Question

Decomposition of nitrogen dioxide into nitrogen oxide gas is an equillibrium process described by the following equation: 2NO2(g)--2NO(g)+ O2(g), deltaH=-98.7kj. Predict whether the position of equilberium will shift to the right left or no change.

-increase the concentration of NO

-Decrease the concentration of NO2

-Increase the pressure by the addition of helium gas

-Increase the pressure by decreasing the volume

- Decrease the temp

-Add a catalyst

Answer 1

Ans 2 NO2(g) 22 NO (g) + O2(g) DH=-98.7kJ Increasing the [Nos, a becomes greater than the kc Kc and thus the seria equilibrium will shift to the left greater t and thus, the e Decreasing the [Noz], @ become than ke equilibrium will shiut to the left. Increasing the pressure by the addition of helium 902.. will not change the partial pressures of all the other gases present in the container. So, the system will rer equilibrium and thus, no change main at occurra.

the in the جي رحيييلم rxh 3-2 = will 부 • Increasing the pressure by decreasing volume will increase the partial pressures of all the gases containes proportionally Dng of is greater than °the equilibrium shift to the left As DHZO, decreasing the temp. increase the value of and o becomes less than * the equilibrium shifts to the rights Adding a catalyst only changes the rxn change the equilibrium constant So, there is the equilibrium. will k . now, as the rate of change in