Question

The equilibrium 2NO(g)+Cl2(g)⇌2NOCl(g) is established at 500 K. An equilibrium mixture of the three gases has...

The equilibrium
2NO(g)+Cl2(g)⇌2NOCl(g)
is established at 500 K. An equilibrium mixture of the three gases has partial pressures of 9.50×10−2 atm , 0.174 atm , and 0.27 atm for NO, Cl2, and NOCl, respectively.

Part A

Calculate Kp for this reaction at 500.0 K.

Express your answer using two significant figures.

Part B

If the vessel has a volume of 5.80 L, calculate Kc at this temperature.

Express your answer using two significant figures.

.

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Consider the reaction between NO and Cl2 to form NOCl: 2NO(g)+Cl2(g)⇌2NOCl(g) A reaction mixture at a...
Consider the reaction between NO and Cl2 to form NOCl: 2NO(g)+Cl2(g)⇌2NOCl(g) A reaction mixture at a certain temperature initially contains only [NO]= 0.50 M and [Cl2]= 0.55. After the reaction comes to equilibrium, the concentration of NOCl is 0.35 M . Part A Find the value of the equilibrium constant (Kc) at this temperature. Express your answer using two significant figures. Kc=???
The reaction 2NOCl(g) 2NO(g) + Cl2(g) has an equilibrium constant Kp (in terms of pressures) at...
The reaction 2NOCl(g) 2NO(g) + Cl2(g) has an equilibrium constant Kp (in terms of pressures) at 300 °C of 0.180. Calculate the concentration of NO that will be present at 300 °C in equilibrium with NOCl (at a concentration of 1.89×10-2 mol L-1) and Cl2 (at a concentration of 7.00×10-3 mol L-1). [NO] =    mol L-1
1. For the reaction: 2NOCl(g) 2NO(g) + Cl2(g), Kc = 1.6 x 10− 5 . What...
1. For the reaction: 2NOCl(g) 2NO(g) + Cl2(g), Kc = 1.6 x 10− 5 . What are the equilibrium concentrations of each species if 1.0 mole of NOCl is initially placed in an empty 2.0 L flask? 2. A reaction vessel is charged with hydrogen iodide, which partially decomposes to molecular hydrogen and iodine: 2HI (g) H2(g) + I2(g): When the system comes to equilibrium at 425 °C, PHI = 0.708 atm and 2 2 P P H I =...
1)A reaction vessel at 27 ∘C contains a mixture of SO2(P= 3.10 atm ) and O2(P=...
1)A reaction vessel at 27 ∘C contains a mixture of SO2(P= 3.10 atm ) and O2(P= 1.00 atm ). When a catalyst is added the reaction 2SO2(g)+O2(g)⇌2SO3(g) takes place. At equilibrium the total pressure is 3.85 atm. -Find the value of Kc. 2)A sample of SO3 is introduced into an evacuated sealed container and heated to 600 K. The following equilibrium is established: 2SO3(g)⇌2SO2(g)+O2(g). The total pressure in the system is found to be 3.0 atm and the mole fraction...
The decomposition of NOCl: 2NOCl (g) <---> Cl2 (g) + 2NO (g) has an equilibrium constant...
The decomposition of NOCl: 2NOCl (g) <---> Cl2 (g) + 2NO (g) has an equilibrium constant of K=1.6*10^-5 at 35 degrees C. if the initial concentration of NOCl is 0.500M, what is the equilibrium concentration of NO? A. 1.00*10^-4M B. 2.00*10^-2M C. 1.00*10^-2M D. 2.3*10^-3M When sodium is added to the reaction vessel, it scavenges the chlorine gas in an exothermic reaction. What will the impact of adding sodium be on the equilibrium of the decomposition of NOCl? A. Shifts...
Nitrosyl chloride decompeses to nitrogen monoxide and chlorine gas 2NOCL (g) <--> 2NO (g) + Cl2(g)...
Nitrosyl chloride decompeses to nitrogen monoxide and chlorine gas 2NOCL (g) <--> 2NO (g) + Cl2(g) K= 1.6 x10-4 0.0435M nitrosyl chloride is allowed to come to equilibrium. Find the equilibrium concentrations of all three species: [NOCl], [NO], [Cl2]
At 100 ∘C, Kc=0.078 for the reaction SO2Cl2(g)←−→SO2(g)+Cl2(g) In an equilibrium mixture of three gases, the...
At 100 ∘C, Kc=0.078 for the reaction SO2Cl2(g)←−→SO2(g)+Cl2(g) In an equilibrium mixture of three gases, the concentrations of SO2Cl2 2 and SO2 are 0.130 M and 0.125 M respectively. Part A What is the partial pressure of Cl2 in the equilibrium mixture? Express your answer using two significant figures.
For the following reaction, Kc = 255 at 1000 K. CO (g) + Cl2 (g) ⇌...
For the following reaction, Kc = 255 at 1000 K. CO (g) + Cl2 (g) ⇌ COCl2 (g) A reaction mixture initially contains a CO concentration of 0.1530 M and a Cl2 concentration of 0.176 M at 1000 K. Part A What is the equilibrium concentration of CO at 1000 K? Express your answer in molarity to three significant figures. Part B What is the equilibrium concentration of Cl2 at 1000 K? Express your answer in molarity to three significant...
1) The equilibrium constant, Kp, for the following reaction is 0.497 at 500 K: PCl5(g) <---...
1) The equilibrium constant, Kp, for the following reaction is 0.497 at 500 K: PCl5(g) <--- ----->PCl3(g) + Cl2(g) (reversible) Calculate the equilibrium partial pressures of all species when PCl5(g) is introduced into an evacuated flask at a pressure of 1.52 atm at 500 K.   PPCl5 = _____atm PPCl3 = ______atm PCl2 = ______atm 2) The equilibrium constant, Kp, for the following reaction is 55.6 at 698 K: H2(g) + I2(g) <----- ----> 2HI(g) (reversible) Calculate the equilibrium partial pressures...
Problem 15.52 For the equilibrium Br2(g)+Cl2(g)⇌2BrCl(g) at 400 K, Kc = 7.0. Part A If 0.25...
Problem 15.52 For the equilibrium Br2(g)+Cl2(g)⇌2BrCl(g) at 400 K, Kc = 7.0. Part A If 0.25 mol of Br2 and 0.55 mol of Cl2 are introduced into a 3.0-L container at 400 K, what will be the equilibrium concentration of Br2? Express your answer to two significant figures and include the appropriate units. SubmitMy AnswersGive Up Part B If 0.25 mol of Br2 and 0.55 mol of Cl2 are introduced into a 3.0-L container at 400 K, what will be...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT