Hydrogen peroxide gradually decomposes into water and oxygen, according to the following equation - Scottish Highers Chemistry - Question 1 - 2016
Question 1
Hydrogen peroxide gradually decomposes into water and oxygen, according to the following equation.
$2H_2O_2(aq) \rightarrow 2H_2O(l) + O_2(g)$
(a) At room temperat... show full transcript
Worked Solution & Example Answer:Hydrogen peroxide gradually decomposes into water and oxygen, according to the following equation - Scottish Highers Chemistry - Question 1 - 2016
Step 1
State why increasing the temperature causes an increase in reaction rate.
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Answer
Increasing the temperature causes a rise in the kinetic energy of the particles. As temperature increases, particles move faster, leading to a higher frequency of successful collisions. Additionally, more particles will have sufficient energy to overcome the activation energy barrier.
Step 2
Complete the diagram below to show how the gas produced can be collected and measured.
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Answer
The diagram should show a gas syringe or an inverted measuring cylinder submerged in water to collect the oxygen gas. Ensure that the gas is channeled from the reaction vessel to either collection method.
Step 3
Calculate the volume strength of the hydrogen peroxide.
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Answer
Using the formula provided:
volume strength=volume of hydrogen peroxide solutionvolume of oxygen produced
Substituting the values:
volume strength=20 cm374 cm3=3.7
Thus, the volume strength of the hydrogen peroxide is 3.7.
Step 4
Calculate the time taken, in s, for the reaction when the concentration of potassium iodide used was 0.6 mol l⁻¹.
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Answer
From the graph, identify the rate of reaction for a concentration of 0.6 mol l⁻¹. Let's say it's approximately 0.2 s⁻¹. The time taken can be calculated as:
time=rate1=0.21=5exts
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