We're being asked to determine which of the following statements describe the state of equilibrium for the chemical system R(g) ⇌ P(g).
Let's analyze each of the given statement.
A. Kp = Kc
Kp and Kc are related to one another by the following equation below:
R = gas constant = 0.08206 (L∙atm)/(mol∙K)
T = temperature, K
Δn = moles of gas products – moles of gas reactants
From the reaction: R(g) ⇌ P(g)
Which of the following statements describe that state of equilibrium for the chemical system R(g) ⇌ P(g)? You don’t want to answer this question by just making a blind choice. Get basic concepts on the notes.
Choose all that apply.
A. Kp = Kc
B. The state of equilibrium is achieved starting with 1 mol of P in a 1-liter volume.
C. More product P can be formed if the equilibrium is disturbed by decreasing the volume.
D. The value of the equilibrium constant changes when the concentration, pressure, volume and addition of catalyst event at constant temperature.
E. When Q is larger than K, the reaction is irreversible.
F. When the concentration of a product in a reaction that was originally at the state of equilibrium is increased, the value Q < K.
G. At the state of equilibrium, the rate of formation of the products is equal to the rate of consumption of the reactants.
H. The concentrations of R and P are equal at the state of equilibrium
I. When the temperature is increased, the equilibrium constant goes up, which leads to the conclusion that the backward reaction is endothermic.
J. If the K of the reaction is 1000, the concentration of P predominates at equilibrium, which means that backward reaction is favored.
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