Question
In: Chemistry
Consider this reaction between solid carbon and carbon dioxide gas. C(s) + CO2(g) ⇌ 2 CO(g);...
Consider this reaction between solid carbon and carbon dioxide gas. C(s) + CO2(g) ⇌ 2 CO(g); ΔH = +172.5 kJ/mol Please explain the following: When chemical systems are subjected to stresses, the equilibrium position may shift toward the reactants or products, or it may be unaffected. How would each of the following changes affect this equilibrium? 1. decreasing the temp 2. increasing the CO2 3. increasing the volume of the container 4. adding C 5. adding a catlyst Options: Would #'s 1-5... a. shift the reaction towards the reactants, shift the reaction towards the products, or would the change not have any effect on the reaction at all?
Solutions
queen_honey_blossom answered 2 years agoRelated Solutions
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Coke can be converted into CO in following reaction CO2(g) + C(s) -> 2CO(g). A coke...
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carbon by mass and the balance noncombustible ash is fed to a
reactor with a stoichiometric amount of CO2. The coke is
fed at 77 oF, and the CO2 enters at 400 oF. Heat is
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Coke can be converted into CO in following reaction CO2(g) + C(s) -> 2CO(g). A coke...
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C(s) -> 2CO(g). A coke that contains 84% carbon by mass and the
balance noncombustible ash is fed to a reactor with a
stoichiometric amount of CO2. The coke is fed at 77 oF, and the CO2
enters at 400 oF. Heat is transferred to the reactor in the amount
of 5200 btu/lbm coke fed. The gaseous products and the solid
reactor effluent (the ash and unburned carbon) leave...
Consider the reaction: NO2 (g) + CO (g) ---> CO2 (g) + NO (g) The equilibrium...
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to come to equilibrium, what is the equilibrium concentration of
carbon dioxide?
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