Nitrogen dioxide dimerizes according to the following reaction: 2NO2(g)⇌N2O4(g) Kp=6.7at298K A 2.35-L container contains 0.057 mol...

Question

Question

Nitrogen dioxide dimerizes according to the following reaction:

2NO2(g)⇌N2O4(g)
Kp=6.7at298K

A 2.35-L container contains 0.057 mol of NO2 and 0.084 molof N2O4at298K.

Calculate Kc for the reaction.

Express the equilibrium constant with respect to concentration to three significant figures.

Calculate Q for the reaction.

Express the reaction quotient to three significant figures.

Answer 1

✔ Recommended Answer

Answer #1

if you have any query please comment...

If satisfied please rate it thanks...

Answer 2

Similar Homework Help Questions

Nitrogen dioxide dimerizes according to the following reaction: 2NO2(g)⇌N2O4(g) Kp=6.7at298K A 2.35-L container contains 0.052 mol...

Nitrogen dioxide dimerizes according to the following reaction: 2NO2(g)⇌N2O4(g) Kp=6.7at298K A 2.35-L container contains 0.052 mol of NO2 and 0.087 mol of N2O4at298K. Calculate Q for the reaction.
Decomposition of nitrogen dioxide dimer N2O4 is described by the reaction: N2O4(g) = 2NO2(g) Concentration of...

Decomposition of nitrogen dioxide dimer N2O4 is described by the reaction: N2O4(g) = 2NO2(g) Concentration of N2O4 became 2 times less after 2,5⋅103 s. You have to calculate: a) the value of rate constant k of the reaction; b) the value of equilibrium constant Kp. You are given the value of standard Gibb’s energy of formation Goform: substance Goform, kJ/mol NO2(g) 51.6 N2O4(g) 98.4
Question text Calculate the equilibrium constants, KpKp and KcKc for the equilibrium reaction N2O4(g)⇄2NO2(g)N2O4(g)⇄2NO2(g) at 298...

Question text Calculate the equilibrium constants, KpKp and KcKc for the equilibrium reaction N2O4(g)⇄2NO2(g)N2O4(g)⇄2NO2(g) at 298 K. N2O4(g)N2O4(g) NO2(g)NO2(g) S0S0 (J/K/mol) 304.29 240.06 ΔfH0ΔfH0 (kJ/mol) 9.16 33.18 Select one or more: A. Kp=9.23Kp=9.23 , Kc=12.3Kc=12.3 B. Kp=0.563Kp=0.563 , Kc=0.33Kc=0.33 C. Kp=0.144Kp=0.144 , Kc=0.0058Kc=0.0058 D. Kp=0.355Kp=0.355 , Kc=1.23

The equilibrium constant, Kc, for the reaction N2O4(g)⇌2NO2(g) is 5.1×10−3. If the equilibrium mixture contains [NO2]...

The equilibrium constant, Kc, for the reaction N2O4(g)⇌2NO2(g) is 5.1×10−3. If the equilibrium mixture contains [NO2] = 0.047 M , what is the molar concentration of N2O4? Express the concentration to two significant figures and include the appropriate units.
Chemical equilibrium

Nitrogen Dioxide Dimerizes according th the following reaction2NO2(g) = N2O4(g)Kp= 6.7 a 298 kA 2.25 L container contains 0.055 mol of NO2 and 0.082 mol N2O4 at 298kIs the reaction at equilibrium? If not, in what direction will the reaction proceed?
Dinitrogen tetroxide decomposes to nitrogen dioxide: N2O4(g)→2NO2(g)ΔHorxn= 55.3kJ At 298 K, a reaction vessel initially contains...

Dinitrogen tetroxide decomposes to nitrogen dioxide: N2O4(g)→2NO2(g)ΔHorxn= 55.3kJ At 298 K, a reaction vessel initially contains 0.100 atm of N2O4. When equilibrium is reached, 58% of the N2O4 has decomposed to NO2. What percentage of N2O4 decomposes at 380 K ? Assume that the initial pressure of N2O4 is the same (0.100 atm).

Consider the following reaction: N2O4(g)⇌2NO2(g),Kc=0.36 at 2000∘C The reaction mixture initially contains only the reactant, [N2O4]=0.0300M...

Consider the following reaction: N2O4(g)⇌2NO2(g),Kc=0.36 at 2000∘C The reaction mixture initially contains only the reactant, [N2O4]=0.0300M , and no NO2. Find the equilibrium concentration of N2O4. Find the equilibrium concentration of NO2.
Dinitrogen tetroxide decomposes to nitrogen dioxide: N2O4(g)→2NO2(g) ΔrH∘=55.3kJmol−1 At 298 K, a reaction vessel initially contains...

Dinitrogen tetroxide decomposes to nitrogen dioxide: N2O4(g)→2NO2(g) ΔrH∘=55.3kJmol−1 At 298 K, a reaction vessel initially contains 0.100 bar of N2O4. When equilibrium is reached, 58% of the N2O4 has decomposed to NO2. What percentage of N2O4 decomposes at 369 K? Assume that the initial pressure of N2O4 is the same (0.100 bar)
Kp for the reaction: N2O4(g)<======> 2NO2(g) in 25C is 0.15. A certain amount of N2O4(g) is...

Kp for the reaction: N2O4(g)<======> 2NO2(g) in 25C is 0.15. A certain amount of N2O4(g) is being inserted into a container in 25C and at equilibrium, the pressure was 0.54 bar. a. what is the partial pressure of each of the system's components at equilibrium? **show detailed calculations in salving the two equations that you will receive. (answers should be : p=0.43, x=0.11 so that: Peq(N2O4)= 0.32bar And Peq(NO2)=0.22bar)

Dinitrogen tetroxide decomposes to nitrogen dioxide: N2O4(g)→2NO2(g) ΔrH∘=55.3kJmol−1 At 298 K, a reaction vessel initially contains...

Dinitrogen tetroxide decomposes to nitrogen dioxide: N2O4(g)→2NO2(g) ΔrH∘=55.3kJmol−1 At 298 K, a reaction vessel initially contains 0.100 bar of N2O4. When equilibrium is reached, 58% of the N2O4 has decomposed to NO2. What percentage of N2O4 decomposes at 389 K? Assume that the initial pressure of N2O4 is the same (0.100 bar). Please use bar and not atm.