2NO(g) + O₂(g) → 2NO₂ (9) For the above reaction, the following data were collected for the rate of disappearance of NO

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2no G O G 2no 9 For The Above Reaction The Following Data Were Collected For The Rate Of Disappearance Of No 1 (42.04 KiB) Viewed 50 times

2no G O G 2no 9 For The Above Reaction The Following Data Were Collected For The Rate Of Disappearance Of No 2 (42.04 KiB) Viewed 50 times

2no G O G 2no 9 For The Above Reaction The Following Data Were Collected For The Rate Of Disappearance Of No 3 (48.78 KiB) Viewed 50 times

2NO(g) + O₂(g) → 2NO₂ (9) For the above reaction, the following data were collected for the rate of disappearance of NO in the reaction: Experiment [NO] (M) (0₂) (M) 0.0126 0.0252 0.0252 1 2 Rate (M/s) 0.0125 1.41 x 10-2 0.0250 1.13 x 10-1 0.0125 5.64 x 10-2 3 The rate constant determined in Part C and the given concentrations are plugged into the rate law determined in Part A to calculate the initial rate of reaction at those concentrations. The rate at which NO disappears is the same rate as the formation of NO₂, the product, based on the stoichiometric relationship depicted in the balanced chemical equation. Part E What is the rate of disappearance of O₂ when [NO] -0.0830 and [0₂] =0.0199 ? Express the rate in molarity per second to three significant figures. 15. ΑΣΦ 4 → rate= .974 Submit Previous Answers Request Answer PE M/s X Incorrect; Try Again; One attempt remaining Plug the given concentrations and rate constant (determined in Part C) into the rate law for this reaction (determined in Part A) in order to solve for the initial rate of reaction. Make certain you take into account the stoichiometry of the reactant and any exponents expressed in the rate law.
Express the rate constant in the provided units to three significant figures. k= 7110 M-2-1 Submit Previous Answers Correct Correct answer is shown. Your answer 7109.293 M-2s1 was either rounded differently or used a different number of significant figures than required for this part. Important: If you use this answer in later parts, use the full unrounded value in your calculations. Plugging the rate of reaction and concentrations from Experiment 1 into the rearranged rate law (from Part A). gives a rate constant of 7.11 x 10³ M2s¹ For Experiment 2, the calculated rate constant is 7.12 x 10³ M2s¹, and for Experiment 3, the calculated rate constant is 7.11 x 10³ M²s¹ Averaging those three rate constants provides a more accurate rate constant for the reaction because it minimizes the contribution of measurement error. ▾ Part D What is the rate of disappearance of NO when [NO] = 0.0830 and [0₂] = 0.0199 ? Express the rate in molarity per second to three significant figures. rate= 0.975 M/s Submit Previous Answers A