Discuss: Reaction-Rate Factors

1 answer:

3 0

1) The time depends on what the lab wanted you to do. It will tell you in the procedure when you are supposed to considered a reaction to be complete and you just measure the time for that to happen.

2) Most text books say that increasing the concentration of one or more reactants will increase the rate of the reaction. To prove this with your data you need to show that when you increased the concentration of one of the reactants, the reaction rate did increase. The results of this experiment are not enough to make a general statement since the experiment was not on a large enough scale to diffidently prove anything. (you could have been testing the one exception or had a error in one of your trials)
I hope this helps. Let me know in the comments if anything is unclear.

(The concentration of one or more of the reactants will increase the rate of the reaction. This is explained through the fact that all reactions require collisions that have certain orientations and a minimum energy level. By increasing the concentration of one or more reactants, you increase the number of collisions which increases the rate since requires collisions in order to occur.)

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If 5.4 moles of Fe react with 4.7 moles of O2, what is the maximum amount of Fe2O3 (in moles) that can be produced? What is the

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Answer:

2.7 moles of Fe₂O₃ is the maximum amount that can be produced. Iron is the limiting reactant.

Explanation:

The balanced reaction is:

4 Fe + 3 O₂ → 2 Fe₂O₃

By reaction stoichiometry (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of each compound participate in the reaction:

Fe: 4 moles
O₂: 3 moles
Fe₂O3: 2 moles

The limiting reagent is one that is consumed first in its entirety, determining the amount of product in the reaction. When the limiting reagent is finished, the chemical reaction will stop.

You can use a simple rule of three as follows: if by stoichiometry 4 moles of Fe reacts with 3 moles of O₂, how much moles of Fe will be needed if 4.7 moles of O₂ react?

$moles of Fe =\frac{4. moles of Fe*4.7 moles of O_{2}}{3 moles of O_{2} }$

moles of O₂= 6.27

But 6.27 moles of Fe are not available, 5.4 moles are available. Since you have less moles than you need to react with 4.7 moles of O₂, iron Fe will be the limiting reagent.

So you can use a simple rule of three as follows: if by stoichiometry 4 moles of Fe produce 2 moles of Fe₂O₃, how many moles of Fe₂O₃ will be produced if 5.4 moles of Fe react?

$moles of Fe_{2}O_{3}=\frac{5.4 moles of Fe*2 moles of Fe_{2} O_{3} }{4 moles of Fe}$