Nitric oxide gas (NO) reacts with chlorine gas according to the chemical equation given below. NO + %Cl2 The following initial rates of reaction have been measured for the given reagent concentrations. --> NOCI EXPERIMENT [NO') M [C,] M rate (M/hr) 1. 0.50 0.50 1.19 1.00 0.50 4.79 3 1.00 1.00 9.59 What is the rate law (rate equation) for this reaction?

Nitric oxide gas (NO) reacts with chlorine gas according to the chemical equation given below. NO + %Cl2 The following initial rates of reaction have been measured for the given reagent concentrations. --> NOCI EXPERIMENT [NO') M [C,] M rate (M/hr) 1. 0.50 0.50 1.19 1.00 0.50 4.79 3 1.00 1.00 9.59 What is the rate law (rate equation) for this reaction?

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter14: Chemical Equilibrium

Section: Chapter Questions

Problem 14.95QE: Nitrogen, hydrogen, and ammonia are in equilibrium in a 1000-L reactor at 550 K. The concentration...

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7-12 Two kinds of gas molecules are reacted at a set temperature. The gases are blown into the reaction vessel from two tubes. In setup A, the two tubes are aligned parallel to each other; in setup B, they are 900 to each other; and in setup C, they are aligned directly opposite each other. Which setup would yield the most effective collisions?
In a solution at a constant H+ concentration, iodide ions react with hydrogen peroxide to produce iodine. Â H+(aq)+ I(aq)+12 H2O2(aq)12 I2(aq)+H2OThe reaction rate can be followed by monitoring the appearance of I2. The following data are obtained: (a) What is rate expression for the reaction? (b) Calculate k (c) What is the rate of the reaction when 25.0 mL of a 0.100 M solution of KI is added to 25.0 mL of a 10.0% by mass solution of H2O2(d=1.00g/mL) ? Assume volumes are additive.
Nitrogen, hydrogen, and ammonia are in equilibrium in a 1000-L reactor at 550 K. The concentration of N2 is 0.00485 M, H2 is 0.022 M, and NH3 is 0.0016 M. The volume of the container is halved, to 500 L. (a) Calculate the equilibrium constant. (b) Define y as the change in the concentration of nitrogen in the 500-L container. Is y positive or negative? (c) Write the iCe table and express the equilibrium constant in a polynomial in terms of y.
Some sulfuric acid is spilled on a lab bench. You can neutralizethe acid by sprinkling sodium bicarbonate on it and thenmopping up the resulting solution. The sodium bicarbonatereacts with sulfuric acid according to:2 NaHCO31s2 + H2SO41aq2¡Na2SO41aq2 +2 H2O1l2 + 2 CO21g2Sodium bicarbonate is added until the fizzing due to the formationof CO21g2 stops. If 27 mL of 6.0 M H2SO4 was spilled,what is the minimum mass of NaHCO3 that must be addedto the spill to neutralize the acid?
One of the many remarkable enzymes in the human bodyis carbonic anhydrase, which catalyzes the interconversionof carbon dioxide and water with bicarbonate ionand protons. If it were not for this enzyme, the body couldnot rid itself rapidly enough of the CO2 accumulated bycell metabolism. The enzyme catalyzes the dehydration(release to air) of up to 107 CO2 molecules per second.Which components of this description correspond to theterms enzyme, substrate, and turnover number?
For the following reaction 6 experiments have been run and the data collected is in the following table: 2 MnO4-(aq) + 5 H2C2O4 (aq) + 6 H+ (aq) ---> 2 Mn2+ (aq) + 10 CO2 (g) + 8 H2O (l) Experiment [MnO4-], M [H2C2O4], M [H+], M Rate, M/s 1 0.2410 0.3470 0.2690 0.1147 2 0.3260 0.6210 0.2270 0.2776 3 0.5630 0.5740 0.7420 0.4431 4 0.2410 0.3470 0.3840 0.1147 5 0.4140 0.5740 0.5610 0.3258 6 0.3260 0.4930 0.4910 0.2203 a) Find the order of the reaction with respect to H+. _______________ b) Find the order of the reaction with respect to MnO4-. ______________ c) Find the order of the reaction with respect to H2C2O4. _____________ d) What is the overall order of the reaction? ________________________
