Consider the following equilibrium for which H = 664.38:
N2(g) + 2 H2O(g) 2 NO(g) + 2 H2(g)
How will each of the following changes affect an equilibrium mixture of the 4 gases in this reaction?
(a) NO(g) is added to the system.
(b) The reaction mixture is heated.
(c) The volume of the reaction vessel is reduced by 50%.
(d) A catalyst is added to the reaction mixture.
(e) The total pressure of the system is increased by adding a noble gas.
(f) H2O(g) is removed from the system.
The answer choice options for each are:
The equilibrium will not shift
The equilibrium will shift towards product but Keq will not change,
The equilibrium will shift towards reactant but Keq will not change
The equilibrium will shift towards product and Keq will increase
The equilibrium will shift towards reactant and Keq will decrease
Consider the following equilibrium for which H = 664.38: N2(g) + 2 H2O(g) 2 NO(g) +...
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