Directions: Write your answers on a separate sheet of paper; show answers with little to no work will only receive partial credit even if correct Use this reaction to answer the following questions: CH4(s) +202(g) → CO2(g) + 2H₂O) AH = -35 kJ/mol Kc = 57.3 at 298 K R = 0.0821 L atm/K mol 1. Calculate Kp. ✓2. Write the expression of the equilibrium constant Kc. 3. If [CH4] = 0.1 M, [0₂] = 0.25 M, [CO₂] = 0.35 M, and [H₂O] = 0.15 M, what is the value of Qc? ✓ 4. 5. Which direction should the reaction proceed to reach equilibrium? If the combustion of methane is a zero-order reaction, and [CH4]0= 5.02 M, and k = 1.7 x 10-³ M/sec: a. What is the concentration of CH4 after 10 minutes? b. What is the half-life of the reaction? 6. If the combustion of methane is a first-order reaction, and [CH4]0= 5.02 M, and k = 1.7 x 10-3 M/sec: a. What is the concentration of CH4 after 10 minutes? b. What is the half-life of the reaction? √ 7. If the combustion of methane is a second-order reaction, and [CH4]0 = 5.02 M, and k = 1.7 x 10-3 M/sec: a. What is the concentration of CH4 after 10 minutes? b. What is the half-life of the reaction? ✓ 8. What will happen to the concentrations of CH4, O2, CO2, and H₂O under the following conditions: a. The temperature of the reaction decreases b. The pressure exerted on the reaction increases c. The concentration of CH4 increases d. The concentration of CO₂ decreases