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At 2000 ∘C the equilibrium constant for the reaction 2NO(g)⇌N2(g)+O2(g) is Kc=2.4×103.?
Kc = [N2][O2] / [NO]²
2400 = (x)(x) / (0.171 – 2x)²
2400 = x² / (0.171 – 2x)²
sqrt(2400) = x / (0.171 – 2x)
sqrt(2400) (0.171 – 2x) = x
(0.171)sqrt(2400) = [1 + 2(sqrt(2400))]x
x = 0.084636
[NO] = 0.171 – 2(0.084636) = 1.73e-3 M
[N2] = [O2] = x = 8.46e-2 M
The equilibrium constant for the reaction N2(g)+O2(g) gives 2NO… – Equilibrium constant is defined as the ratio of concentration of products to the concentration of reactants each raised to the power their stoichiometric ratios. That is the above reaction is reversed and halved, the new equilibrium constant is: Learn More about equilibrium constant.At 100 ∘C the equilibrium constant for the reaction COCl2(g)←→CO(g)+Cl2(g)has the value Kc=2.19×10−10 Are the following mixtures of COCl2, CO, and Cl2 at 100 ∘C at equilibrium? If not, indicate the direction that the reaction must proceed to achieve equilibrium.Determine Kc for the following overall equilibrium reaction at 700 °C. The equilibrium constant is related to the free energy change by ΔG° = -RTlnKp: ΔG° = -(8.314 J K-1 mol-1)((37 + 273) K) ln Kp = -33 × 103 J mol-1 Kp the reaction vessel to give an equilibrium concentration of NO2(g) of 0.300 M?
Chem 2 Exam 2 Flashcards | Quizlet – 2NO(g) ⇌ N₂(g) + O₂(g). E 0.175M -2x +x +x. Writing the equilibrium constant equation for the given balanced chemical reactionAt 2000oC, the equilibrium constant for the reaction: 2 NO (g) N2 (g) + O2 (g) is Kc = 2.40 103. Effect of Temperature Changes Temperature affects the equilibrium constant: • For an endothermic reaction, heat can be considered a reactant.The important concept to remember here is that equilibrium constant is a thermodynamic quantity that depends on temperature only. Change in Gibbs free energy of reaction and enthalpy are also important state function which help us calculate the equilibrium constant at different temperatures.
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