For the equilibrium system CO (g) + 3 H 2 (g) <-->H 2 O (g) + CH 4 (g), H = -206
ID: 868743 • Letter: F
Question
For the equilibrium system
CO (g) + 3 H2 (g) <-->H2O (g) + CH4 (g), H = -206 kJ/mol, state whether the yield of CH4 will increase, decrease or remain the same for the following changes:
a. Adding some H2 gas to the system
b. Removing H2O from the system
c. Increasing the volume of the system
d. Decreasing the temperature on the system
e. Adding a catalyst to the system
A sealed glass tube is filled with NO2(brown) and N2O4(colorless). When the tube is inserted in an ice bath color becomes lighter, but it turns dark brown when the tube is put in a hot water bath. Explain this observation. Is the forward reaction exothermic or endothermic?
2 NO2(brown) ? N2O4(colorless)
Explanation / Answer
1 . CO (g) + 3 H2 (g) <-->H2O (g) + CH4 (g), H = -206 kJ/mol
applying lechatliers principle : whaen a system at equilibrium undergoes stress. the equilibriumshifts in such a direction inorder to undo the change.
a. Adding some H2 gas to the system : formation CH4 increases
b. Removing H2O from the system : formation CH4 increases
c. Increasing the volume of the system : No effect
d. Decreasing the temperature on the system : formation CH4 increases.
e. Adding a catalyst to the system : No effect
2. 2 NO2(brown) ---> N2O4(colorless)
at low temperature exothermic reaction takes place
at high temperature endothermic reaction takes place
When the tube is inserted in an ice bath color becomes lighter. That indicates formation of N2O4.
So that forward reaction is exothermic.
in a hot water bath color becomes dark brown . That indicates formation of NO2.