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Hydrogen peroxide decomposes rapidly in the presence of a manganese(IV) oxide (MnO₂) catalyst - Leaving Cert Chemistry - Question 3 - 2005
Question 3
Hydrogen peroxide decomposes rapidly in the presence of a manganese(IV) oxide (MnO₂) catalyst. (a) Write a balanced equation for the decomposition of hydrogen perox... show full transcript
Worked Solution & Example Answer:Hydrogen peroxide decomposes rapidly in the presence of a manganese(IV) oxide (MnO₂) catalyst - Leaving Cert Chemistry - Question 3 - 2005
Step 1
Step 2
Use the graph to determine the instantaneous rate of the reaction at 2.5 minutes.
Answer
To determine the instantaneous rate of the reaction at 2.5 minutes, draw a tangent to the curve at this point. Measure the slope of the tangent line, which represents the rate of change in volume of O₂ over time. This slope gives the instantaneous rate of oxygen production in cm³/min.
Step 3
What changes would you expect in the graph if the experiment were repeated using a solution of the same volume but exactly half the concentration of the original hydrogen peroxide solution?
Answer
If the concentration of the hydrogen peroxide solution is halved, the overall rate of reaction would decrease. This graphical representation would show a slower increase in the volume of oxygen produced over time, resulting in a curve that flattens more gradually compared to the original experiment. The maximum volume of O₂ would still be the same but would take longer to achieve.