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- Answer: C<br />
- The answer is C because to increase the rate of a reaction, you would have to use a catalyst<br />
to move the rate up<br />
- The definition of a catalyst is “A substance that increases the rate of a chemical reactions<br />
without itself undergoing any permanent chemical change.”<br />
- In most equations, by simply increasing the pressure or temperature, the reaction rate will be<br />
increased.<br />
- -Here in this equation, by increasing the pressure of 2H2O2, that will make the reaction occur<br />
not as fast than it normally would.<br />
3 For the reaction<br />
A + (aq) + B — (aq) → AB (s)<br />
increasing the temperature increases the rate of the reaction. Which is the best explanation for this<br />
happening?<br />
A The pressure increases, which in turn increases the production of products.<br />
B The concentration of reactants increases with an increase in temperature.<br />
C The average kinetic energy increases, so the likelihood of more effective collisions between ions<br />
increases.<br />
D Systems are more stable at high temperatures.<br />
- The Collison Theory us when atoms, ions and molecules react in order to form products by<br />
colliding with one another’s. It explains why some reactants are extremely slow at room<br />
temperature.<br />
- If having enough kinetic energy those who do not have enough energy will bounce apart,<br />
unchanged<br />
- Activation Energy – minimum energy that particles who collide must have to react<br />
- -The answer would be letter D because, when the temperature is increased, that makes the<br />
pressure increase too, and when the pressure is increased, the rate of the reaction would also<br />
be increasing, thus explaining how the rate of reaction is increasing.<br />
- -Both Temperature and rate of reaction have a relationship with the pressure of the equation.<br />
- This problem is similar to question number 2, when the pressure of temperature is increased,<br />
the rate will happen faster.<br />
- Here when the temperature gets increased, that will let A and B come together in a quicker<br />
way than expected because of the heat.<br />
4 Which statement explains why the speed of some reactions is increased when the surface area of<br />
one or all the reactants is increased?<br />
A increasing surface area changes the electronegativity of the reactant particles<br />
B increasing surface area changes the concentration of the reactant particles<br />
C increasing surface area changes the conductivity of reactant particles<br />
D increasing surface area enables more reactant particles to collide<br />
- The answer is letter D because when the surface area is increased the concentration does get<br />
changed because it will decrease.<br />
- If the concentration of the reactant particles were to decrease, the substance would have a<br />
lower electronegativity.<br />
- When I was figuring out the problem, i thought of how the concentration of a substance gets<br />
watered down with ice, because there is more substance in the container. this would be the<br />
same case when you increase the surface area there will be more room for the particles to be<br />
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