5. For the following chemical reaction. 2NO(g) + O2(g) -> 2NO(g) Use the experimental data shown below and the method of initial rates to determine the complete rate law for the reaction. Show your work. [5]
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Consider the following reaction: 2NO(g)+O2(g)⇌2NO2(g)2NO(g)+O2(g)⇌2NO2(g) The data in the table show the equilibrium constant for this reaction measured at several different temperatures. Temperature K 400 1.9x10^7 425 2.5x10^6 465 1.6x10^5 515 8.8x10^3 600 2.0x10^2 Use the data to find ΔrS∘ΔrS∘ for the reaction. (answer in J K-1 mol-1) The answer is NOT 158
2. Good question. The reaction 2NO(g) + O2(g) → 2NO.(g) was studied by a CHEM 154 student and the following data were obtained for the rate of consumption of oxygen. Write the rate law for this reaction. What would be the initial rate for an experiment where [NO), = 1.03 x 10-mol/L and [O),= 1.22 x 102 mol/L? Expt. [NO], (M) (01. (M) Initial rate (M/s) 1 1.66 x 10-3 1.66 x 10-3 3.32 x 10-5 2 4.98 x 10-...
Consider the reaction 2NO(g) -N2(g) + O2(g). Identify which one of the following rates of reaction is TRUE. rate = -A[N]/At rate = -A[NO]/2At rate = -2A[NO] At rate = A[O2]/2At rate = 2^[NO]/At
4. . The reaction 2NO(g) + O2(g) → 2NO2(g) has the following rate law: Rate = k[O2][NO]2 . If the concentration of NO is reduced by a factor of two, the rate will __________
N2 (g) + O2 (g) --> 2NO (g) The following data was recorded: Exper [N2] [O2] Rate 1 0.04 0.02 707 mol/Lsec 2 0.04 0.01 500 mol/Lsec 3 0.01 0.01 125 mol/Lsec Determine the rate law.
1. Nitrosyl chloride is produced from the reaction of nitrogen monoxide and chlorine: 2NO(g) + Cl2(g) → 2NOCI(g) The following initial rates at a given temperature were obtained for the concentrations listed below. Experiment Initial Rate (mol:L-.h-1) [NO]. (mol.L-1 [Cl2]. (mol.L-1). 2.21 8.84 0.5 0.25 4.42 0.25 0.5 What is the experimental rate law? 0.25 0.25
Consider the following reaction: 2NO(g)+O2(g)⇌2NO2(g) The data in the table show the equilibrium constant for this reaction measured at several different temperatures. Temperatures: Kp: 170K 3.8*10^-3 180K 0.34 190K 18.4 200K 681 Part A Use the data to find ΔH∘rxn and ΔS∘rxn for the reaction. i found ΔH∘rxn = 114 kJ but i dont know how to get ΔS∘rxn. please help and show work
Consider the following equilibrium system. N2(g) + O2(g) ⇌ 2NO(g) a) Write the chemical equation for the forward reaction. (Use the lowest possible coefficients. Use the smaller blank lines to specify states such as (aq) or (s). If a state is not needed, leave it blank. ___________ ___ + ___________ ___ -----------> ___________ ___ b) Write the chemical equation for the reverse reaction. (Use the lowest possible coefficients. Use the smaller blank lines to specify states such as (aq) or...
Using The Following Data, Determine the Rate Law For The Reaction. Part A. 2NO(g)+O(g) --> 2NO2(g) Experiment [NO] [O2] Initial Rate (M/s] 1 0.0126 0.0125 1.41x10^-2 2 0.0252 0.0250 1.13x10^-1 3 0.0252 0.0125 5.64x10^-2 Part B. S2O8charge2-(ag)+3 I charge 1-(aq) ----> 2SO4charge2-(aq)+I3charge1-(aq) Experiment [S2O8charge2-] [ I charge1-] Initial Rate (M/s) 1 0.023 0.048 6.8x10^-6 2 0.054 0.048 1.6x10^-5 3 0.054 0.019 6.3x10^-6
3. Consider the following reaction and its rate law. Answer the following questions. 2NO(g) + O2(g) → 2NO2(g) Rate = k[NO] [2] a. True or False The reactions order with respect to NO(g) is 2 due to the stoichiometry of the reaction. b. True or False The overall reaction order is 3. C. True or False change in the value of k. If the temperature of the reaction is changed we expect a d. What would happen to the rate...