Hello, Im a chem 122 student.. I need help with the problems listed here. Thanks in advance.

Worksheet 1 - CH 14 & 15 (10 points) 1. For the reaction: 2 NO (g) + O2(g) 2 NO2 (g), given the following data determine the rate law and the rate constant (with correct units). Exp # No1 [02] Rate (M/s) 0.0010 0.0010 7.10 2 0.0040 0.0010 28.4 0.0040 10.0030 255.6 1 3 2. For the reaction: 2 A+B 3 C the rate of disappearance of B was 0.30 M/s. What is the rate of disappearance of A and the rate of appearance of C? 3. The decomposition reaction: SO2Cl2 SO2 + Cl2, has a first order rate constant of 2.2 x 10- stat 320 C. If the initial concentration of SO2Cl2 is 0.0040 M, what will be its concentration be (a) after 1.00 hr and (b) after 1.00 day? 4. The decomposition reaction 2 HI(g) H2(g) + 12 (g), is second order and has a rate constant equal to 1.6 x 10- M's' at 700 C. If the initial concentration of HI in the container is 3.4 x 10-M, how many minutes will it take for the concentration to be reduced to 8.0 x 104 M? 5. The conversion of cyclopropane to propylene is first order and has a rate constant of 1.3 x 10 s' at 400C. The rate constant is 1.1 x 10's' at 430C. What is the activation energy in kJ/mol? Rev: 9/3/2020 Worksheet 1 - CH 14 & 15 (10 points) 6. The partial pressures in an equilibrium mixture of NO, Cl2, and NOCI at 500 K are as follows: PNo = 0.240 atm, PC12 = 0.608 atm, and PNoci = 1.35 atm. What is Kp at 500 K for the reaction: 2 NO (g) + Cl2(g) + 2NOCI (g)? 7. At 700 K, Kp = 0.140 for the reaction: CIF: (g) = CIF (g) + F2 (g) Calculate the equilibrium partial pressures of CIF, CIF, F2 if only CIF3 is present initially at a partial pressure of 0.978 atm. 8. If a mixture of reactants and products contains 0.035 M H20, 0.050 M CH4, 0.15 M CO, and 0.20 M Hz. For the reaction: H20 (g) + CH4 (g) = CO (g) + 3 H2(g) Kc = 4.7 at 1400 K. In which direction does the reaction proceed to reach equilibrium? What is the value of Kp? 9. Write the equilibrium constant expression Kc for: C2H5OH (aq) + O2 (aq) = CH3CO, H (aq) + H20 (1) 10. The equilibrium constant Kp for the reaction (CH3)CCI(g) = (CH3)2C=CH2(g) + HCl (g) is 3.45 at 500. K. (5.00 x 10K) Calculate the value of Kc at 500. K. For the same reaction, calculate the molar concentration of reactants and products at equilibrium if initially 1.00 mol of (CH3)3CCI was placed in a 5.00 L vessel