For the reaction PCl3(g) + Cl2(g) ⟷⟷ PCl5(g) at a particular temperature, Kc = 32.4. Suppose a system at that temperature is prepared with [PCl5] = 0.50 M, [Cl2] = 0.4 M, and [PCl3] = 0.10 M. Which of the following is correct?    Group of answer choices the system will proceed in the direction of forming more PCl3 and PCl5 until equilibrium is reached. the system is at equilibrium. the system will proceed in the direction of forming more PCl5 until equilibrium is reached. the system will proceed in the direction of forming more PCl3 and Cl2 until equilibrium is reached. the system will proceed in the direction of forming more PCl5 and Cl2 until equilibrium is reached.

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4) At high temperatures nitrogen (N₂) and oxygen (O₂) will react to form NO. N₂(g) + O₂(g) 2 NO(g) The value for the equilibrium constant for reaction 4.1 is Kc = 2.7 x 10-¹7 at some temperature T. A system initially has [N₂] = 0.0800 M and [0₂] = 0.0500 M. There is no NO initially present in the system. Find the value for [NO] that will be present at equilibrium. (4.1)

I2(g)+Br2(g) --> 2 IBr(g). Kc= 250. the system is charged with 0.0500 M of I2 and Br2. What value should the student obtain for the equilibrium concentration of IBr(g)?

Equilibrium mixture in a 2.50 L flask at 250 °C in the reaction PCI3(g) + Cl₂(g) →PCI5(g); It contains 0.105 g PCI5, 0.220 g PCI3, and 2.12 g Cl₂. What is the value of (a) Kc and (b) Kp for this reaction at 250 °C? P: 31 g/mol; CI: 35.5 g/mol

Consider the following reaction: 2HI(g) = H2 (g) + I2 (g)   If 2.99 moles of HI(g) , 0.359 moles of H2, and 0.628 moles of I2 are at equilibrium in a 19.6 L container at 859 K, the value of the equilibrium constant, Kc , is .

Consider the equilibrium system described by the chemical reaction below. If the partial pressures at equilibrium of NO, Cl2, and NOCI are 0.095 atm, 0.171 atm, and 0.28 atm, respectively, in a reaction vessel of 7.00 L at 500 K, what is the value of Kp for this reaction? 2 NO(g) + Cl2(g) = 2 NOCI(g)

4. Given the reaction: 3X(g) + Y(g) ↔ 2 Z(g) + W(g)Which of the following is true?a. Kc > Kpb. Kc < Kpc. Kc = Kp5. For the reaction: 2 X(s) + 3 Y(g) ↔ 2 Z(s) Kc = ???At equilibrium, the system contains [Y] = 0.0025 M. The amounts of [X(s)] = 100 mol/Land [Z(s)] = 395 mol/L. What is the value of the equilibrium constant?6. For the reaction: 3A(g) + 2B(g) ↔ 3 C(g) Kc = 0.0245At equilibrium, the system contains [A] = 0.075 M and [B] = 0.115 M. What is theconcentration of C at equilibrium (in M)?7. Given the reaction A(g) + 3B(g) ↔ 2 C(g) Kc = ???Initially, only 0.200 M of C(g) is present. At equilibrium, 0.050 M of A is present. What isthe value of the equilibrium constant?

For the reaction 2SO2(g) + O2g) 2SO3(2) If K. = 4.3 x 10° and the following concentrations are present: [SO2] = 0.010 M, [SO3] = 10 M, [O2] = 0.01 M. Which of the following statements is correct? A. The system is at equilibrium B. The system is not at equilibrium and is shifting from left to right C. The system is not at equilibrium and is shifting from right to left D. There is not enough information E. The system is at equilibrium and is shifting from left to right 3.

Express the equilibrium constant for this reaction:   2 NH3(g) <=>  N2(g) + 3 H2(g)     K = [NH3]2 / ([NH3]2 x [N2])     K = ([NH3]2 x [N2]) / [H2]3     K =  ([N2] x [H2]3) / [NH3]2