Express the equilibrium constant for the following reaction: CH 3 Cl(g)+ 1/2 Cl 2 (g)? CH 2 Cl 2 (g)+ 1/2 H 2 (g)

The equilibrium constant expression for a reaction is written by taking the partial pressures of the products in the numerator and the partial pressures of the reactants in the denominator, each raised to the power of their stoichiometric coefficients. In this case, the equilibrium constant expression is:K P = $\frac { \mathrm { P } \left( \mathrm { CH } _ { 2 } \mathrm { Cl } _ { 2 } \right) \times \mathrm { P } ^{1 / 2} \left( \mathrm { H } _ { 2 } \right) } { \mathrm { P } \left( \mathrm { CH } _ { 3 } \mathrm { Cl } \right) \times \mathrm { P } ^ { 1 / 2 } \left( \mathrm { Cl } _ { 2 } \right) }$

Express the equilibrium constant for the following reaction: CH 3 Cl(g)+ 1/2 Cl 2 (g)? CH 2 Cl 2 (g)+ 1/2 H 2 (g)

The equilibrium constant expression for a reaction is written by taking the partial pressures of the products in the numerator and the partial pressures of the reactants in the denominator, each raised to the power of their stoichiometric coefficients. In this case, the equilibrium constant expression is:K P = $\frac { \mathrm { P } \left( \mathrm { CH } _ { 2 } \mathrm { Cl } _ { 2 } \right) \times \mathrm { P } ^{1 / 2} \left( \mathrm { H } _ { 2 } \right) } { \mathrm { P } \left( \mathrm { CH } _ { 3 } \mathrm { Cl } \right) \times \mathrm { P } ^ { 1 / 2 } \left( \mathrm { Cl } _ { 2 } \right) }$

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Express the Equilibrium Constant for the Following Reaction:
CH₃Cl(g)

Question 4

Multiple Choice

Express the equilibrium constant for the following reaction:
CH₃Cl(g) + 1/2 Cl₂(g) ? CH₂Cl₂(g) + 1/2 H₂(g)

A) K_P = $\frac { \mathrm { P } \left( \mathrm { CH } _ { 2 } \mathrm { Cl } _ { 2 } \right) \times \mathrm { P } ^{1 / 2} \left( \mathrm { H } _ { 2 } \right) } { \mathrm { P } \left( \mathrm { CH } _ { 3 } \mathrm { Cl } \right) \times \mathrm { P } ^ { 1 / 2 } \left( \mathrm { Cl } _ { 2 } \right) }$
B) K_P = $\frac { \mathrm { P } ^ { 2 } \left( \mathrm { CH } _ { 2 } \mathrm { Cl } _ { 2 } \right) \times \mathrm { P } \left( \mathrm { H } _ { 2 } \right) } { \mathrm { P } ^ { 2 } \left( \mathrm { CH } _ { 3 } \mathrm { Cl } \right) \times \mathrm { P } \left( \mathrm { Cl } _ { 2 } \right) }$
C) K_P = $\frac { \mathrm { P } ^ { 2 } \left( \mathrm { CH } _ { 3 } \mathrm { Cl } \right) \times \mathrm { P } \left( \mathrm { Cl } _ { 2 } \right) } { \mathrm { P } ^ { 2 } \left( \mathrm { CH } _ { 2 } \mathrm { Cl } _ { 2 } \right) \times \mathrm { P } \left( \mathrm { H } _ { 2 } \right) }$
D) K_P = $\frac { \mathrm { P } \left( \mathrm { CH } _ { 3 } \mathrm { Cl } \right) \times \mathrm { P } \left( \mathrm { Cl } _ { 2 } \right) } { \mathrm { P } \left( \mathrm { CH } _ { 2 } \mathrm { Cl } _ { 2 } \right) \times \mathrm { P } \left( \mathrm { H } _ { 2 } \right) }$
E) K_P = $\frac { \mathrm { P } \left( \mathrm { CH } _ { 3 } \mathrm { Cl } \right) \times \mathrm { P } ^{1 / 2} \left( \mathrm { Cl } _ { 2 } \right) } { \mathrm { P } \left( \mathrm { CH } _ { 2 } \mathrm { Cl } _ { 2 } \right) \times \mathrm { P } ^ { 1 / 2 } \left( \mathrm { H } _ { 2 } \right) }$

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Express the Equilibrium Constant for the Following Reaction: CH3Cl(g)

Express the Equilibrium Constant for the Following Reaction:
CH₃Cl(g)