2 NO (g) equilibrium arrow N2 (g) + O2 (g) Initially, 0.75 M NO is placed...

Question

Question

2 NO (g) equilibrium arrow N2 (g) + O2 (g) Initially, 0.75 M NO is placed...

2 NO (g) equilibrium arrow N2 (g) + O2 (g)

Initially, 0.75 M NO is placed in a reaction vessel and the reaction is allowed to reach equilibrium. If the equilibrium constant for this reaction is 0.463, what is the equilibrium concentration of NO?

science chemistry

Add a comment Improve this question Transcribed image text

Answer 1

Answer #1

The reaction is 2NO(g)<-----------> N2 (g) + O2 (g)

Initially NO= 0.75

let x= concenttration of N2 at equilibrium

hence at equilibrium

[N2] =[O2] =x and [NO] =0.75-2x

Equilibrium constant = [N2] [O2]/[NO]² = 0.463

x²/(0.75-2x)²= 0.463

taking square toor on both sides give

x/(0.75-2x)= 0.68

x= 0.68*(0.75-2x)

x*(1+2*0.68)= 0.68*0.75

2.36x= 0.68*0.75

x= 0.216

At equilibrium [NO] =0.75-2*0.216= 0.75-0.432= 0.318M

Add a comment

Answer 2

Similar Homework Help Questions

Nitrogen and oxygen react at high temperatures. N2(g) + O2(g) equilibrium reaction arrow 2 NO(g) ΔH...

Nitrogen and oxygen react at high temperatures. N2(g) + O2(g) equilibrium reaction arrow 2 NO(g) ΔH = 182.6 kJ (a) Write the expression for the equilibrium constant (Kc) for this reversible reaction. (Concentration equilibrium expressions take the general form: Kc = [C]c / [A]a . [B]b. Subscripts and superscripts that include letters must be enclosed in braces {}.)
For the first-order reaction, 2 N2O(g) ? 2 N2(g) + O2(g), what is the concentration of...

For the first-order reaction, 2 N2O(g) ? 2 N2(g) + O2(g), what is the concentration of N2O after 3 half-lives if 0.15 mol of N2O is initially placed into in a 1.00-L reaction vessel?
N2(g) + O2(g) equilibrium reaction arrow 2 NO(g); Kc = 5.6 ✕ 10−4 at 2098 K...

N2(g) + O2(g) equilibrium reaction arrow 2 NO(g); Kc = 5.6 ✕ 10−4 at 2098 K (a) What is the value of Kc for the reaction 2 NO(g) equilibrium reaction arrow N2(g) + O2(g) at the same temperature? (b) What is the value of Kc for the reaction 1/2 N2(g) + 1/2 O2(g) equilibrium reaction arrow NO(g) at the same temperature? (c) Does the equilibrium in (a) favor the reactant or the products? reactant products (d) Does the equilibrium in...

Consider the following equilibrium reaction : Heat + 2 SO2 (g) + O2(g) ↔ 2 SO3(g) Assume the above...

Consider the following equilibrium reaction : Heat + 2 SO2 (g) + O2(g) ↔ 2 SO3(g) Assume the above reaction is allowed to reach equilibrium prior to the following changes. Answer the following questions by writing increase, decrease or remain the same on the line. **please also explain why** If the reaction mixture is heated up , the value of the equilibrium constant will _______________________ If SO2 (g) is added to the reaction vessel the concentration of O2(g) will____________________________. If SO3 (g) is...
For the following reaction, 0.500 M of COCl2 is placed in a reaction vessel. Calculate the...

For the following reaction, 0.500 M of COCl2 is placed in a reaction vessel. Calculate the equilibrium concentrations of all gases at equilibrium. COCl2(g) 2 CO(g) + Cl2(g) Kc = 1.70 x 10-4 4 NH3(g) + 3 O2(g) = 2 N2(g) + 6 H2O(g) When 0.256 g of NH3 and 0.480 g if O2 are initially placed in a 1.00 L container at a certain temperature, the N2 concentration at equilibrium is 1.96 x 10 M. Calculate K, for the...
4. The equilibrium constant for the reaction is 2.60 x 10-7 at 300 °C. 2 NO2(g)...

