FINISHED_Final_Notebook_Jones
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everse reaction rate as well.<br />
11. In which of the following reactions involving gases would the forward reaction be favored by an<br />
increase in pressure?<br />
A. A + B ⇄AB<br />
B. A + B ⇄ C + D<br />
C. 2A + B ⇄ C + 2D<br />
D. AC ⇄ A + C<br />
Explanation: The answer here is ‘A’ because, the greater the pressure, the greater the ability for the<br />
molecules A and B to collide and form the reactant AB. The other answers are incorrect because A +<br />
B cannot equal C or D. ‘D’ is wrong because an increase in pressure would favor the reverse<br />
reaction, because if you increase pressure, A and C would have a greater chance of colliding with<br />
one another, which would consequently increase the rate of reaction.<br />
4HCl (g)<br />
+ O 2(g)<br />
⇄ 2H2O(l)<br />
+ 2Cl2(g)<br />
+ 113 kJ<br />
12. Which action will drive the reaction to the right?<br />
A. heating the equilibrium mixture<br />
B. adding water to the system<br />
C. decreasing the oxygen concentration<br />
D. increasing the system’s pressure<br />
Explanation: The answer here is “increasing the system’s pressure.” This is the answer because<br />
heating the mixture will cause the reverse reaction to be favored, since heat is a product of the<br />
reaction. Adding water to the system will drive the reaction left, because if more product is added, the<br />
reverse reaction increases. Decreasing the oxygen concentration would reduce the concentration of<br />
products, but also of reactants. Increasing the pressure increases the rate of reaction between<br />
reactants, because of the decreased volume and thus a greater chance of collision (which leads to a<br />
higher rate of reaction)<br />
NO2(g)<br />
+ CO(g)<br />
⇄ NO(g)<br />
+ CO2(g)<br />
13. The reaction shown above occurs inside a closed flask. What action will shift the reaction to the<br />
left?<br />
A. pumping CO gas into the closed flask<br />
B. raising the total pressure inside the flask<br />
C. increasing the NO concentration in the flask<br />
D. venting some CO2 gas from the flask<br />
Explanation: “Increasing the NO concentration in the flask” is the answer to this question. This is<br />
because the larger the volume of NO (a product) in a given space, the greater the chance it has of<br />
colliding with CO 2<br />
, which would thus lead to an increased reaction rate. Pumping more CO (reactant)<br />
into the flask would shift the reaction right, and raising the pressure would increase the production of<br />
product as reactants collide more frequently. Increasing the concentration of reactants would lead to<br />
more product; this is simply because the greater the volume of particles within a given space, the<br />
greater the chance of collision between said particles. Venting CO 2<br />
would result in a greater forward<br />
reaction, again, as the reaction attempts to reach equilibrium, and so NO 2<br />
and CO begin producing<br />
more product.<br />
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