1) At a certain temperature, 322 K, Kp for the
reaction,
Cl2(g) <=> 2 Cl(g), is 7.82 x
10-60.
Calculate the value of ΔGo in kJ for the reaction at
this temperature.
2)
The equilibrium constant for the reaction,
2 Fe3+(aq) + Hg22+(aq)
<=> 2 Fe2+(aq) + 2 Hg2+(aq)
is 9.1 x 10-6(aq) at 298 K. Calculate ΔG in J when
{Fe3+(aq)} = 0.375
{Hg22+(aq)} = 0.051
{Fe2+(aq)} = 0.021
{Hg2+(aq)} = 0.06
Consider the following reaction: CO(g)+2H2(g)⇌CH3OH(g)
Kp=2.26×104 at 25 ∘C. Calculate ΔGrxn for the reaction at 25 ∘C
under each of the following conditions. - standard conditions - at
equilibrium - PCH3OH= 1.4 atm ; PCO=PH2= 1.5×10−2 atm
Consider the following reaction:
CO(g)+2H2(g)⇌CH3OH(g)
Kp=2.26×104 at 25 ∘C. Calculate ΔGrxn for the
reaction at 25 ∘C under each of the following conditions.
A) Standard conditions
B) At equilibrium
C) PCH3OH= 1.5 atm ;
PCO=PH2= 1.5×10−2 atm
The following reaction N2 (g) + O2 (g) ⇔ 2 NO (g) has a KP =
0.032 at a particular temperature. At that temperature, a vessel is
filled with 0.040 atm of N2 (g), 0.040 atm of O2 (g) and 0.043 atm
of NO (g). What is the pressure of NO (g) at equilibrium?
The equilibrium constant, Kp, for the following
reaction is 2.01 at 500 K:
PCl3(g) +
Cl2(g)
<----->PCl5(g)
Calculate the equilibrium partial pressures of all species when
PCl3 and
Cl2, each at an intitial partial
pressure of 1.56 atm, are introduced into an
evacuated vessel at 500 K.
PPCl3
=
atm
PCl2
=
atm
PPCl5
=
atm
The equilibrium constant, Kp, for the following reaction is 1.57
at 600 K:
CO(g) + Cl2(g) COCl2(g)
Calculate the equilibrium partial pressures of all species when
CO and Cl2, each at an intitial partial pressure of 1.65 atm, are
introduced into an evacuated vessel at 600 K.
PCO = ______ atm
PCl2= _______ atm
PCOCl2 = _______ atm
The equilibrium constant, Kp, for the following
reaction is 2.01 at 500 K:
PCl3(g) +
Cl2(g)
<<<----->>PCl5(g)
Calculate the equilibrium partial pressures of all species when
PCl3 and
Cl2, each at an intitial partial
pressure of 1.01 atm, are introduced into an
evacuated vessel at 500 K.
PPCl3
=
atm
PCl2
=
atm
PPCl5
=
atm
The equilibrium constant (Kp) for the following reaction is 4.40
at 2000.K.
H2(g) + CO2(g) <=>
H2O(g) + CO(g)
a) Calculate Delta Go for the reaction. ____________
KJ/mol
b) Calculate Delta G for the reaction when the partial pressures
are PH2 = 0.28 atm, PCO2 = 0.81 atm,
PH2O = 0.63 atm, and PCO = 1.17 atm.
______________ KJ/mol
Consider the following reaction where Kp = 1.57 at 600 K: CO(g)
+ Cl2(g) COCl2(g) If the three gases are mixed in a rigid container
at 600 K so that the partial pressure of each gas is initially one
atm, what will happen?
Indicate True (T) or False (F) for each of the following:
1. A reaction will occur in which COCl2(g) is produced
2. Kp will decrease.
3. A reaction will occur in which CO is produced.
4. Q...
1. The equilibrium constant, Kp, for the following
reaction is 10.5 at 350 K:
2CH2Cl2(g)
<--->CH4(g) +
CCl4(g)
Calculate the equilibrium partial pressures of all species when
CH2Cl2(g) is introduced into
an evacuated flask at a pressure of 0.865 atm at
350 K.
PCH2Cl2
=____
atm
PCH4
=____
atm
PCCl4
=____
atm
2. The equilibrium constant, Kp, for the following
reaction is 0.215 at 673 K:
NH4I(s) <---->
NH3(g) + HI(g)
Calculate the equilibrium partial pressure of HI
when 0.413...