temperature does Kc = 6.4x10⁹, T=0.599*[tex]10^{7\\[/tex] K.
The equilibrium constant, abbreviated Kc, is the ratio of the equilibrium concentrations of the products over the equilibrium concentrations of the reactants, each raised to the power of their respective stoichiometric coefficients.
Kp = Kc (RT)∧Δn
Kp = 1.3 ˣ 10⁴
kc=6.4 x [tex]10^{9}[/tex]
Δn = -1
kp/kc=(RT)∧Δn
R = 0.0821 Latm/K.mol
1/T=[tex]\frac{1.3 X 10^{4} }{6.4 X 10^{9} } * 0.0821[/tex]
T=0.599*[tex]10^{7\\[/tex] K
The equilibrium constant, Kp, can be calculated using the partial pressures in the reaction equation. The ratio of the equilibrium product concentrations to the reactant concentrations is represented by the equilibrium constant, Kc.
Link between KP and KC In general, the relationship between KP and KC is K P = K C (RT) n, where n = the sum of the moles of the gaseous reactants and products.
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