For the equilibrium Br 2 ( g ) ⇌ 2Br ( g ) Equilibrium partial pressures at 755 K are p Br 2 = 0.668 bar and p Br = 0.226 bar . If the volume of the system is suddenly doubled so that p Br 2 = 0.334 bar and p Br = 0.113 bar , what are the new partial pressures when equilibrium is reestablished? Is this consistent with Le Chatelier’s principle?
For the equilibrium Br 2 ( g ) ⇌ 2Br ( g ) Equilibrium partial pressures at 755 K are p Br 2 = 0.668 bar and p Br = 0.226 bar . If the volume of the system is suddenly doubled so that p Br 2 = 0.334 bar and p Br = 0.113 bar , what are the new partial pressures when equilibrium is reestablished? Is this consistent with Le Chatelier’s principle?
Solution Summary: The author explains that the new partial pressures for the given condition are to be calculated.
Equilibrium partial pressures at
755
K
are
p
Br
2
=
0.668
bar
and
p
Br
=
0.226
bar
. If the volume of the system is suddenly doubled so that
p
Br
2
=
0.334
bar
and
p
Br
=
0.113
bar
, what are the new partial pressures when equilibrium is reestablished? Is this consistent with Le Chatelier’s principle?
When talking about the acidity of carboxylic acids, is it the same thing to say higher or stronger acidity?
Using the following two half-reactions, determine the pH range in which $NO_2^-\ (aq)$ cannot be found as the predominant chemical species in water.* $NO_3^-(aq)+10H^+(aq)+8e^-\rightarrow NH_4^+(aq)+3H_2O(l),\ pE^{\circ}=14.88$* $NO_2^-(aq)+8H^+(aq)+6e^-\rightarrow NH_4^+(aq)+2H_2O(l),\ pE^{\circ}=15.08$
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