An exothermic, aqueous phase, irreversible, first order reaction, Y Z is carried out in an ideal continuous stirred tank reacto (CSTR) operated adiabatically at steady state. Rate of consumption of Y (in mol liter"minute) is given by 6500 -1; = 10°e TC; Where C, is the concentration of Y (in mol liter), and T is the temperature of the reaction mixture (in K). Reactant Y is fed a 50°C. Its inlet concentration is 1.0 mol literand its volumetric flow rate is 1.0 liter minute. In addition, use the following data and assumptions Heat of the reaction = -42000 Jmol" • Specific heat capacity of the reaction mixture = 4.2 g K • Density of the reaction mixture = 10000 g liter Heat of the reaction, specific heat capacity and density of the reaction mixture do no vary with temperature Shaft work is negligible If the conversion of Y at the exit of the reactor is 90 %, the volume of the CSTR (in liter) is (round off to 2 decimal places)

A chemical engineer is studying the following reaction: BF3(aq)+NH3(aq) → BF3NH3(aq) At the temperature the engineer picks, the equilibrium constant K, for this reaction is 1.1. The engineer charges ("fills") three reaction vessels with boron trifluoride and ammonia, and lets the reaction begin. She then measures the composition of the mixture inside each vessel from time to time. Her first set of measurements are shown in the table below. Predict the changes in the compositions the engineer should expect next time she measures the compositions. reaction vessel compound concentration expected change in concentration BF 3 0.64 M O f increase OI decrease O (no change) A NH, 0.90 M O f increase OI decrease O (no change) BF;NH; 0.63 M O f increase O! decrease (no change) BF3 0.84 M O f increase O! decrease O (no change) В NH, 1.19 M O f increase OI decrease O (no change) BF;NH, 1.09 M O 1 increase OI decrease (no change) BF3 0.38 M O t increase OI decrease O (no change) NH, 0.64 M O t…

An electron in a hydrogen atom is excited from the ground state to the n = 3 state. True or false? (i) The n = 3 state is the first excited state. (ii) It takes more energy to ionize (remove) the electron from n = 3 than from the ground state. (iii) The electron is farther from the nucleus (on average) in n = 3 than in the ground %3D state. (iv) The wavelength of light emitted when the electron drops from n = 3 to n = 1 is longer than that from n = 3 to n = 2.

As reported in US Patent 4203923, cyclohexanone is an important chemical raw material in the production of nylon intermediates. The separation and purification section for cyclohexanone production usually done through a series of distillation units. Liquid mixture of cyclohexanone (1) and phenol (2) was reported to exist in equilibrium with its vapor at 144 °C (417.15K). The system conforms closely to Modified Raoult’s Law. The mixture forms azeotrope at composition of 0.695. (Refer Table) (a) Provide a sketch that clearly shows that the system exhibits azeotrope(α12)x1=0 = P1sat eA / P2sat and (α12)x1=1 = P1sat / P2sat eA (b) State Paz and sketch a P-xy diagram of the system

Consider the following reaction in a sealed vessel kept at constant temperature: A(g)  ⇌  2B(g) If the reaction is started with 2.0 mol of A and no B, the amount of B at equilibrium is 3.0 mol. How many moles of A should one start with to obtain 6.0 mol of B at equilibrium under the same conditions (same vessel, same temperature, no gas B present initially)?   A.  5.6 mol   B.  5.0 mol   C.  4.0 mol   D.  6.0 mol   E.  6.5 mol

I have few minutes left please answer ASAP I will give like

You are in a research & development team responsible for generating preliminary data for the following gas-phase reaction: CO₂(g)+ 4H₂ (g) → 2 H₂O (g) + CH.(g) The reaction occurs over a catalyst at a reactor pressure of 1 atm and 500 C and goes essentially to completion. Use the following heat capacities data for your calculation: CO₂ (g): H₂ (g): H₂O (g): CH₁ (g): Cp=0.0451 kJ/mol C Cp = 0.0291 kJ/mol C Cp = 0.0358 kJ/mol C Cp=0.0487 kJ/mol C a) Calculate the standard heat of reaction (kJ/mol). (-165.01 kJ/mol) b) If the gases enter and leave the reactor at 1 atm and 500 C, what is the heat of reaction at 500 C (i.e. Ê, at 500 C) in kJ/mol. Assume the reactants are fed in stoichiometric amounts. (-184.63 kJ/mol)

27.- In an adiabatic plug flow reactor the gas phase reaction A + B →R + S is carried out at an absolute pressure of 2 atm. The kinetics of the reaction is given by -ra = kpapB, where k(100°C) = 0.05 and k(500°C) = 50 (both in mol/(L-h- atm?)). The reaction enthalpy can be considered constant in the range of working temperatures with a value of AH = 41.8 kJ/mol A. The reactor is fed with 5 kg/h of an equimolar mixture of A and B at 250°C and a conversion of 35% is desired. Calculate the volume of the reactor needed. Data: Cp reactant mixture = 1.5 cal/(g.°C) MW (assumed constant) 40 g/mole reactant mixture =

The following elementary gas-phase reaction has a rate constant of 20 L⁄mol min at 350 K. A + B → C The reaction is carried out in an isothermal, isobaric PFR at 350 K and 2 atm. The feed is a 30:60:10 mixture of A:B:inert. The feed flow rate of A is 5 mol/min. (a) Determine the PFR volume required to achieve a conversion of 90%. (b) Determine the conversion that could be achieved if the PFR volume were half of the volume calculated in part (a). Give your answer correct to 3 s.f. (c) Present your answers to parts (a) and (b) on a single Levenspiel Plot.

Please help, with some explanation.