The equilibrium constant, K., for the following reaction is 77.5 at 600 K. CO(g) + Cl₂(g) →COCI₂(g) Calculate the equilibrium concentrations of reactant and products when 0.211 moles of CO and 0.211 moles of Cl₂ are introduced into a 1.00 L vessel at 600 K. [CO] = [Clzl = [COCI₂] = M M M
The equilibrium constant, Kc, for the following reaction is 77.5 at 600 K.
CO(g) + Cl2(g) COCl2(g)
Calculate the equilibrium concentrations of reactant and products when 0.211 moles of CO and 0.211 moles of Cl2 are introduced into a 1.00 L vessel at 600 K.
| [CO] | = | M |
| [Cl2] | = | M |
| [COCl2] | = | M |
![The equilibrium constant, K, for the following reaction is 77.5 at 600 K.
CO(g) + Cl₂(g)
COCI₂(g)
Calculate the equilibrium concentrations of reactant and products when 0.211 moles of CO and 0.211 moles of Cl₂ are introduced into a 1.00 L vessel at 600 K.
[CO] =
[Cl₂] =
[COCI₂] =
M
M
M](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F2be65d23-e07e-4ce3-8dd7-b7173547e175%2F9db87aae-30ce-4082-aa35-8ba185853d73%2Fk28rr5_processed.png&w=3840&q=75)
The equilibrium constant of a chemical reaction is the ratio of the product of the active masses of the products to the product of the active masses of the reactants, with each concentration term raised to its corresponding stoichiometric coefficient in the balanced chemical equation.
The given equilibrium reaction is CO(g) + Cl2(g) format('truetype')%3Bfont-weight%3Anormal%3Bfont-style%3Anormal%3B%7D%3C%2Fstyle%3E%3C%2Fdefs%3E%3Ctext%20font-family%3D%22math1aa495e18c7e3a21a4e48923b92%22%20font-size%3D%2216%22%20text-anchor%3D%22middle%22%20x%3D%2210.5%22%20y%3D%2216%22%3E%26%23x21CC%3B%3C%2Ftext%3E%3C%2Fsvg%3E)
COCl2(g)
Initial number of moles of carbon monoxide = 0.211 mol
Initial number of moles of chlorine = 0.211 mol
Volume of the container = 1.00 L
The equilibrium constant of the reaction, Kc =77.5
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