Question
In: Chemistry
2 NO(g) + Cl2(g) ⇄ 2 NOCl(g) Kp = 1.40 × 10^8 A reaction vessel initially...
2 NO(g) + Cl2(g) ⇄ 2 NOCl(g) Kp = 1.40 × 10^8 A reaction vessel initially contains 3.0 atm of NO and 2.0 atm of Cl2. What is the pressure of Cl2(g) when equilibrium is reached?
Solutions
Expert Solution
2 NO(g) + Cl2(g) ⇄ 2 NOCl(g)
I 3 2 0
C -2x -x 2x
E 3-2x 2-x 2x
Kp = P^2NOCl/P^2NOPCl2
1.4*10^8 = (2x)^2/(3-2x)^2(2-x)
1.4*10^8 *(3-2x)^2*(2-x) = 4x^2
x = 1.499
PNO = 3-2x = 3-2*1.499 = 0.002atm
PCl2 = 2-x = 2-1.499 = 0.501atm >>>>answer
PNOCl = 2x = 2*1.499 = 3atm
queen_honey_blossom answered 2 years agoRelated Solutions
2 NO(g) + Cl2(g) ⇄ 2 NOCl(g) Kp = 1.40 × 10^8 A reaction vessel initially...
2 NO(g) + Cl2(g) ⇄ 2 NOCl(g) Kp = 1.40 × 10^8 A reaction
vessel initially contains 3.0 atm of NO and 2.0 atm of Cl2. What is
the pressure of Cl2(g) when equilibrium is reached?
For the reaction Br2 (g) + Cl2 (g) → 2 BrCl Kp = 1.11 x 10-4...
For the reaction Br2 (g) + Cl2 (g) → 2
BrCl Kp = 1.11 x 10-4 at 150K.
a) If 1.0 atm each of bromine and chlorine gas are placed in an
otherwise empty 1 L container and allowed to equilibrate at a
temperature of 150K, what will be the partial pressures at
equilibrium of all three gases?
Br2 atm
Cl2 atm
BrCl atm
b) suppose 0.2 atm each of all three gases are placed in a selaed
container and allowed to equilibrate...
2 NO(g) + Cl2(g) --> 2 NOCl (g) Two proposed mechanisms for the reaction are given...
2 NO(g) + Cl2(g) --> 2 NOCl (g)
Two proposed mechanisms for the reaction are given below. Which
is the better mechanism? Explain both why the better mechanism is
better and why the worse mechanism is worse.
Mechanism
1
Mechanism 2
NO + Cl2 --> NOCl +
Cl
Cl2 --> Cl + Cl
NO + Cl --> NOCl NO + Cl --> NOCl
NO + Cl2 --> NOCl + Cl
For the correct mechanism, identify:...
1. Consider the following reaction: Br2(g)+Cl2(g)⇌2BrCl(g) Kp=1.11×10−4 at 150 K. A reaction mixture initially contains a...
1. Consider the following reaction:
Br2(g)+Cl2(g)⇌2BrCl(g) Kp=1.11×10−4 at 150 K. A reaction mixture
initially contains a Br2 partial pressure of 750. torr and a Cl2
partial pressure of 735 torr at 150 K.
Calculate the equilibrium partial pressure of BrCl in
atm and torr. (State any assumptions).
1) At a certain temperature, 322 K, Kp for the reaction, Cl2(g) <=> 2 Cl(g), is...
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
The equilibrium constant, Kp, for the following reaction is 2.01 at 500 K: PCl3(g) + Cl2(g)...
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)...
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)...
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
Consider the following reaction: I2(g)+Cl2(g)⇌2ICl(g) Kp= 81.9 at 25 ∘C. Calculate ΔGrxn for the reaction at...
Consider the following reaction:
I2(g)+Cl2(g)⇌2ICl(g)
Kp= 81.9 at 25 ∘C.
Calculate ΔGrxn for the reaction at 25 ∘C under each of
the following conditions.
PICl= 2.65 atm ;
PI2= 0.325 atm ;
PCl2= 0.212 atm .
2 NOCl(g) <=> 2 NO(g) + Cl2(g), K= 1.6E-5. Calculate the concentrations when: a). 6.0 mol...
2 NOCl(g) <=> 2 NO(g) + Cl2(g), K= 1.6E-5. Calculate the
concentrations when:
a). 6.0 mol of NO and 2.0 mol of Cl2 in a 1.2-L flask
b). 2.2 mol of NOCl, 2.2 mol of NO, and 1.1 mol of
Cl2 in a 1.0-L flask
c). 1.01 mol/L concentration of all three gases
Please show work and don't just solve the top problem. I need
all three and I don't know how to correctly solve either of
them!!
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