In which direction does the equilibrium shift as a result of each change?
The following equilibrium takes place in a rigid container:
2NO(g) ---> 2NO(g) + O2(g) deltaH = 54kJ
The arrow is supposed to be two half arrows pointing in opposite directions. Anyway...
In which direction does the equilibrim shift as a result of each change? Why?
a) increasing the surrounding temperature
b) removing NO(g)
c) adding helium gas
- 8 years agoFavorite Answer
your equation itself is wrong....anyway if the reactant is NO2 then-
* on adding helium gas there will be no effect on equilibrium at constant volume and at constant pressure the equilibrium will shift in the forward direction as the number of gaseous moles of products is greater than number of gaseous moles of reactants
*on removing NO(g) the equilibrium is shifted in forward direction
*since the given reaction is an endothermic reaction from left to right,it should be an exothermic reaction from right to left,when the temp. is increased, the equilibrium should shift in such a way to reduce the temp. to normal again,hence heat should be absorbed this is favored in the forward direction,hence the equilibrium will shift in the forward direction
- yauLv 44 years ago
a)left. Favors facet with fewer moles b) Dry ice is CO2 in its solid state. no longer something will ensue c)no longer something forget approximately approximately solid basically concerns as long as some little quantity is modern-day d)properly suited because of the fact the Mg(CLO4)2 is removing particularly some the water e) no exchange for argon its no longer in our equation