Consider the following equilibrium:
2NOCl(g) ⇌ 2 NO(g) + Cl2(g) Kc = 1.6 x 10-5
1.00 mole of pure NOCl and 1.00 mole of pure Cl2 are placed in a 1.00 L container. Calculate the equilibrium concentration of NO(g)
concentration of NOCl [NOCl] = no of moles/volume in L
= 1/1 = 1M
concentration of Cl2 [Cl2] = no of moles/volume in L
= 1/1 = 1M
2NOCl(g) ⇌ 2 NO(g) + Cl2(g)
I 1 0 0
C -2x 2x x
E 1-2x 2x x
Kc = [NO]^2[Cl2]/[NOCl]^2
1.6*10^-5 = (2x)^2*x/(1-2x)^2
1.6*10^-5 *(1-2x)^2 = 4x^3
x = 0.01554
[NO] = 2x = 2*0.01554 = 0.03108M >>>>answer
Consider the following equilibrium: 2NOCl(g) ⇌ 2 NO(g) + Cl2(g) Kc = 1.6 x 10-5 1.00...
At some temperature, the Kc for the reaction 2NOCl(g) ⇌ 2NO(g) + Cl2(g) is 1.6 x 10^-5. Calculate the concentrations of all species at equilibrium if 1.0 moles of pure NOCl is initially placed in a 2.0 L flask
22. Consider the following equilibrium: 2NOCI(8) = 210g)+Ch ) with K = 1.6 x 10-5 1.00 mole of pure NACI and 9.40 x 10-1 mole of pure Cl2 are placed in a 1.00-L container. Calculate the equilibrium concentration of Cl2(g). A) 1.6 x 10-SM B) 9.4 x 10-M C) 4.7 x 10-1 M D) 2.1 x 10-3M E) 4.1 x 10-3M
At 500.0 K, gaseous NOCl decomposed to NO and Cl2 according the
following reaction:
2NOCl(g) ⇌ 2NO(g) + Cl2(g)
If 1.00 mole of NOCl is placed in a 1.00 liter contained, and at
equilibrium, the
concentration is 0.91M, what is the equilibrium constant,
Kc?
4. At 500.0 K, gaseous NOCI decomposed to NO and Cl2 according the following reaction: 2NOCI(g) = 2NO(g) + Cl2(g) If 1.00 mole of NOCI is placed in a 1.00 liter contained, and at equilibrium, the...
Consider the slowing equilibrium: 2NOC(g) =2NO(g) + Cl2(g) with K = 1.6 x 10 Segiment 100 mole of pure NOCI and 1.00 mole of pure Cly are placed in 100.container Reference: Ref 13-6 Tundles of NO react, what is the equilibrium concentration of Cl2? 01-2
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]= 0.65 M and [Cl2]= 0.64 M. After the reaction comes to equilibrium, the concentration of NOCl is 0.1 M. Find the value of the equilibrium constant (Kc) at this temperature.
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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]= 0.67 M and [Cl2]= 0.65. After the reaction comes to equilibrium, the concentration of NOCl is 0.15 M. Find the value of the equilibrium constant (Kc) at this temperature. Express your answer using two significant figures.
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The following reaction has an equilibrium constant, Kc, of 1.80 x 10-4 at a particular temperature: 2NOCl (g) → 2 NO (g) + Cl2 (g) You have a container in which the concentration of HOCl is 0.99 M, the concentration of NO is 0.45 M, and the concentration of Cl2 is 0.67 M. (a) Calculate the value of the reaction quotient Q. (b) Is the system at equilibrium? If not, predict which way (right or left) the reaction will proceed...