SECTION 3 (AC3.1/AC3.2) (A) After experimentation you have determined the following rate equations: 1. Rate = K[H₂] [NO]² 2. Rate = K[H₂]² [0₂] 3. Rate = K[H²] [NO] Identify the order of reaction for each of these rate equations. You must show your workings within your submission, and explain your reasoning. Your explanation should be a maximum of 300 words. (B) Through experimentation, you note that at high temperatures ethyl chloride produces HCI and ethylene by the following reaction: CH3CH2Cl(g) → HCI(g) + C2H4(g) Using the rate data for the reaction at 650°C presented in the following table, calculate the reaction order with respect to the concentration of ethyl chloride (CH3CH2CI). You must show your workings within your submission, and explain your reasoning. Your explanation should be a maximum of 300 words. Experiment [CH3CH2CI]. (M) 1 0.010 2 0.015 0.030 0.040 3 4 Initial Rate (M/s) 1.6 x 10-8 2.4 x 10-8 4.8 x 10-8 6.4 x 10-8

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