ChE201 HW6

For the decomposition rate constant of methyl acetoxypropionate (=A) CH3COOCH(CH3)COOCH3(g) → CH3COOH(g) + CH2=CHCOOCH3(g) a value 0.0317 s-1 was found at 610 K. The decomposition is carried out at this temperature in a closed vessel having a volume of 20 dm³. This reactor initially contained 0.4 moles of pure acetoxypropionate. Assuming ideal gas phase behaviour, calculate: a) what will be the composition of the reaction mixture (in mole%) after 90 s from the start of the reaction, b) reactor pressure at this time.

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5.10. A reaction 3A → B is carried out in a batch reactor. Molar con- centrations of A and B are monitored with time. Determine the appropriate reaction model based on the following data: 1. d 0.0 0.5 1.0 1.5 2.0 2.5 3.0 3.5 4.0 4.5 5.0 [A]. mol/m² 15.0 13.2 10.8 8.2 5.6 3.6 2.2 1.3 0.7 0.4 0.2 (B). mol/m 1.0 1.6 2.4 3.3 4.1 4.8 5.3 5.6 5.8 5.9 5.9

Q2: Methylamine using the following gas-phase reaction: 2 CH,NH, + (CH3),NH + NH, This reaction converts the methylamine to dimethylamine at 130°C, using a silica-alumina catalyst. The molar flow rate into a packed-bed reactor is 30 mol/s and the entering pressure is 16 atm. Assume there is no pressure drop or temperature change in the reactor. The reaction rate follows an elementary rate law. mol k = 4.25 x 10-6 and K, = 2.5 2 atm gcatalyst s a) Write the rate law solely in terms of conversion. b) What is the equilibrium conversion, Xe? c) How many kilograms of catalyst would be needed to load in a PBR to obtain a conversion of 0.9Xe? d) Plot X, and rate law interms of catalyst weight.

2. Consider a gas-phase reaction: A + 2B → C that takes place in a packed-bed reactor (PBR) with a catalyst volume of 0.2 L. The feed rate of A is 0.1 mol/s and the feed rate of B is 0.2 mol/s. The reaction rate constant is 0.01 L/(mol*s) and the pressure drop across the catalyst bed is 2 bar. What is the conversion of A at the exit of the reactor?

A 1000 L completely mixed reactor contains a chemical that undergoes first-order decay with a rate constant of 0.4 /day. The reactor receives an inflow of 100 L/day with a concentration of 50 mg/L. The initial chemical concentration in the reactor is 200 mg/L. Predict the concentration in the effluent in mg/L at: (i) steady-state (ii) after 4 days.

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PREV 1 2 3 NEXT Based on your ICE table (Part 1) and the definition of Kb, set up the expression for Kb in order to determine the unknown. Each reaction participant must be represented by one tile. Do not combine terms. Kb = [0] [0.50] (x) [x +4.20] [x - 4.20] [x+6.3 x 10 < PREV 1 [2x] = 3.8 × 10-10 RESET [4.20] [6.3 x 10-5] [1.6 × 10-19] [3.8 × 10-19] [x-6.3 x 10] [x+1.6 × 10-9] [x-1.6 x 10-19 [x+3.8 x 10-9] [x-3.8 x 10-19 2 3 Based on your ICE table (Part 1) and the equilibrium expression for Kb (Part 2), determine the original concentration of C6H5NH3+. [C6H5NH3+] = M RESET 0 8.3 × 1010 0.86 1.2 10 2.1 0.50

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Consider a pseudo-first order rate constant for the degradation of MTBE in a fully mixed batch reactor that is equal of k' = 0.054min - 1 What will be the half life of MTBE in the reactor in units of minutes (min)?- will a reaction time of 1 minute be sufficient to get 50% removal of the MTBE?

A stream of ozone-enriched air (3% ozone by volume) is bubbled into a reactor as part of a disinfection strategy. Water entering the reactor is free of ozone. KH = 0.011 M/atm and KLa = 18 h-1 for ozone in this system.   Ozone (O3) dissolved in water is unstable. The kinetics of decomposition are complex, but the rate can be approximated as first-order with respect to dissolved ozone. The first-order rate coefficient is pH-dependent and, at pH 8.0 and 25 C, is 12 h-1 in the system of interest.   Find the steady-state concentration (mg/L) of dissolved ozone in the effluent if the reactor is operated as a CMFR with a 15-min retention time

Analyze the following reaction mechanism: 1. H2O2 → H2O + O 2. O + CF2CI2 → CIO + CF2CI 3. CIO + O3 → CI + 202 4. Cl + CF2CI → CF2CI2 From the mechanism provided, write the overall balanced equation for this chemical reaction. Ignore phases. 4- 2. 2+ 3+ 4+ 1 2 3 4 6 8 04 O6 Do 1 3 8. (s) (1) (g)|(aq) + F CI H C Reset • x H2O || Delete 3.