4. The equilibrium constant for the reaction is 2.60 x 10-7 at 300 °C. 2 NO2(g) = 2 02(g) + N2(g) If 0.250 mol of NO, gas is placed in 5.00 L vessel and allowed to reach equilibrium at this temperature, calculate the equilibrium concentrations of the nitrogen gas and oxygen gas. (Ignoring X Method) s. For the following reaction: 2 NH3(g) = 3 H2(g) + N2(g) When 1.2 mol of hydrogen gas and 0.40 mol of nitrogen gas are...

At equilibrium, the concentrations in this system were found to be [N2]=[O2]=0.300 M[N2]=[O2]=0.300 M and [NO]=0.400...

At equilibrium, the concentrations in this system were found to be [N2]=[O2]=0.300 M[N2]=[O2]=0.300 M and [NO]=0.400 M.[NO]=0.400 M. N2(g)+O2(g)−⇀↽−2NO(g)N2(g)+O2(g)↽−−⇀2NO(g) If more NONO is added, bringing its concentration to 0.700 M,0.700 M, what will the final concentration of NONO be after equilibrium is re‑established?
At equilibrium, the concentrations in this system were found to be [N2]=[O2]=0.100 M[N2]=[O2]=0.100 M and [NO]=0.600...

At equilibrium, the concentrations in this system were found to be [N2]=[O2]=0.100 M[N2]=[O2]=0.100 M and [NO]=0.600 M.[NO]=0.600 M. N2(g)+O2(g)−⇀↽−2NO(g)N2(g)+O2(g)↽−−⇀2NO(g) If more NONO is added, bringing its concentration to 0.900 M,0.900 M, what will the final concentration of NONO be after equilibrium is re‑established? [NO]final=
At 4124 oC the equilibrium constant for the reaction: 2 NO(g) N2(g) + O2(g) is KP...

At 4124 oC the equilibrium constant for the reaction: 2 NO(g) N2(g) + O2(g) is KP = 7.16. If the initial pressure of NO is 0.00663 atm, what are the equilibrium partial pressures of NO, N2, and O2? p(NO) = . p(N2) = . p(O2) = .

Initially 0.80 atm of N2 and 1.68 atm of Bra are placed into an evacuated reaction...

Initially 0.80 atm of N2 and 1.68 atm of Bra are placed into an evacuated reaction vessel. When equilibrium is established, there are 1.42 atm of Brz remaining in the vessel. What is Kp for this reaction? 2 NBr; (g) = N2 (g) + 3 Brz (g) A) 5.8 B) 19 C) 26 D) 67

2 NO (g) equilibrium arrow N2 (g) + O2 (g) Initially, 0.75 M NO is placed...

Homework Answers

Add Answer to:
2 NO (g) equilibrium arrow N2 (g) + O2 (g) Initially, 0.75 M NO is placed...

Post as a guest

Earn Coins

Nitrogen and oxygen react at high temperatures. N2(g) + O2(g) equilibrium reaction arrow 2 NO(g) ΔH...

For the first-order reaction, 2 N2O(g) ? 2 N2(g) + O2(g), what is the concentration of...

N2(g) + O2(g) equilibrium reaction arrow 2 NO(g); Kc = 5.6 ✕ 10−4 at 2098 K...

Consider the following equilibrium reaction : Heat + 2 SO2 (g) + O2(g) ↔ 2 SO3(g) Assume the above...

For the following reaction, 0.500 M of COCl2 is placed in a reaction vessel. Calculate the...

4. The equilibrium constant for the reaction is 2.60 x 10-7 at 300 °C. 2 NO2(g)...

At equilibrium, the concentrations in this system were found to be [N2]=[O2]=0.300 M[N2]=[O2]=0.300 M and [NO]=0.400...

At equilibrium, the concentrations in this system were found to be [N2]=[O2]=0.100 M[N2]=[O2]=0.100 M and [NO]=0.600...

At 4124 oC the equilibrium constant for the reaction: 2 NO(g) N2(g) + O2(g) is KP...

Initially 0.80 atm of N2 and 1.68 atm of Bra are placed into an evacuated reaction...

2 NO (g) equilibrium arrow N2 (g) + O2 (g) Initially, 0.75 M NO is placed...

Homework Answers

Add Answer to: 2 NO (g) equilibrium arrow N2 (g) + O2 (g) Initially, 0.75 M NO is placed...

Post as a guest

Earn Coins

Add Answer to:
2 NO (g) equilibrium arrow N2 (g) + O2 (g) Initially, 0.75 M NO is placed...