consider the following reaction SO2Cl2= SO2+Cl2. A reaction
mixture is made containing an initial [SO2Cl2] of...
consider the following reaction SO2Cl2= SO2+Cl2. A reaction
mixture is made containing an initial [SO2Cl2] of 2.3 x10^-2 M. At
equilibrium, [Cl2]= 1.1x10^-2 M. Calculate the value of the
equilibrium constant (Kc)
1.
Consider the following reaction:
SO2Cl2(g)⇌SO2(g)+Cl2(g)
A reaction mixture is made containing an initial [SO2Cl2] of
2.2×10−2 M . At equilibrium, [Cl2]=1.3×10−2 M
.
Calculate the value of the equilibrium constant
(Kc).
2.
Consider the following reaction:
CO(g)+2H2(g)⇌CH3OH(g)
A reaction mixture in a 5.17-L flask at a certain temperature
initially contains 27.4 g CO and 2.36 g H2. At equilibrium, the
flask contains 8.67 gCH3OH.
Calculate the equilibrium constant (Kc) for the
reaction at this temperature.
3.
Consider the following...
Question 1: Consider the following reaction:
SO2Cl2(g)⇌SO2(g)+Cl2(g)
Kc=2.99×10−7 at 227 ∘C
If a reaction mixture initially contains 0.195 MSO2Cl2,
what is the equilibrium concentration of Cl2at 227 ∘C??
Question 2:
Consider the reaction
CO(g)+H2O(g)⇌CO2(g)+H2(g)
Kc=102 at 500 K
A reaction mixture initially contains 0.130 MCOand
0.130 MH2O.
What will be the equilibrium concentration of H2O?
Question 3:
The following reaction was performed in a sealed vessel at 768
∘C :
H2(g)+I2(g)⇌2HI(g)
Initially, only H2 and I2 were present at concentrations...
Consider the following reaction:
SO2Cl2(g)⇌SO2(g)+Cl2(g)
Kc=2.99×10−7 at 227∘C
Part A
If a reaction mixture initially contains 0.195 M SO2Cl2, what is
the equilibrium concentration of Cl2 at 227 ∘C?
[Cl2] =
Consider the following reaction: SO2Cl2(g)⇌SO2(g)+Cl2(g)
Kc=2.99×10−7 at 227 ∘C If a reaction mixture initially contains
0.159 MSO2Cl2, what is the equilibrium concentration of Cl2 at 227
∘C?
Consider the reaction:
SO2Cl2(g)⇌SO2(g)+Cl2(g)
Kp=2.91×103 at 298 K
In a reaction at equilibrium, the partial pressure of SO2 is 0.135
atm and that of Cl2 is 0.342 atm .
Part A
What is the partial pressure of SO2Cl2 in this mixture?
Consider the following reaction: 2H2S(g)+SO2(g)⇌3S(s)+2H2O(g) A
reaction mixture initially containing 0.500 M H2S and 0.500 M SO2
was found to contain 1.3×10−3 M H2O at a certain temperature. A
second reaction mixture at the same temperature initially contains
[H2S]= 0.255 M and [SO2]= 0.325 M . Calculate the equilibrium
concentration of H2O in the second mixture at this temperature.
1. Given the equilibrium: SO2Cl2(g) SO2(g) + Cl2(g) Kp = 3.60
at 125 °C Is this reaction at equilibrium under the following
conditions. If the reaction is not at equilibrium state which
direction it will go to reach equilibrium. a) PSO2CL2 = 0.568 atm,
PSO2 = 0.125 atm, and PCl2 = 0.500 atm b) PSO2CL2 = 0.125 atm, PSO2
= 0.250 atm, and PCl2 = 1.200 atm c) PSO2CL2 = 0.108 atm, PSO2 =
0.500 atm, and PCl2 =...
Consider the following reaction: Fe3+(aq)+SCN−(aq)⇌FeSCN2+(aq) A
solution is made containing an initial [Fe3+] of 1.2×10−3 M and an
initial [SCN−] of 7.8×10−4 M . At equilibrium, [FeSCN2+]= 1.7×10−4
M .Calculate the value of the equilibrium constant (Kc).
Consider the following reaction:
Fe3+(aq)+SCN−(aq)⇌FeSCN2+(aq)
A solution is made containing an initial [Fe3+] of
1.1×10−3 M and an initial [SCN−] of 8.2×10−4
M. At equilibrium, [FeSCN2+]= 1.8×10−4 M .
Part A
Calculate the value of the equilibrium constant
(Kc).
Express your answer using two significant figures.
Kc=
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).