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 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).
1. Consider a reaction mixture containing 100.0 mL of 0.112 M
borate buffer at pH = pKa = 9.24. At pH = pKa, we know that [H3BO3]
= [H2BO3−] = 0.0560 M. Suppose that a chemical reaction whose pH we
wish to control will be generating acid. To avoid changing the pH
very much we do not want to generate more acid than would use up
half of the [H2BO3−].
a)How many moles of acid could be generated without using...