Consider the following equilibrium system: N2 2+ 3H2@)_ + 0.80 moles of N2 and 0.80 moles of H2 are placed into a 1.0 L container and allowed to establish equilibrium. At equilibrium [NH3] = 0.46 M. a) Calculate the equilibrium [N2] b) Calculate the equilibrium [H2] c) Determine the value of Keq at this temperature. →2NH3 g

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Consider the following equilibrium system:
N2 (2) + 3H2@)_
0.80 moles of N2 and 0.80 moles of H2 are placed into a 1.0 L container and allowed
to establish equilibrium. At equilibrium [NH3] = 0.46 M.
a) Calculate the equilibrium [N2]
b) Calculate the equilibrium [H2]
c) Determine the value of Keq at this temperature.
NOTE: In a 1.0 Litre container, concentration is moles/ 1.0 litre, so concentration is the
same as the moles. In other words, if 0.80 moles of N2 are placed in a 1.0 L container,
the initial concentration of N2 = 0.80 M
→2NH3 2
Transcribed Image Text:Consider the following equilibrium system: N2 (2) + 3H2@)_ 0.80 moles of N2 and 0.80 moles of H2 are placed into a 1.0 L container and allowed to establish equilibrium. At equilibrium [NH3] = 0.46 M. a) Calculate the equilibrium [N2] b) Calculate the equilibrium [H2] c) Determine the value of Keq at this temperature. NOTE: In a 1.0 Litre container, concentration is moles/ 1.0 litre, so concentration is the same as the moles. In other words, if 0.80 moles of N2 are placed in a 1.0 L container, the initial concentration of N2 = 0.80 M →2NH3 2
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