Question

Consider the following reaction: N2(g)+O2(g) <-=-> 2NO(g) At a cetain temperatre, the equilibrium constant for the...

Consider the following reaction:

N2(g)+O2(g) <-=-> 2NO(g)

At a cetain temperatre, the equilibrium constant for the reaction is 0.0639. What are the partial pressuers of all gases at equilibrium if the initial partial pressuer of the gases (both products and reactants) is 0.400atm.

Homework Answers

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
Consider the reaction: N2(g)+O2(g)<=>2NO(g). Suppose a sample of air contains initially N2]=0.80M and [O2]=0.20M. Calculate the...
Consider the reaction: N2(g)+O2(g)<=>2NO(g). Suppose a sample of air contains initially N2]=0.80M and [O2]=0.20M. Calculate the equilibrium concentration of all reactants and products at equilibrium if Kc= 1.0x10-5 and if Kc=1.20
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
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.
The following reaction establishes equilibrium at 2000K: N2(g) + O2(g) ⇌ 2NO(g) where Keq = 4.1...
The following reaction establishes equilibrium at 2000K: N2(g) + O2(g) ⇌ 2NO(g) where Keq = 4.1 x 10-4 If the reaction began with 0.150 M of N2 and 0.150 M of O2, the equilibrium concentration of NO would be
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.
1) Identify the proper form of the equilibrium-constant expression for the equation N2(g)+O2(g)⇌2NO(g) K=[NO]   / [N2][O2]...
1) Identify the proper form of the equilibrium-constant expression for the equation N2(g)+O2(g)⇌2NO(g) K=[NO]   / [N2][O2] K=[NO]2 / [N2][O2] K=[N2][O2]   /   [NO]2 K=2[NO][N2]   /   [O2] 2) The acid HOCl (hypochlorous acid) is produced by bubbling chlorine gas through a suspension of solid mercury(II) oxide particles in liquid water according to the equation 2HgO(s)+H2O(l)+2Cl2(g)⇌2HOCl(aq)+HgO⋅HgCl2(s) What is the equilibrium-constant expression for this reaction? K=[HOCl]2   /   [Cl2]2 K=[HOCl]2[HgO⋅HgCl2]    /   [Cl2]2[H2O][HgO]2 K=[HOCl]2    /     [Cl2]2[H2O] K=[Cl2]2    /    [HOCl]2
Consider the reaction: 1/2 N2(g) + O2(g)<<<----->>>NO2(g) Write the equilibrium constant for this reaction in terms...
Consider the reaction: 1/2 N2(g) + O2(g)<<<----->>>NO2(g) Write the equilibrium constant for this reaction in terms of the equilibrium constants, Ka and Kb, for reactions a and bbelow: a.) N2O4(g) <-------> 2NO2(g) Ka b.) N2(g) + 2 O2(g) <------> N2O4(g) Kb K =
At a given temperature the gas phase reaction: N2 + O2 2NO has an equilibrium constant...
At a given temperature the gas phase reaction: N2 + O2 2NO has an equilibrium constant of4.00x10-2 . What will be the concentration of NO at equilibrium, if1.00 moles of nitrogen and 1.00 moles of oxygen are allowed to cometo equilibrium in a 250 mL flask?
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 for the reaction N2 + O2<--> 2NO is 1.69 × 10^?3 at 2300...
The equilibrium constant for the reaction N2 + O2<--> 2NO is 1.69 × 10^?3 at 2300 K. A mixture consisting of 2 mol of nitrogen and 1.0 mol of oxygen is heated to 2300 K at 1 bar and allowed to come to equilibrium. Calculate the mole fraction of NO at equilibrium.
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT