At 35°C, K = -5 1.7 x 10 for the reaction 2 NOCI(9) = 2 N0(9) + Cl2 (g) Calculate the concentrations of all species at equilibrium for each of the following original mixtures. a. 3.2 moles of pure NOCI in a 2.0-L flask [NOCI] M =

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At 35°C,
K =
1.7 x 10- for the reaction
2 NOCI(g) = 2 NO(g)+ Cl2 (g)
Calculate the concentrations of all species at equilibrium for each of the following original mixtures.
a. 3.2 moles of pure NOCI in a 2.0-L flask
[NOCI]
M
%3D
[NO]
M
[Cl2]
M
%3D
b. 1.0 mole of
NOCI and 1.0 mole of
NO in a 1.0-L flask
[NOCI]
M
[NO] =
M
[Cl2] =
M
С. 2.8 mole of
NOCI and 1.0 mole of
Cl2 in a 1.0-L flask
[NOCI]
M
[NO] =
M
[Cl2]
M
Transcribed Image Text:At 35°C, K = 1.7 x 10- for the reaction 2 NOCI(g) = 2 NO(g)+ Cl2 (g) Calculate the concentrations of all species at equilibrium for each of the following original mixtures. a. 3.2 moles of pure NOCI in a 2.0-L flask [NOCI] M %3D [NO] M [Cl2] M %3D b. 1.0 mole of NOCI and 1.0 mole of NO in a 1.0-L flask [NOCI] M [NO] = M [Cl2] = M С. 2.8 mole of NOCI and 1.0 mole of Cl2 in a 1.0-L flask [NOCI] M [NO] = M [Cl2] M
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We are given an Equilibrium mixture, and it's equilibrium constant

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