Suppose the decomposition of dinitrogen monoxide proceeds by the following mechanism: step elementary reaction rate constant 1 N,0 (g) → N, (g) + 0 (g) 2 N,0 (g) +0 (g) - N, (g) + 0, (g) k2 Suppose also k, « k,. That is, the first step is much slower than the second. Write the balanced chemical equation for the overall chemical reaction. Write the experimentally- observable rate law for the overall chemical reaction. rate = k|I Note: your answer should not contain the concentrations of any intermediates.

The following initial rate data are for the reaction for the formation of phosgene from carbon monoxide and chlorine: со + Clz → COCI2 Initial Rate, Ms-1 Experiment [CO]o, M [CIz]o, M 2.45 0.399 1.43x10-28 2 2.45 0.798 |2.85х10-28 3 4.90 0.399 2.85x10-28 4 4.90 0.798 5.71x10-28 Complete the rate law for this reaction in the box below. Use the form k[A]m[B]^ , where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n Rate = From these data, the rate constant is M-1s-1.

KINETICS AND EQUILIBRIUM Identifying intermediates in a reaction mechanism Consider the following mechanism for the reduction of nitric oxide: H₂(g) + 2NO(g) → N₂O(g) + H₂O(g) H₂(g) + N₂O(g) → N₂(g) + H₂O(g) Write the chemical equation of the overall reaction: Are there any intermediates in this mechanism? If there are intermediates, write down their chemical formulas. Put a comma between each chemical formula, if there's more than one. ☐ yes no (1) (2) ローロ 00 09 0.0.... X Ś 0/3

Consider the following general reaction for which gases A and B are mixed in a constant volume container: A(g) + B(g) -> C(g) + D(g) Match what happens to the rate of the reaction under the following changes: (consider each change separately) v all of gas B is removed from the container more gas A is added to the container the temperature of the container is increased there is no change to the reaction rate ya catalyst is added to the container I. the reaction proceeds at a faster rate v gas D is also added to the container the reaction proceeds at a slower rate II. some of gas B is removed from the container Iy the reaction does not proceed at all the volume of the container is increased

Without a catalyst, the activation energy of a reaction is 162.9 kJ/mol. With a catalyst, the activation energy is 92.8 kJ/mol. Assuming the frequency factor (A) and the initial concentrations of all reactants are the same for each reaction, how many times faster is the initial rate of the catalyzed reaction at 37.4°C? IMPORTANT: When entering your answer: • Enter whole numbers only (no spaces, letters, or other characters) • Enter a number for the coefficient rounded to the units column (regardless of significant figures) • Enter a number for the power of 10 (the exponent only) Example: for 6.022 x 102, you would enter 6 and 23 The catalyzed rate is × 10^ times faster than the uncatalyzed rate

Enter your answer in the provided box Consider the reaction: 2NOG) - 0,g) - 2NO,() Suppose that a particular moment during the reaction nitric oxide (NO) is reacting at a rate of 0.034 Mis. At what rate is molecular oxygen reacting? Molecular oxygen is consumed at a rate of

Consider this reaction: 2NH, (g) - N2 (g) +3H, (g) At a certain temperature it obeys this rate law. rate =(0.0103 s")[NH,] S Suppose a vessel contains NH, at a concentration of 0.170M. Calculate the concentration of NH, in the vessel 68.0 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. OM x10

Question 17 of 23 Submit Butadiene reacts to form a dimer according to the equation 2C,H6(g) → C3H12(g) The reaction obeys the second order rate law, Rate = k[C,H,]?, with a rate constant k = 3.68 M-'min at a certain temperature. Starting with an initial concentration of [C,H] = 0.0500 M, what will be the butadiene concentration after 31.0 min? | M 1 2 3 C 7 9. +/- x 10 0 LO 00

The decomposition of N»Os(g) to NO2(g) and O2(g) obeys first-order kinetics. Assuming the form of the rate law is: A[N,05] Rate = *[N,Os] At where k = 3.4 x 10-5 s-l at 25°C, what is the initial rate of reaction at 25°C where [N2O5]o = 4.1 x 10-2 M? а. 1.4x 10-6 mol/L's b. 3.4 x 10-5 mol/L's О с. 8.3 х 10-4 mol/L s d. 4.1 x 10-2 mol/L's e. none of these

Given below is the data for the reaction. Calculate the value of the rate constant "k" with proper units. A + B → C Set [A] (M) [B] (M) Init, rate M-sec 1 0.050 0.200 5.0 x 10-5 2. 0.100 0.200 5.0 x 10-5 0.050 0.600 4.5 x 10-4 Determine the order in "A" Determine the order in "B" Substitute the order for A and B in the rate law equation below. Rate = k [A]' [B]