2 NO(g) + O2(g) 2 NO2(g)
For the reaction above tell whether the reaction would shift to the left (L) or right ® if I
a. Increased the total pressure of the system
b. Removed O2 from the system
c. Increased the amount of NO in the system
Perhaps you mean
2 NO + O2 --> 2NO2
3 molecules on left, two on right so if you increase the pressure it will squeeze the reaction to the right more to take up less space.
If you remove O2, the reaction shifts left because you do not have enough O to combine with the NO and pressure is reduced.
If you increase NO, you increase pressure and force the reaction right.
To determine whether the reaction would shift to the left (L) or to the right (R), we need to consider Le Chatelier's principle. Le Chatelier's principle states that when a system in equilibrium is subject to a change in conditions, the equilibrium will shift in the direction that tends to minimize the effect of the change.
a. If the total pressure of the system is increased:
According to Le Chatelier's principle, an increase in pressure will cause the reaction to shift in the direction that reduces the number of moles of gas. In this reaction, the total number of moles of gas on the left side of the equation is 3 (2 NO(g) + O2(g)), while on the right side, it is 2 (2 NO2(g)). Therefore, increasing the total pressure would shift the reaction to the right (R) to reduce the number of moles of gas.
b. If O2 is removed from the system:
Since O2 is a reactant in the given reaction, removing it would decrease the concentration of O2. According to Le Chatelier's principle, removing a reactant would cause the equilibrium to shift in the direction that replaces the reactant. Therefore, the reaction would shift to the left (L) to favor the formation of O2.
c. If the amount of NO is increased in the system:
Increasing the amount of NO would increase the concentration of NO. According to Le Chatelier's principle, increasing the concentration of a reactant would cause the equilibrium to shift in the direction that consumes the added reactant. In this case, it would shift to the right (R) to consume the additional NO.
In summary:
a. Increased total pressure → shift to the right (R)
b. Removed O2 → shift to the left (L)
c. Increased NO → shift to the right (R)