(FINAL) Chemistry Notebook 2016-17

12 Which action will drive the reaction to the right?
A heating the equilibrium mixture
B adding water to the system
C decreasing the oxygen concentration
D increasing the system’s pressure
4HCl(g) + O2(g) ⇄ 2H2O(l) + 2Cl2(g) + 113 kJ
* Increasing the pressure on this reaction would drive the reaction to the right, because when the
pressure is increased in a reaction, the point of equilibrium is shifted towards the side with less
molecules. In this reaction, the right side has less molecules, and so the system will try to achieve
equilibrium in order to reduce the pressure to its original amount. In order to do this, it’s shifted from
left to right*
NO2(g) + CO(g) ⇄ NO(g) + CO2(g)
13 The reaction shown above occurs inside a closed flask. What action will shift the reaction to the
left?
A pumping CO gas into the closed flask
B raising the total pressure inside the flask
C increasing the NO concentration in the flask
D venting some CO2 gas from the flask
* In order to shift the reaction to the left, increasing the concentration of NO would be the most viable
method. NO is a product, and by increasing its concentration, it will collide more with CO2, causing
the reaction to shift to the left. If you were to pump in more CO the reaction rate would only shift to the
right because of the increased amount of collisions on the right side, and venting out CO2 would only
make the reaction try to reach equilibrium from the left to the right. Raising the total pressure would
barely do anything at all, because the number of molecules on both sides wouldn’t change at all, so
the equilibrium wouldn’t move in any way to try to reduce the pressure, meaning that the reaction
would not shift at all.
NH4Cl(s) + heat ⇄ NH3(g) + HCl(g)
14 What kind of change will shift the reaction above to the right to form more products?
A a decrease in total pressure
B an increase in the concentration of HCl
C an increase in the pressure of NH3
D a decrease in temperature
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