Help me plsss..  *For the reaction N2(g) + O2(g) ↔ 2 NO(g), Kc = 4.080×10–4 at 2000 K. What is the equilibrium concentration of N2 and O2, for the reaction 2 NO(g) ↔ N2(g) + O2(g) if the initial concentration of NO is 0.1000 M? *Following the problem above, what is the equilibrium constant of the reverse reaction used? *Following the problem above, if the reaction is reduced to decomposition of 1 mole NO, what is the value of the equilibrium constant?

For the reaction H₂(g) + CO₂(g) → H₂O(g) + CO(g) at 700 °C, K=0.534. Calculate the number of moles of H₂ that are present at equilibrium if a mixture of 0.660 mole of CO and 0.660 mole of H₂O is heated to 700 °C in a 30.0 L container. Round your answer to 3 significant digits. mol x10 X

At a certain temperature, the reaction: PCl5(g) ⇆ PCl3(g) + Cl2(g) has an equilibrium constant Kc = 5.7E-6.  Calculate the equilibrium concentration of PCl3 if only PCl5 is present initially at a concentration of 0.30 M.  Your answer should have two significant figures.

[NH₂] = 3.6 X 102 mol L- 12.34 The equilibrium constant for the reaction, 3 H₂(g) + N₂(g) 22 NH3(g), at a given temperature is 1.4 x 10-7. Calculate the equilibrium concentration of ammonia, if [H₂] = 1.2 X 102 mol L¹ and [N₂] = 3.2 x 10³ mol L-¹.

At 700 K, the reaction 2SO2(g) + O2(g)    2SO3(g) has the equilibrium constant Kc = 4.3 × 106, and the following concentrations are present: [SO2] = 0.010 M; [SO3] = 10. M; [O2] = 0.010 M. Which of the following is true based on the above? a) Qc< Kc , the reaction proceeds from left to right to reach equilibrium b) Qc= Kc, the reaction is currenty at equilibrium c) Qc > Kc, the reaction proceeds from right to left to reach equilibrum d) Qc > Kc, the reaction proceeds from left to right to reach equilibrium e) Qc < Kc, the reaction proceeds from right to left to reach quilibrium

1

A chemist is studying the following equilibirum, which has the given equilibrium constant at a certain temperature: 3 O,(g) = 203 (g) K, =7. × 107 р He fills a reaction vessel at this temperature with 13. atm of oxygen gas. Use this data to answer the questions in the table below. Can you predict the equilibrium pressure of O3, using only the tools | Oyes x10 available to you within ALEKS? no If you said yes, then enter the equilibrium pressure of O, at right. atm Round your answer to 1 significant digit.

3. If the equilibrium constant K, for the reaction 2 NO (g) + O2(g) = 2 NO2 (g) is 5.0 x 1012 at a given temperature, what is the value of the equilibrium constant K, for each of the following reactions at the same temperature? a) NO (g) + ½ O2 (g) → NO2 (g) b) 2 NO2 (g) = 2 NO (g) + 02 (g) c) NO2(g) = NO (g) + ½ 02 (g)

Picture 1 is A) And  Picture 2 is B)

(Data attached in picture)