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At some temperature for the equilibrium PX3(g) + X2(g) # PX5(g) the equilibrium constant is 0.74. At the same temperature the equilibrium constant for PX5(9) + PX3(g) X2(g) is​

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Answer: The equilibrium constant for
PX_5(g)\rightarrow PX_3(g)+X_2(g) is 1.35

Step-by-step explanation:

Equilibrium constant is defined as the ratio of concentration of products to the concentration of reactants each raised to the power their stoichiometric ratios. It is expressed as
K_c

For the given chemical reaction:


PX_3(g)+X_2(g)\rightarrow PX_5(g)

The expression for
K_c is written as:


K_c=([PX_5]^1)/([PX_3]^1[X_2]^1)


0.74=([PX_5]^1)/([PX_3]^1[X_2]^1)

For the reverse chemical reaction:


PX_5(g)\rightarrow PX_3(g)+X_2(g)

The expression for
K_c' is written as:


K_c'=([PX_3]^1[X_2]^1)/([PX_5]^1)


K_c'=(1)/(K_c)=(1)/(0.74)=1.35

The equilibrium constant for
PX_5(g)\rightarrow PX_3(g)+X_2(g) is 1.35

User Tom Clift
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