During a study visit to a chemical industry, you learned that the isothermal and isobarically carried out the gas phase reaction A -> R + S is carried out in a tube reactor at 700°C and the pressure 2 atm. The operating engineer was very secretive about the size of the production but mistakenly states that space velocity is 600 h^-1 and that inert components are not included at all the reaction. You yourself estimate the diameter of the reactor to be 1 dm and the length to 20 meters. Using this data, calculate the production per hour of R during continuous operation. From the literature you have found that the reaction is of first order with the rate constant 0.8 s^-1 at 700°C. The molecular weight of R is 32 g/mol. Could the steps in the calculation be explained, why we do it. Would truly appreciate it.
During a study visit to a chemical industry, you learned that the isothermal and isobarically carried out the gas phase reaction A -> R + S is carried out in a tube reactor at 700°C and the pressure 2 atm. The operating engineer was very secretive about the size of the production but mistakenly states that space velocity is 600 h^-1 and that inert components are not included at all the reaction. You yourself estimate the diameter of the reactor to be 1 dm and the length to 20 meters. Using this data, calculate the production per hour of R during continuous operation. From the literature you have found that the reaction is of first order with the rate constant 0.8 s^-1 at 700°C. The molecular weight of R is 32 g/mol.
Could the steps in the calculation be explained, why we do it. Would truly appreciate it.
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Im sorry but how did u solve the equation for turnover?
4.8 = 2ln(1-x)-x isnt solvable
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