See the attached file. 1. The reversible exothermic water-gas shift reaction (seen in attached file), takes place in an isobaric and adiabatic PFR reactor of V=1m3. Ftot = 100 moles/sec contains 40 mol% H20 and 20 mole % of inert I. The total pressure is 3 bar and the inlet temperature is Tin = 500 k. In parallel the methanatio
Natural sources add sulfur dioxide (SO2) to the atmosphere at a rate of about 1E8 tonnes (S)/yr. The background concentration of atmospheric SO2, measured in remote areas where anthropogenic sources are not likely to have much influence, is about 0.4 parts per billion, by volume. What is the residence time of atmospheri
(a) The zinc-containing enzyme carbonic anhydrase is present in the red blood cells of humans and catalyses the following physiologically important reaction. Please see the attached document for the reaction. Where the carbon dioxide produced during respiration is converted to hydrogen carbonate, which is very soluble in
Please show all work and explain the answer. Question For the reaction A+2B ---> E A. Give the rate law if the mechanism is: 2A+B ---->C (slow) B+C -----> D+A (fast) D--------->E (fast) B. Give the rate law if the mechanism is: 2A+B ------>C (fast) B+C -------> D+A (slow) D----------->E (fast)
Question 1. Write the rate law and give the rate constant for this reaction. 2 ClO2(aq) + 2 OH^-(aq) ---> ClO-3(aq) + ClO2^-(aq) + H2O(l) The following rate data were collected: Experiment----------[ClO2]---------[OH-]-----------initial rate 1----------------------0.060M-------0.030M--------0.0248 M/s 2------------
i am clarifying this is not an assignemt is just practice questions. It was part of an old test that the teacher gave to us to practice . This are practice questions 1. Calculate deltaH for the reaction P4O10 + 6 PCl3 ----? 10 Cl3PO From P4 + 6 Cl2 -----> 4 PCl3 deltaH = -1225.6 kJ P4 + 5 O2 -----> P4O10 deltaH =
For the reaction o(g) + o3(g) --> 2O2(G) the preexponential factor is 4.8 x 10^9 mol s-l . Given the activation energy is 17.1 kJ mol, what is the rate of reaction at 298 k? What is the value of kb for the cyanide anion cn- given that ka= 4x10-4? Report to one significant figure.
For the reaction O(g) + o3(g)--- > 2o2(g) the activation energy is 17.1 kJ/mol. By what factor does the reaction rate increase ongoing from 100k to 200? Consider the reaction A+2B --> 2C. If C is increasing at a rate of 7.0 mol L-1 s-1, at what rate is (A) changing?
Hello: We are to assume a 129 m3 closed tank. The tank previously contained heptane and therefore has residual vapor. The vapor pressure is given and known as 40 mm Hg The temperature is given as 25 degrees C. 1) Is there a way to determine what the residual concentration of heptane gas would be in this closed con
Consider modeling the air over an area to be abox, 100km on each side that reaches an altitude of 1km. Clean mountain air blows into this box from the west with an average speed of 4m/s. A key pollutant is generated in this box at a rate of 10kg/s. The pollutant degrades in proportion to its concentration (k=.2(1/hr)) Find the
HWU3-2 QUESTION: A 1577 kg car is traveling down the road at 81.0 km/h. While traveling at this rate of speed, what is the kinetic energy of this vehicle in kilojoules? Answer: __________ kJ ________________________________________ HINT: Kinetic energy can be found using the formula E_k= 1/2 mv^2 where Ek is kinetic e
1. Express the rate of reaction in terms of products and reactants 2. In the first 15 secs of the reaction, 0.015 mol of O2 is produced in a vessel with 0.500 L volume. What is the average reaction rate for this time interval? 3. Predict the change in N2O over the time interval.
Why are active on-duty firefighters likely to experience the adverse health effects from inhaling 300 ppm of carbon monoxide faster than nonactive off-duty firefighters who inhale the same concentration of the same substance? Explain your answer using the chemicals/process involved.
In the discussion of the Lindemann mechanism, it was assumed that the rate of activation by collisions with another reactant molecule, A, was the same with a non-reactant molecule, M, such as an inert gas. What if the rates of activation for these two process are different? In this case, the mechanism become k1
Solve the conversion problems listed in the assignment section by setting-up the solution equation using the Factor-Label Method.
I am completely lost here and really could use some help. All of the problems require 2 or more conversion factors. Please show all your work, and don't forget the rules of Significant Digits.. hereby known as Sig Digs. Again, let me repeat this... when you do Lab number two.. you must show your work for each problem. S
A step-by-step guide on how to construct a first order kinetics plot and determine rate constant and half life from experimental data [concentration and time]
After applying 2,4-D to turf, an experiment was conducted measuring the concentration of 2,4-D that was present over time. The 2,4-D concentration was 80 ppm on day zero, 45 ppm on day 14, and 6 ppm on day 56. a. Do a first order kinetic plot to determine the rate constant for the disappearance of 2,4-D. b. What is the half
Using this data calculate the rate law for the reaction A + B -> C [A] (M) [B] (M) Initial rate (M/s) 0.10 0.10 0.0092 0.20 0.20 0.0184 0.20 0.40 0.0368
Please can you provide an explanation for the following questions: For the rate law, Rate = k[A]2[B], which of the following is false about the chemical reaction having this rate law? A) Doubling [A] quadruples the rate. B) The reaction is third order overall. C) The chemical reaction must be: 2 A + B â?' C. D) Do
In aqueous solution, iodine reacts with acetone as represented by the following stoichiometric equation: I2 + CH3COCH3---> CH3COCH2I + H+ + Iâ?" The experimental rate law is Rate = k[H+][CH3COCH3] According to the information above, an increase in the hydrogen ion concentration has what effect on the reaction? A) It d
An enzyme is a large protein molecule (typically with a molar mass greater than 20,000 AMU) that has a structure capable of catalyzing specific biological reactions. In general one or more reactant molecules (called substrates) bind to an enzyme at its "active sites" where the reaction the enzyme is responsible for occurs. The g
Provide help with the following problem with the steps: Consider the reaction 2NO(g) + O2(g) --> 2NO2(g) Suppose that at a particular moment during the reaction nitric oxide (NO) is reacting at the rate of 0.066 M/s. (a). At what rate is NO2 being formed? (b) At what rate is molecular oxygen reacting?
In 2000, the US accounted for one-fourth of the total world energy consumption and both the US and world rates were growing at a 3.5 percent annual rate.
In 2000, the US accounted for one-fourth of the total world energy consumption and both the US and world rates were growing at a 3.5 percent annual rate. Suppose the US cut its growth rate to 0.7 percent, while the rest of the world growth propelled by the needs of developing countries, continued to increase by the historic rate
At an altitude of about 35 kilometers, the average concentrations of O* and of CH4 are approximately 100 and 1E11 molecules cm-3 respectively, and the rate constant k for the above reaction is approximately 2.9E-10 cm3 Molecules-1 s-1. Calculate the rate of destruction of methane in molecules per second per cubic centimeter.
Radioactive radon gas (222Rn) enters an average building at a rate of 2 picocuries per second per square meter of foundation area.
Radioactive radon gas (222Rn) enters an average building at a rate of 2 picocuries per second per square meter of foundation area. Consider a house with a foundation of 100 square meters and a volume of 1000 cubic meters. Assume the house if well designed for energy conservation so that the ventilation rate is low and only one t
I missed this question on my exam. Can you show me the correct way to do it? H2O(l)= H+(aq) +OH(aq) If K1(reaction going towards right)= 2.4e-5/second and if K-1(reaction going towards left) = 1.3e11/M.s what is the equilibrium constant K where K= [H][OH]/[H2O]? what are the product values in Moles for [H][OH],
Consider the following reaction: A+B----AB For a certain set of initial concentrations of A and B, it takes 10 seconds to produce 0.1 mmol of AB at 20 degrees celsius and 150 seconds at 0 degrees celsius. What is the ratio of the rate at 20 degrees to that at 0 degrees?
A compound X undergoes two simultaneous first-order reactions as follows: X Y with rate constant k1 and X Z with rate constant k2. The ratio of k1/k2 at 40°C is 9.9. What is the ratio at 280°C? Assume that the frequency factors of the two reactions are the same. I used the equation ln k1/k2=(Ea/R)(T1-T2/T1*T2) my ans
The rate constants of some reactions double with every 10 degree rise in temperature. Assume that a reaction takes place at 291 K and 301 K. What must the activation energy be for the rate constant to double as described? kJ/mol I have no idea where to start on this problem. I can't seem to figure out how to set up the ra
The second-order rate constant for the decomposition of nitrous oxide (N2O) into a nitrogen molecule and oxygen atom has been measured at different temperatures given below. k(1/M·s) t(°C) 1.87 10-3 600 0.0113 650 0.0569 700 0.244 750 Determine graphically the activation energy for the reaction. I took 1/873 wa
For the reaction given below, the frequency factor A is 8.7 1012 s-1 and the activation energy is 63 kJ/mol. NO(g) + O3(g) NO2(g) + O2(g) What is the rate constant for the reaction at 50°C? I used the equation k=Ae^(-Ea/RT) by plugging in the variables I got 8.5e12. But they say this is significantly off. where did i go