Given the reaction below: N2O4(g)→2NO2(g)N2O4(g)→2NO2(g) d) You increase [NO2][NO2], but change nothing else about the system....

Question

Question

Given the reaction below:

N2O4(g)→2NO2(g)N2O4(g)→2NO2(g)

d) You increase [NO2][NO2], but change nothing else about the system. How will this affect the value of K?

Select one:

a. K will decrease.

b. K will increase.

c. K will not change.

Answer 1

Answer #1

N ₂ Oyly) - 2N02 K= No 272 N2oy K only depends here charge Nog does not on temperature charge & c) I will not charge.

Answer 2

Similar Homework Help Questions

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
N2O4(g)→2NO2(g)N2O4(g)→2NO2(g) c) Based on the K value calculated in 4c, which of the following is true...

N2O4(g)→2NO2(g)N2O4(g)→2NO2(g) c) Based on the K value calculated in 4c, which of the following is true about the reaction when it is performed at 100˚C? Select one or more: a. The reaction is nonspontaneous. b. The reaction is spontaneous.
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

For the reaction N2O4(g)⇌2NO2(g), the value of K at 25∘C is 7.19×10−3. Calculate [NO2] at equilibrium...

For the reaction N2O4(g)⇌2NO2(g), the value of K at 25∘C is 7.19×10−3. Calculate [NO2] at equilibrium when [N2O4]=6.90×10−2mol/L.
Consider the following reaction. 2NO2(g)⇌N2O4(g) When the system is at equilibrium, it contains NO2 at a...

Consider the following reaction. 2NO2(g)⇌N2O4(g) When the system is at equilibrium, it contains NO2 at a pressure of 0.870 atm, and N2O4 at a pressure of 0.0757 atm. The volume of the container is then reduced to half its original volume. What is the pressure of each gas after equilibrium is reestablished?
Consider the following reaction. 2NO2(g)⇌N2O4(g) When the system is at equilibrium, it contains NO2 at a...

Consider the following reaction. 2NO2(g)⇌N2O4(g) When the system is at equilibrium, it contains NO2 at a pressure of 0.722 atm, and N2O4 at a pressure of 0.0521 atm. The volume of the container is then reduced to half its original volume. What is the pressure of each gas after equilibrium is reestablished? PNO2= ?? atm PN2O4= ?? atm

For the reaction at 298 K, 2NO2 g → N2O4 g the values of ΔHo and...

For the reaction at 298 K, 2NO2 g → N2O4 g the values of ΔHo and ΔSo are -58.0 kJ and -177 J/K, respectively. What is the value of ΔG nonstandard at 298 K when the concentration of N2O4 is 1.69 M and the concentration of NO2 is 2.75 M? Remember to answer in correct units. ΔG=
The value of Kc for the the following reaction is 0.470 at 471 K. N2O4(g)---->2NO2(g) Part 1)...

The value of Kc for the the following reaction is 0.470 at 471 K. N2O4(g)---->2NO2(g) Part 1) If a reaction vessel at that temperature initially contains 0.0200 M NO2 and 0.0200 M N2O4, what is the concentration of NO2 at equilibrium? _______M? part 2) What is the concentration of N2O4 at equilibrium? _______M?
what happens at the molecular level when the following reaction occurs? N2O4(g)>2NO2(g) What change in entropy...

what happens at the molecular level when the following reaction occurs? N2O4(g)>2NO2(g) What change in entropy and enthalpy occur for this reaction? - Both entropy and enthalpy will increase -Entropy will increase, but enthalpy will decrease -Entropy will decrease, but enthalpy will increase -Both entropy and enthalpy will decrease Explain

Consider the equilibrium constant Kc for the reaction: N2O4(g) ↔ 2NO2(g) is 0.211 at 100°C. What...

Consider the equilibrium constant Kc for the reaction: N2O4(g) ↔ 2NO2(g) is 0.211 at 100°C. What is the value for the equilibrium constant is the reaction is balanced as ½ N2O4(g) ↔ NO2(g) ? A. 0.106 B. 0.459 C. 0.211 D. 0.422