A student carried out an experiment to find the rate of decomposition of hydrogen peroxide into
water and oxygen gas. The student used 100 cm3 of a 1M solution of hydrogen peroxide at 25°C
and 1 atm pressure.
1 g of powdered MnO2 as a catalyst was added and the solution was constantly stirred. The
student measured the total volume of oxygen produced.
The procedure was repeated, but this time using 100 cm3 of 2M hydrogen peroxide, under
identical conditions.
Which option below shows the effect on (R) the rate of reaction, (V) the total volume of oxygen
collected, by using the 2M solution compared to the 1M solution?
I don't see any options.
@DrBob222
Options:
A) R: Doubled; V: Halved
B) R: No effect; V: Doubled
C) R: No effect; V: No effect
D) R: Doubled; V: Doubled
E) R: Doubled; V: No effect
To determine the effect of using a 2M solution of hydrogen peroxide compared to a 1M solution on the rate of reaction (R) and the total volume of oxygen collected (V), we can analyze the given information.
Given:
- Experiment using 1M hydrogen peroxide solution
- Experiment using 2M hydrogen peroxide solution
If the concentration of a reactant is increased, it usually leads to an increase in the reaction rate. Therefore, we can expect that the rate of reaction (R) will be higher when using the 2M solution compared to the 1M solution.
Similarly, since the reaction involves the decomposition of hydrogen peroxide into water and oxygen gas, an increase in the concentration of hydrogen peroxide will result in the production of a greater volume of oxygen gas.
In conclusion, using a 2M solution of hydrogen peroxide compared to a 1M solution will likely increase both the rate of reaction (R) and the total volume of oxygen collected (V).
To determine the effect of using a 2M solution of hydrogen peroxide compared to a 1M solution on the rate of reaction (R) and the total volume of oxygen collected (V), we need to analyze the given information and the principles of the reaction.
The reaction being investigated is the decomposition of hydrogen peroxide (H2O2) into water (H2O) and oxygen gas (O2). This reaction is catalyzed by MnO2.
From the experiment, we know that the student used 100 cm3 of a 1M solution of hydrogen peroxide at 25°C and 1 atm pressure. The student added 1 g of powdered MnO2 as a catalyst and constantly stirred the solution. The total volume of oxygen produced was measured.
Now, let's consider the effect of increasing the concentration of hydrogen peroxide from 1M to 2M.
According to the rate equation for this reaction, the rate of the reaction is directly proportional to the concentration of the reactants. In other words, increasing the concentration of the reactants will increase the rate of the reaction.
Therefore, using a 2M solution of hydrogen peroxide will likely increase the rate of the reaction (R) compared to using a 1M solution.
Now, let's analyze the effect on the total volume of oxygen collected (V).
The decomposition of hydrogen peroxide produces oxygen gas. The total volume of oxygen collected will depend on the amount of hydrogen peroxide decomposed.
Since the 2M solution of hydrogen peroxide has a higher concentration, it contains more moles of hydrogen peroxide than the 1M solution. Therefore, using the 2M solution will provide more moles of reactant available for decomposition, resulting in a higher total volume of oxygen collected (V) compared to the 1M solution.
In conclusion, the effect on the rate of reaction (R) is that it will increase when using the 2M solution compared to the 1M solution. The effect on the total volume of oxygen collected (V) is that it will also increase when using the 2M solution compared to the 1M solution.