Question

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

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
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. .
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...
NO reacts with Cl2 to form NOCl. The equilibrium constant, Kp, for this reaction is 5.56...
NO reacts with Cl2 to form NOCl. The equilibrium constant, Kp, for this reaction is 5.56 at 573 K. 2NO(g) + Cl2(g) 2NOCl(g) The standard enthalpy change for this reaction (ΔH°) is -77.1 kJ/mol. (a) Predict the effect on the production of NOCl when the temperature of the equilibrium system is decreased. *production is favored or production is disfavored (b) Use the van’t Hoff equation to estimate the equilibrium constant for this reaction at 488 K. Kp at 488 K...
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=???
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 =...
At 473 K, for the elementary reaction 2NOCl(g)k1⇌k−12NO(g)+Cl2(g) k1=7.8×10−2L/mols and k−1=4.7×102L2/mol2s A sample of NOCl is...
At 473 K, for the elementary reaction 2NOCl(g)k1⇌k−12NO(g)+Cl2(g) k1=7.8×10−2L/mols and k−1=4.7×102L2/mol2s A sample of NOCl is placed in a container and heated to 473 K. When the system comes to equilibrium, [NOCl] is found to be 0.60 mol/L . Find the concentration of NO. Find the concentration of Cl2.
the decomposition of NOCL,2NOCl 2NO+Cl2 has k=9.3*10^-5 L mol^-1 s^-1 at 100C and k=1.0*10^-3 mol^-1s^-1 at...
the decomposition of NOCL,2NOCl 2NO+Cl2 has k=9.3*10^-5 L mol^-1 s^-1 at 100C and k=1.0*10^-3 mol^-1s^-1 at 130C..what is Ea for reaction in kJ mol^-1
The equilibrium constant, Kc, for the formation of nitrosyl chloride from nitric oxide and chlorine. 2NO(g)...
The equilibrium constant, Kc, for the formation of nitrosyl chloride from nitric oxide and chlorine. 2NO(g) + Cl2(g) ⇌ 2NOCl(g) is 6.5 ×10^4 at 35°C. In which direction will the reaction proceed to reach equilibrium if the starting concentrations of NO, Cl2, and NOCl are 6.8 ×10^−3 M, 7.5 ×10^−4 M, and 7.4 M respectively?
The equilibrium constant, Kc, for the formation of nitrosyl chloride from nitric oxide and chlorine. 2NO(g)...
The equilibrium constant, Kc, for the formation of nitrosyl chloride from nitric oxide and chlorine. 2NO(g) + Cl2(g) ⇌ 2NOCl(g) is 6.5 ×104 at 35°C. In which direction will the reaction proceed to reach equilibrium if the starting concentrations of NO, Cl2, and NOCl are 5.2 × 10−3M, 3.4 × 10−4M, and 3.4 M respectively?
Pure NOCl gas was heated at 240°C in a 1.00−L container. At equilibrium the total pressure...
Pure NOCl gas was heated at 240°C in a 1.00−L container. At equilibrium the total pressure was 1.00 atm and the NOCl pressure was 0.64 atm. 2NOCl(g) ⇆ 2NO(g) + Cl2(g) (a) Calculate the partial pressure of NO and Cl2 in the system. b) Calculate the equilibrium constant KP.
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT