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19.09.2019 • 

Chemistry

Acetylene is hydrogenated to form ethane. the feed to the reactor contains 1.50 mol h2/mol c2h2. (a) calculate the stoichiometric reactant ratio (mol h2 react/mol c2h2 react) and the yield ratio (kmol c2h6 formed/kmol h2 react). (b) determine the limiting reactant and calculate the percentage by which the other reactant is in excess. (c) calculate the mass feed rate of hydrogen (kg/s) required to produce 4 106 metric tons of ethane per year, assuming that the reaction goes to completion and that the process operates for 24 hours a day, 300 days a year. (d) there is a definite drawback to running with one reactant in excess rather than feeding the reactants in stoichiometric proportion. what is it? [hint: in the process of part (c), what does the reactor effluent consist of and what will probably have to be done before the product ethane can be sold or used? ]

Ответ:

beetle1234

09.05.2022

Chemistry

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 Best   We would write the molecular equation as  
BaCl2(s) + H2SO4(aq) --> BaSO4(s) + 2HCl(aq) 

You would write the ionic equation as 
BaCl2(s) + H+ + HSO4^- --> BaSO4(s) + 2H+ + 2Cl- 

remove the H+ from both sides and write the net ionic equation as 
BaCl2(s) + HSO4^- --> BaSO4(s) + H+ + 2Cl- 

If you placed BaCl2 solid in sulfuric acid it would quickly acquire a coating of insoluble BaSO4 which will prevent the further reaction of the barium chloride. 

The same is true if you took a block of BaCl2 and placed a drop of H2SO4 solution on it. The solid BaSO4 that forms will block further reaction. You would get HCl gas only if the small amount of solution became saturated in HCl.

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