A researcher is studying the decomposition of A as shown by the general reaction below: 3 A(g) 2 B(s) + 1 C(g) Initially, the scientist fills an evacuated 5.368 L flask with 6.020 x 10-1 moles of species A. Upon equilibrium, it is determined that the concentration of A is 4.620 x 10-2 M. Calculate Kc.

Label the following statements as true or false.    1) If Kc=5 for the reaction A + B <--> AB, then AB <--> A + B has a Kc=0.2   2)  When a system is at equilibrium, the reactants and the products of the reaction will be equal in concentration.    When Q > Kc, the reaction shifts to the left to reduce stress on the system.    3) When a system is at equilibrium, the reaction rate of the forward reaction is less than to the reaction rate of the reverse reaction.    4) When Q < Kc, the reaction shifts to the left to reduce stress on the system.    5) For a reversible reaction, the ΔH of the forward reaction is equal in magnitude but opposite in sign to the ΔH of the reverse reaction.

5. The reaction: 2NO₂(g) + 7H₂(g) = 2NH3(g) + 4H₂O(g) was allowed to reach equilibrium at 455 K. Analysis showed that there was 34.6 g of NO2, 53.2 g of H₂, 52.6 g of NH3 and 87.4 g H₂O present in a 2.65 L vessel once equilibrium was achieved. a. Determine the equilibrium concentration for both reactants. b. Determine the equilibrium concentration for both products. C. Write the Kc expression. d. Solve for the Kc. e. Solve for the Kp at the same temperature.

H2 + I2 → 2 HI At a certain temperature, the Kc of this reaction is 58.2. At this temperature, 5.00 mol H2 and 5.00 mol I2 were placed in a 0.500 L container to react. What concentration of HI is present at equilibrium?

Please help me solve both questions I’m begging

Nitesh

Enter your answer in the provided box. The equilibrium constant for the reaction is 6.8 × 103 at a certain temperature. 2SO2(g) + O2(g) = 2SO3(g) If at equilibrium, [SO2] = 0.0611 M and [GE] = 0.07 M, what is the equilibr 1.33 X

7. Consider the following equilibrium: 2NOCI(g) = 2NO(g) + Cl2(g) K = 1.56 x 10-5 If 2.00 moles of pure nitrogen monoxide and 3.00 moles of pure chlorine gas are placed in a 2.00-L container, calculate the concentration of Cl2(g) once the reaction has reached equilibrium.

1. The diagrams below represent the following reversible chemical reaction: H2(g) + 12 (g) =2 HI (g) At 448 °C, the equilibrium constant, K, for this reaction is 51 Initial Conditions: Temperature = 448 °C Volume of the container = 2.0 L 0 = 1 mole H2 (g) = 1 mole I2 (g) 00 00 .. 00 00 •. What is the initial molar concentration of hydrogen. [H:]? What is the initial molar concentration of iodide, [I2]? M This system will reach equilibrium when rate of the forward reaction is equal to the rate of the reverse reaction. Write the equilibrium constant expression, Kc, for this reaction: Calculate the equilibrium concentrations for H;(g), I (g) and HI (g) H2(g}_ + l2 (g) 2 HI (g) [H2] [L2] [HI Initial Change Equilibrium +2x -X-

KINETICS AND EQUILIBRIUM Using the general properties of equilibrium constants At a certain temperature, the equilibrium constant for the following reaction is 0.83: Cl₂(g) + CHC1₂(g) →HC1(g) + CC14(g) Use this information to complete the following table. Suppose a 38. L reaction vessel is filled with 2.0 mol of Cl₂ and 2.0 mol of CHCI 3. What can you say about the composition of the mixture in the vessel at equilibrium? What is the equilibrium constant for the following reaction? Be sure your answer has the correct number of significant digits. HC1(g) +CC1₂(g) C1₂(g) +CHC13 (9) What is the equilibrium constant for the following reaction? Be sure your answer has the correct number of significant digits. 2 C1₂(g) +2CHC13 (9) 2 HC1(g) + 2CC14(9) There will be very little Cl₂ and CHCl3. There will be very little HCI and CCl4. Neither of the above is true. 0 0 0 x10 X 3 1/5