Question

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]

Homework Answers

Answer #1

K = NO^2*Cl2/(NOCl^2)

initially

NOCl = 0.0435

NO = 0

Cl2 = 0

in equilibrium

NOCl = 0.0435 - 2x

NO = 0 + 2x

Cl2 = 0 + x

then

K = NO^2*Cl2/(NOCl^2)

1.6*10^-4 = (2x)^2*x/(0.0435 - 2x)^2

(0.0435 - 2x)^2 = (4/(1.6*10^-4))*x^3

(0.0435 - 2x)^2 = 25000x^3

0.0435 ^2 + -2*0.0435 x + 4x^2 =  25000x^3

25000x^3 - 4x^2 +0.087x - 0.00189225 = 0

x = 0.004

then

NOCl = 0.0435 - 2*0.004 = 0.0355

NO = 0 + 2*0.004 = 0.008

Cl2 = 0 + 0.004 = 0.004

proof

K = NO^2*Cl2/(NOCl^2) = (0.008^2)(0.004)/(0.0355^2) = 2.0313429*10^-4 which is pretyt near to K

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
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?
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...
If delta H rxn is -75.2 kJ, 2NO(g) + Cl2 (g) <---> 2NOCl(g) A scientist places...
If delta H rxn is -75.2 kJ, 2NO(g) + Cl2 (g) <---> 2NOCl(g) A scientist places four moles of nitrogen monoxide and two moles of chlorine gas into flask A and the same amounts into Flask B, then allows the systems to reach equilibrium. Flask A is at 25 degrees Celsius and Flask B is at 200 degrees Celsius A) In which flask will the reaction occur faster? Explain. B) In which flask will the reaction occur to a greater...
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 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. .
Nitric oxide was reacted with chlorine to produce nitrosyl chloride according to the following equation: 2NO(g)...
Nitric oxide was reacted with chlorine to produce nitrosyl chloride according to the following equation: 2NO(g) + Cl2(g) ?? 2NOCl(g) The rate constant for this reaction at 25oC is 4.9 X 10-6 L/(mol.s) while the rate constant at 150C is 1.5 X 10-5 L/(mol.s). Use this data to calculate the energy of activation for this reaction. 2) What is the rate constant at 150oC for the reaction in question 1? 3) Does the reaction between acetone and iodine follow the...
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 =...
CO(g)+Cl2(g)⇌COCl2(g) Carbon monoxide and chlorine gas are allowed to react in a sealed vessel at 464...
CO(g)+Cl2(g)⇌COCl2(g) Carbon monoxide and chlorine gas are allowed to react in a sealed vessel at 464 ∘C . At equilibrium, the concentrations were measured and the following results obtained: Gas Partial Pressure (atm) CO 0.780 Cl2 1.22 COCl2 0.120 What is the equilibrium constant, Kp, of this reaction? Part B The following reaction was performed in a sealed vessel at 767 ∘C : H2(g)+I2(g)⇌2HI(g) Initially, only H2 and I2 were present at concentrations of [H2]=3.75M and [I2]=2.05M. The equilibrium concentration...