The reaction A → R+S with rate -rA = k (0th order) occurs in a batch reactor that operates under isothermal and isobaric conditions (assume that g = 1). The initial reaction mixture contains reactant A only. The half-life of the reaction (i.e., CA = CA0/2) is t1/2 = 10 min. Calculate the time required for the reaction to be completed (i.e., CA = 0). 2. %3D

TM 31.7 & O 32 |14 5:50 TNT K/s Gen-Chem-2-Activity OBSERVE THE UNIQUE PROPERTIES OF WATER IN EVERYDAY LIFE Directions: Read and analyse the scenarios provided below about unique properties of water. The students should give the answer they feel most sure about and can be backed up by identifying other potential answers. Scenarios 1. It is a sweltering day at an outdoor concert. You walk through a misting booth, which sprays fine water droplets onto you, and for a few minutes afterward you feel much cooler. 2 You're on a road trip through the desert. You stay in a hotel with a swimming pool. Even though it's been scorching hot all day, you dive in without fear 3. You go for a hike and decide to add a powdered energy drink to your water bottle. You sprinkle in the powder and it quickly dissolves. 4. In chemistry class, you pour water into a graduated cylinder. You carefully take note of the meniscus that forms at the top 5. While sitting by the edge of a stream, you observe that some…

D Question 31 The rate of a liquid phase reaction of the type, A + B → Products; is found to be independent of concentration of A and B, and equal to 1 Kmol/(m³)(min) at 300 K. find the conversion in a mixed flow reactor having volume 2 m³ with feed concentration of A and B equal to 5 kmol/m³, feed flow rate equal to 1 m³/min and reactor temperature equal to 300 K. If the activation energy of the reaction is given as 83.1 kJ/mol find the volume (m³) of the isothermal plug flow reactor for the same conversion and feed conditions as in the case of the above- mentioned reactor but with reactor temperature kept at 320 K. 0.42 O NOTG 0.50 0.33 0.20

Reaction in an ideal gas system A2(g) + 3 B2(g) → 2 AB3(g) takes place at a temperature of 860 K in a reactor with a volume of 5.0 dm³. At the point, when 75% of the initial amount of substance B2 reacted, the substance amount of this component decreases rapidly: 6.0-104 mol min-1. Determine the reaction rate at the given moment.

1- In the enzymatic reaction that took place in the batch constant volume reactor, the reaction rates were measured at different initial concentrations and are given in the table below. Find the appropriate kinetic model and coefficients Substrate cconcentration (mM) 1 2 4 16 32 Reaction rate (mmol/L min) 1 1.8 3.2 6.6 7.8

Can please do a step by step explanation

From the equation of the line of best fit for the temperature-rate constant data in Part C, y= -22314x + 25.181 determine the value of Ea in kJ/mol. Include a unit analysis. R is a constant equal to 8.314 J/molK. When you take the natural log of a number, the units disappear.

The following irreversible reaction takes place in a batch reactor? → B Consider the same reaction, first-order irreversible reaction with respect to A. The concentration of A after one minute is 2 mol dm-3. If k is the same (k = 1 min-1), determine the initial concentration of A.

liquid phase reaction:trityl (A) + methanol (B) -> product a batch reactor was carried out at 25°C in excess solution (Cb0 = 0.5 mol/dm^3). The pyridine reacts with HCL, which then precipitates as pyridine hydrochloride making the reaction irreversible. the order of the reaction with respect to the methanol concentration (B) is order 1. The concentration of triphenyl methyl chloride (A) is measured as a function of time and is shown below. -ra = kCa x Cb it is assumed that the value of Cb is almost always constant, or Cb = Cb0-rA = kCb0 x CA^x-rA = k1 x CA^x   use the integral method to ensure that the reaction is second order with respect to triphenyl methyl chloride

Which of the following must be true if the steady state assumption is to be used? Ok₁[E][S] = k₂[ES] d[ES]/dt = 0 O[E]T=[ES] k₁[E][S]=k₂[ES] -k.₁[ES] (k₂-k.1)/k₁ = 1