=-RT\ln K_p

where,

\Delta G = Gibbs free energy = 78 kJ/mol = 78000 J/mol  (Conversion factor: 1kJ = 1000J)

R = Gas constant = 8.314J/K mol

T = temperature = 1000 K

K_p = equilibrium constant in terms of partial pressure = ?

Putting values in above equation, we get:

78000J/mol=-(8.314J/Kmol)\times 1000K\times \ln K_p\\\\Kp=8.341\times 10^{-5}

Hence, the value of K_p for the chemical equation is 8.341\times 10^{-5}

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here ya go trust

Explanation:

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Why did you blank with the 0.0020 M Fe(NO3)3 solution as opposed to just DI water? What does it do to your spectrum? What chemic
Vlad1618 [11]

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Explanation:

The cuvette was blank with the solution so that the spectrometer will only read the solute absorbance. This also ensures that the spectrometer will ignore other absorbance fluctuations that normally occur due to the chemical make-up of water. The spectrometer only considered the absorbance of FeNCS^{2+} as indicated on the spectrum.

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