Balance the following reaction and write the reaction rate. __CH3NH2(g) + __O2 --> __CO2(g) + __H2O(g) + __N2(g)
Consider the following organic reaction, in which onehalogen replaces another in an alkyl halide:CH₃+CH₂+BrKI→CH₃+CH₂I+KBr .In acetone, this particular reaction goes to completion becauseKI is soluble in acetone but KBr is not. In the mechanism, Iapproaches the carbon oppositeto the Br . After Br⁻ has been replaced by I⁻ and precipitates as KBr, other I⁻ ions react with the ethyliodide by the same mechanism.(a) If we designate the carbon bonded to the halogen as C-1,what is the shape around C-1 and the hybridization of C-1 inethyl iodide?(b) In the transition state, one of the two lobes of the unhy-bridized 2porbital of C-1 overlaps a porbital of I, while theother lobe overlaps a porbital of Br. What is the shape aroundC-1 and the hybridization of C-1 in the transition state?(c) The deuterated reactant, CH₃CHDBr (where D is deuterium,2H), has two optical isomers because C-1 is chiral. If the reac-tion is run with one of the isomers, the ethyl iodide is notopti-cally active.…
The white powder of LiHCO3 is unstable and when heated the following reaction occurs: 2LiHCO3(s) → Li2CO3(s) + H2O(g) + CO2(g) A student performed a controlled experiment in which he heated 2.3 grams of LiHCO3 powder and collected the gases into a 1.4-liter container. At the end of the reaction the temperature in the tank was 350 ° C 1.a. Calculate how many grams of Li2CO3 were obtained at the end of the reaction. 1. b. Calculate the tank pressure at the end of the reaction. 1.c. Calculate the partial pressure of CO2 in the tank at the end of the reaction. 2. Answer the following questions for the reactants: CO2, H2O, Li2CO3, LiHCO3 a. Determine which of them has the weakest intermolecular forces. b. Determine which of the substances is a molecular substance with a constant dipole. c. Determine the systematic name for the ionic substances.
The following diagram shows a reaction profile. Label thecomponents indicated by the boxes.
Prof. Neiman and Prof. James were first to discovered in 1973 that chlorofluorocarbons (CFCs) were depleting the Earth’sozone layer when released into the atmosphere. Once they reach the stratosphere, Clis released from the CFCs molecules by interaction with UV light. Free Cl atoms areable to react with ozone in a catalytic cycle that converts O3into the more stable O2.It is estimated that a single Cl atom is able to react with∼100000 O3molecules.Although CFCs production was banned in 1996, there are still a substantial numberof motor vehicle air conditioners (MVACs) that use CFC-12 (CF2Cl2) as refrigerant.The average CFC-12 emission rate from operating MVACs has been estimated tobe 59.5 mg per hour per vehicle (Zhang et al.Environ. Sci. Technol. Lett.2017).How much chlorine, in kg, is added to the atmosphere in a year due to 100 millionMVACs using CFC-12 as refrigerant?
Suppose that for the reaction K + L------->M, you monitorthe production of M over time, and then plot the followinggraph from your data: (a) Is the reaction occurring at a constant rate from t = 0to t = 15 min? (b) Is the reaction completed at t = 15min? (c) Suppose the reaction as plotted here were startedwith 0.20 mol K and 0.40 mol L. After 30 min, an additional0.20 mol K are added to the reaction mixture.Which of the following correctly describes how the plotwould look from t = 30 min to t = 60 min? (i) [M] wouldremain at the same constant value it has at t = 30 min,(ii) [M] would increase with the same slope as t = 0 to15 min, until t = 45 min at which point the plot becomeshorizontal again, or (iii) [M] decreases and reaches0 at t = 45 min.