Kp-Kc (RT)AnK=(°C+273.15°C)(C)An= moles of gaseous products-moles of gaseous reactantsR=0.08206 L'atmmol-K1. The equilibrium constant K₁ for the reaction:CO₂(g) CO(g) + 1/2O₂(g)The reaction below has an equilibrium constant K₂.2 CO(g) + O₂(g) 2 CO₂(g) K₂How are K₁ and K₂ related? Calculate the value of K₂.2. Using this data,2 NO(g) + Cl₂(g) 2 NOCI(g)2 NO₂(g) = 2 NO(g) + O₂(g)calculate a value for K3 for the reaction,NOCI(g) + O2(g) NO₂(g) + Cl₂(g)is 6.66 X 10-¹2 at 1000 K.K₁ = 3.20 x 10-³K₂ = 15.5

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1. The equilibrium constant K₁ for the reaction: CO₂(g) CO(g) + 1/2O₂(g) The reaction below has an equilibrium constant K₂. 2 CO(g) + O₂(g) 2 CO₂(g) K₂ How are K₂ and K₂ related? Calculate the value of K₂. is 6.66 X 10-¹2 at 1000 K.

1. The equilibrium constant K₁ for the reaction: CO₂(g) CO(g) + 1/2O₂(g) The reaction below has an equilibrium constant K₂. 2 CO(g) + O₂(g) 2 CO₂(g) K₂ How are K₂ and K₂ related? Calculate the value of K₂. is 6.66 X 10-¹2 at 1000 K.

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter17: Chemcial Thermodynamics

Section: Chapter Questions

Problem 17.89QE: For each reaction, an equilibrium constant at 298 K is given. Calculate G for each reaction. (a)...

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Question

Kp-Kc (RT)An
K=(°C+273.15°C)(C)
An= moles of gaseous products-moles of gaseous reactants
R=0.08206 L'atm
mol-K
1. The equilibrium constant K₁ for the reaction:
CO₂(g) CO(g) + 1/2O₂(g)
The reaction below has an equilibrium constant K₂.
2 CO(g) + O₂(g) 2 CO₂(g) K₂
How are K₁ and K₂ related? Calculate the value of K₂.
2. Using this data,
2 NO(g) + Cl₂(g) 2 NOCI(g)
2 NO₂(g) = 2 NO(g) + O₂(g)
calculate a value for K3 for the reaction,
NOCI(g) + O2(g) NO₂(g) + Cl₂(g)
is 6.66 X 10-¹2 at 1000 K.
K₁ = 3.20 x 10-³
K₂ = 15.5

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