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Consider the following system at equilibrium where ΔH∘=10.4 kJ, and Kc=0.0180, at 69 ; 2HI(g)⇌H2(g)+I2(g) When 0.32 m
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Consider the following system at equilibrium where ΔH∘=10.4 kJ, and Kc=0.0180, at 69 ; 2HI(g)⇌H2(g)+I2(g) When 0.32 m
Consider the following system at equilibrium where ΔH∘=10.4 kJ, and Kc=0.0180, at 69 ; 2HI(g)⇌H2(g)+I2(g) When 0.32 moles of H2(g) are added to the equilibrium system at constant temperature: The value of Ke increases decreases remains the same The value of Qc is greater than Kc is equal to Kc is less than Kc The reaction must run in the forward direction to reestablish equilibrium run in the reverse direction to reestablish equilibrium remain in the current position, since it is already at equilibrium The concentration of H2 will increase decrease remain the same
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