Consider the following equilibrium for which H = 16.48: 2 NOBr(g) Y--> 2 NO(g) + Br2(g) How...

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Chemistry

Consider the following equilibrium for which H = 16.48:
2 NOBr(g) Y--> 2 NO(g) + Br2(g)
How will each of the following changes affect an equilibriummixture of the 3 gases in this reaction?
(a) NO is added to the system.
(b) The reaction mixture is heated.
(c) The volume of the reaction vessel is doubled.
(d) A catalyst is added to the reaction mixture.
(e) The total pressure of the system is increased by adding anoble gas.
(f) Br2(g) is removed from the system.

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4.4 Ratings (794 Votes)

Sol Consider the following equilibrium for which 2 NOBrg Y 2 NOg Br2g delta H 1648Endothermic reaction a NO is added to the systemthen equilibrium will shifts towards reactant side because according to LeChateliers principle as the concentration of any one of the product species increases then equilibrium will shift See Answer

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