Consider the reaction: 2NO(g) + 02(g) → 2NO2(g) Suppose that a particular moment during the reaction nitric oxide (NO) is reacting at a rate of-0.010 M/s (with the rate expressed as a negative number since NO is a reactant). At what rate is molecular oxygen reacting?

Determine the rate law and the value of k for the following reaction using the data provided. 2 NO(g) + O2(g) → 2 NO₂(g) [NO]i (M) [0₂]i (M) 0.030 0.030 0.060 A) Rate = 57 M-1s-1 [NO][0₂] B) Rate = 3.8 M-1/2-1[NO][0₂]¹/2 C) Rate = 3.1 x 105 M-³s-1 [NO]²[0₂]² D) Rate = 1.7 × 103 M-2s-1 [NO]²[0₂] E) Rate = 9.4 × 103 M-²s-1 [NO][0₂]² 0.0055 0.0110 0.0055 Initial Rate (M-1,-1) 8.55 × 10-3 1.71 × 10-2 3.42 × 10-2

Part B

Methane and water react to form carbon monoxide and hydrogen, like this: CH₂(g) + H₂O(g) → CO(g) + 3H₂(g) 2 Imagine 169. mmol of CH4 and 169. mmol of H₂O are added to an empty flask, and then answer the following questions. What is the rate of the forward reaction before any CH4 or H₂O has been added to the flask? What is the rate of the forward reaction just after the CH4 and H₂O has been added to the flask? What is the rate of the forward reaction at equilibrium? How much CH4 is in the flask at equilibrium? Zero. Greater than zero, but less than the rate of the reverse reaction. Greater than zero, and equal to the rate of the reverse reaction. Greater than zero, and greater than the rate of the reverse reaction. Zero. Greater than zero, but less than the rate of the reverse reaction. Greater than zero, and equal to the rate of the reverse reaction. O Greater than zero, and greater than the rate of the reverse reaction. Zero. Greater than zero, but less than the rate of the reverse…