Question detail
A 2.0 g sample of hydrogen peroxide (H₂O₂) decomposes to give 0.50 L of oxygen gas at room temperature and pressure. If the decomposition occurs in 10 s, calculate the mean rate of the reaction in mol s⁻¹.
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At a glance
Question
Type
exam_style
Style
Topic
Rate of reaction
Question
A 2.0 g sample of hydrogen peroxide (H₂O₂) decomposes to give 0.50 L of oxygen gas at room temperature and pressure. If the decomposition occurs in 10 s, calculate the mean rate of the reaction in mol s⁻¹.
Answer
The mean rate of the reaction is 1.0 × 10⁻⁴ mols⁻¹. This calculation links the amount of product formed to the time taken, illustratinghow rate is measured.
Explanation
The answer shows how to convert gas volume to moles usingthe gas volume at RTP formula, then divide by time to give the mean rate. This directly tests the calculation of mean rate of reaction usingproduct formed and time. This answer is strongest when it stays anchored to Factors which affect rates of chemical reactions and directly addresses state that concentration of solutions affects reaction rate.
Common mistake
Misunderstanding Concentration Effects
Students often think that increasing concentration has no effect on the rate of reaction.
To fix this, remember that increasing the concentration of reactants usually increases the rate of reaction due to more frequent collisions between particles.
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