Consider the reaction of nitrogen (II) oxide and hydrogen to form nitrogen and [NO] [Hz] Rate(mol/Ls) water. 0.015 0.020 0.60 2NO(g) + 2H2 –→ N2(g) + 2H2O(g) According to these experimental results, what are the orders for NO and H2O? 0.015 0.040 1.20 0.030 0.020 2.40

The rate of a certain reaction is given by the following rate law: rate =k Use this information to answer the questions below. What is the reaction order in N,? What is the reaction order in H2? What is overall reaction order? At a certain concentration of N2 and H2, the initial rate of reaction is 0.820 M / s. What would the initial rate of the reaction be if the concentration of N2 were halved? Round M S your answer to 3 significant digits. The rațe of the reaction is measured to be 47.0 M/s when [N2] = 1.4 M and [H2] = 0.35 M. Calculate the value of the k = M rate constant. Round your answer to 2 significant digits. Continue MacBook Air

A chemical reaction is characterized by the following experimental data: SO₂Cl2 → SO2 + Cl₂ [SO₂Cl₂] Time (mol L-¹) (min) 0.1000 0 0.0876 1.00 x 10² 0.0768 2.00 x 10² 3.00 x 10² 4.00 x 10² 5.00 x 10² 0.0673 0.0590 0.0517 6.00 x 10² 7.00 x 10² 8.00 x 10² 9.00 x 10² 1.000 x 10³ 0.0234 1.100 x 10³ 0.0453 0.0397 0.0348 0.0305 0.0267 First, graphically determine the instantaneous rate of decomposition of [SO₂Cl₂] using the tangent to the curve. Use scientific notation, e.g.enter 2E3 for 2000. Enter your answer with one significant figure. The decomposition rate: (A) at 200 min: i (B) at 600 min: i M/min M/min

A. Consider the following proposed mechanism for the production of chlorine dixoide from chlorine and ozone. Draw a reaction coordinate diagram for this reaction. Label reactants, products, transition states, intermediates, and activation energy on your sketch. Assume the reaction is endothermic. NOTE: CI is chlorine, not Carbon lodide Overall: Cl₂ (g) + 203 (g) → 2 CIO₂ (g) + O₂ (g) Step 1: Cl₂ (g) → 2 Cl (g) fast Step 2: Cl (g) + Os (g) CIO₂ +O fast Step 3: O (g) + O3 (g) → 202 (g) fast Step 4: Cl (g) + O2 (g) → CIO2 (g) slow

Reaction of nitric oxide gas (NO) and chlorine gas (Cl2) produces a very poisonous gas called nitrosyl chloride (NOCl). The experimental data of the reaction is given below. Use the data to calculate the specific rate constant K and overall order of the reaction. Please show full work!

The rate of a certain reaction is given by the following rate law: =k[N₂]²[H₂]² Use this information to answer the questions below. rate What is the reaction order in N₂? What is the reaction order in H₂? What is overall reaction order? At a certain concentration of N₂ and H₂, the initial rate of reaction is 71.0 M/s. What would the initial rate of the reaction be if the concentration of N₂ were halved? Be sure your answer has the correct number of significant digits. The rate of the reaction is measured to be 0.930 M/s when [N₂] = 0.79 M and [H₂] = 0.88 M. Calculate the value of the rate constant. Be sure your answer has the correct number of significant digits. M 04/1 S -3 1 k = M ²³.5²¹ S

23. Consider the following reaction: 2 NO2(g) + O3(g)  N2O5(g) + O2(g) (a) The rate law for this reaction is first order in NO2(g) and first order in O3(g). What is the rate law for this reaction? Rate = k [NO2(g)] [O3(g)] Rate = k [NO2(g)]2 [O3(g)]     Rate = k [NO2(g)] [O3(g)]2 Rate = k [NO2(g)]2 [O3(g)]2 Rate = k [NO2(g)] [O3(g)]3 Rate = k [NO2(g)]4 [O3(g)] (b) If the rate constant for this reaction at a certain temperature is 62500, what is the reaction rate when [NO2(g)] = 0.530 M and [O3(g)] = 1.08 M?Rate =_____  M/s.(c) What is the reaction rate when the concentration of NO2(g) is doubled, to 1.06 M while the concentration of O3(g) is 1.08 M?Rate =____  M/s

A proposed mechanism for the reaction is: - Step 1: H₂(g) + 2NO(g) → N₂O(g) + H₂O(g) Step 2: N₂O(g) + H₂(g) → N₂(g) + H₂O(g) What is the rate law? More information is needed to answer this question. Or = K[H₂][NO] Or = K[H₂]²[NO]² Or = K[H₂][NO]² Or=K[H₂]²[NO] (slow) (fast)

Use the Image to solve these problems.  1. What is the order of this reaction with respect to NO2? 2. Write a rate law for this reaction, and calculate the value of the rate constant (k). (Report in scientific notation to 3 sig figs without units) Rate law: Rate constant (k): 3. Determine the half-life for this reaction.  (Report in scientific notation to 3 sig figs without units) 4. Calculate [NO2] at 2.70 x 104 seconds after the start of the reaction.  (Report to 3 sig figs without units)

Carbon monoxide is a toxic gas that is often produced in oxidation of hydrocarbons, like methane in a furnace. It binds tightly to hemoglobin, preventing oxygen from binding. The rate of the reaction between hemoglobin (Hb) and carbon monoxide (CO) was studied at 20 degrees celcius. The data were collected and are shown in the table.  a. Determine the orders of the reaction with respect to hemoglobin and carbon monoxide. (Fill in the blanks) The reaction is _______ order with respect to Hb and ____ order with respect to CO.  b. Determine the average value of the rate constant k. When you report it, make sure to include units. K=___________ c. Determine the rate when [Hb]0 is 1.872 umol/L and [CO]0 is 0.220 umol/L. Rate=________