Question

In: Chemistry

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)

Solutions

Expert Solution

                SO2Cl2-------------> SO2 +     Cl2

I               2.3*10^-2                 0                 0

C            -1.1*10^-2               1.1*10^-2      1.1*10^-2

E             1.2*10^-2               1.1*10^-2        1.1*10^-2

        Kc   = [SO2][Cl2]/[SO2Cl2]

               = 1.1*10^-2 *1.1*10^-2/1.2*10^-2

               = 0.01>>>>>answer


Related Solutions

1. Consider the following reaction: SO2Cl2(g)⇌SO2(g)+Cl2(g) A reaction mixture is made containing an initial [SO2Cl2] of...
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...
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...
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...
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...
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...
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...
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...
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...
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...
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).
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT