Question

At 2000°C the equilibrium constant for the reaction is Kc = 2.4 103. 2 NO(g) N2(g)...

At 2000°C the equilibrium constant for the reaction is Kc = 2.4 103. 2 NO(g) N2(g) + O2(g) If the initial concentration of NO is 0.120 M, what are the equilibrium concentrations of NO, N2, and O2?

[O2]__?_____ M

[N2]____?___ M

[NO]___?____ M

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
At 2000 ?C the equilibrium constant for the reaction 2NO(g)???N2(g)+O2(g) is Kc=2.4
At 2000 ?C the equilibrium constant for the reaction 2NO(g)???N2(g)+O2(g) is Kc=2.4
At 2000 degrees celcius, the gas-phase equilibrium 2NO(g)=N2(g)+o2(g) has an equilibrium constant of Kc=2.4X10^3. Use this...
At 2000 degrees celcius, the gas-phase equilibrium 2NO(g)=N2(g)+o2(g) has an equilibrium constant of Kc=2.4X10^3. Use this information to answer the following. a) Determine the relationship between Kc and Kp for this equilibrium. What is the value of Kp? b) Determine the value of Kc for the reaction 1/2N2(g)+1/2O2(g)=NO(g). c) Determine the equilibrium concentrations of NO, N2, O2 when 0.200 mol NO(g) is placed into a (n evacuated) 1.000 L container and heated to 2000 degrees celcius.
The equilibrium constant Kc for the reaction below is 6.16 ✕ 10−6 at 185°C. COCl2(g) equilibrium...
The equilibrium constant Kc for the reaction below is 6.16 ✕ 10−6 at 185°C. COCl2(g) equilibrium reaction arrow CO(g) + Cl2(g) COCl2 at an initial concentration of 6.70 ✕ 10−2 M is placed into an empty reaction vessel at 185°C and allowed to equilibrate. The concentration of Cl2 measured after equilibration is 6.39 ✕ 10−4 M. Create an I.C.E. table showing the initial concentrations, change in concentrations, and equilibrium concentrations of the reactants and products of this reaction. PLEASE HELP...
Consider the following reaction and associated equilibrium constant: aA(g)⇌bB(g), Kc = 2.1 A. Find the equilibrium...
Consider the following reaction and associated equilibrium constant: aA(g)⇌bB(g), Kc = 2.1 A. Find the equilibrium concentrations of A and B for a=1 and b=1. Assume that the initial concentration of A is 1.0 M and that no B is present at the beginning of the reaction. [A], [B] =? B. Find the equilibrium concentrations of A and B for a=2 and b=2. Assume that the initial concentration of A is 1.0 M and that no B is present at...
The air pollutant NO is produced in automobile engines from the high-temperature reaction: N2(g)+O2(g)⇌2NO(g) . Kc=1.7×10−3.  Calculate...
The air pollutant NO is produced in automobile engines from the high-temperature reaction: N2(g)+O2(g)⇌2NO(g) . Kc=1.7×10−3.  Calculate the equilibrium concentrations if the initial concentrations are 2.31 M N2 and 0.59 M O2. (This N2/O2 concentration ratio is the ratio found in air.)
Consider the following reaction and associated equilibrium constant: aA(g)⇌bB(g), Kc = 3.8 PART A Find the...
Consider the following reaction and associated equilibrium constant: aA(g)⇌bB(g), Kc = 3.8 PART A Find the equilibrium concentrations of A and B for a=1 and b=1. Assume that the initial concentration of A is 1.0 M and that no B is present at the beginning of the reaction. PART B Find the equilibrium concentrations of A and B for a=2 and b=2. Assume that the initial concentration of A is 1.0 M and that no B is present at the...
The reaction N2(g)+O2(g)⇌2NO(g)  is carried out at a temperature at which Kc = 0.065. The reaction mixture...
The reaction N2(g)+O2(g)⇌2NO(g)  is carried out at a temperature at which Kc = 0.065. The reaction mixture starts with only the product, [NO] = 0.0300 M , and no reactants. 1)Find the equilibrium concentrations of N2 at equilibrium. 2)Find the equilibrium concentrations of O2 at equilibrium. 3)Find the equilibrium concentrations of NO at equilibrium.
The equilibrium constant (Kc) for the following reaction is 6.7 × 10–10 at 630 °C. N2(s)...
The equilibrium constant (Kc) for the following reaction is 6.7 × 10–10 at 630 °C. N2(s) + O2(g) 2 NO(g) What is the equilibrium constant for the reaction below at the same temperature? 1/2 N2(g) + 1/2 O2(g) NO(g) a. 4.5 × 10−19 b. 3.4 × 10−10 c. 1.3 × 10−9 d. 1.8 × 10−5 e. 2.6 × 10−5
The air pollutant NO is produced in automobile engines from the high-temperature reaction N2(g)+O2(g)←−→2NO(g);Kc=1.7×10−3 at 2300...
The air pollutant NO is produced in automobile engines from the high-temperature reaction N2(g)+O2(g)←−→2NO(g);Kc=1.7×10−3 at 2300 K. The initial concentrations of N2 and O2 at 2300 K are both 1.80 M. Part A:What is the concentration of NO when the reaction mixture reaches equilibrium? Part B:What is the concentration of N2 when the reaction mixture reaches equilibrium? Part C:What is the concentration of O2 when the reaction mixture reaches equilibrium?
The reaction N2(g)+O2(g)⇌2NO(g)  is carried out at a temperature at which Kc = 0.050. The reaction mixture...
The reaction N2(g)+O2(g)⇌2NO(g)  is carried out at a temperature at which Kc = 0.050. The reaction mixture starts with only the product, [NO] = 0.0400 M , and no reactants. Find the equilibrium concentrations of N2 at equilibrium. Find the equilibrium concentrations of O2 at equilibrium. Find the equilibrium concentrations of NO at equilibrium.
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT