What is the equilibrium constant for 2NO2 and N2O4?

The equilibrium constants for the reaction N2O4 (g)=2NO2 (g), at the temperatures 299.71°, 303.70°, and 308.89°K, have been evaluated by combining precise transmittance measurements for the 5461‐Å mercury line with the known vapor pressures of solid N2O4.

What is the equation for KC for the reaction 2NO2 ⇌ N2O4?

Answer and Explanation: For the given reaction, KC=[NO2]2N2O4=4.64×10−3 K C = [ N O 2 ] 2 N 2 O 4 = 4.64 × 10 − 3 .

What is the equilibrium concentration of N2O4?

For a reaction equilibrium, N2O4(g)→2NO2(g), the concentration of N2O4(g) and NO2 at equilibrium are 4. 8×10−2 and 1. 2×10−2mol/L respectively.

When pressure of the equilibrium reaction N2O4 g → 2NO2 g is increased at constant temperature the equilibrium will?

When there is an increase in pressure, the equilibrium will shift towards the side of the reaction with fewer moles of gas. As in the reaction, reactant side has 1 mole while the product side has two moles of gas. Therefore it shifts the equilibrium in backward direction.

What type of reaction is N2O4 g 2NO2 g?

endothermic
N2O4 (g) 2 NO2 (g) is endothermic.

What type of reaction is N2O4 G 2NO2 G?

What type of reaction is N2O4 2NO2?

Thermodynamic and Transport Properties for the N2O4 yields 2NO2 yields 2NO+O2 (reversible reaction) System.

Is N2O4 G to 2NO2 G endothermic?

In 2NO2(g) ↔ N2O4(g) ΔH = -58.0 kJ/mol N2O4: Being that the reaction as written is exothermic (heat is produced in the forward reaction) we can expect that an increase in temperature in this system will cause the reaction to shift reverse (favor the endothermic reaction) to use the excess heat.

In which direction will the equilibrium shift if N2O4 is added?

As temperature is increased, the above reaction equilibrium shifts to the left, generating a higher concentration of NO2, resulting in the darkening of the reddish brown color inside the tube. Conversely, cooling the reaction shifts the equilibrium to the right, producing more N2O4 which is colorless.