The rate of reaction is not dependent on the volume of hydrogen peroxide solution. Explain why.
Question
The rate of reaction is not dependent on the volume of hydrogen peroxide solution. Explain why.
Solution
The rate of reaction is not dependent on the volume of hydrogen peroxide solution because the rate of reaction is determined by the concentration of the reactants, not their total volume. The concentration of hydrogen peroxide dictates how many molecules are available to react at any given time. As long as the concentration remains constant, the rate of reaction will remain the same, regardless of the total volume of the solution. Additionally, other factors such as temperature, presence of a catalyst, and surface area of reactants can influence the rate of reaction, but the volume of the solution itself does not directly affect it.
Similar Questions
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Using 10 cm 3of hydrogen peroxide solution gives less accurate results than using 20 cm 3of hydrogen peroxide solution of the same concentration. Explain why.
The equation for the decomposition of hydrogen peroxide is shown.2H_{2}*O_{2}(aq) -> 2H_{2}*O(l) + O_{2}(g) 25.0 cm³ of aqueous hydrogen peroxide forms 48.0 cm³ of oxygen at room temperature and pressure (r.t.p.).Calculate the concentration of aqueous hydrogen peroxide at the start of the experiment using the following steps.Calculate the number of moles of oxygen formed.molDeduce the number of moles of hydrogen peroxide that decomposed.molCalculate the concentration of hydrogen peroxide in mol / d * m ^ 3mol / d * m ^ 3[3]Calculate the volume of O, gas, at room temperature and pressure ( r .t.p.) needed to produce 1260 g of HNO3. Use the following steps.4.The equation for the reaction in stage 3 is shown.4N*O_{2} + 2H_{2}*O + O_{2} -> 4HNO
In this experiment some students will be determining how the rate of the reaction depends on the concentration of hydrogen peroxide. Which of the solutions you will be supplied with contain hydrogen peroxide?Question 2Answersolution A1 onlysolution B1 onlysolutions B1 and B2solutions A1 and B1solutions A1 and A2
) CalculatetheconcentrationofH2 O2 in FA 3, in mol dm –3 . concentrationofH2 O2 in FA 3 = .............................. mol dm–3 [1](v) When hydrogen peroxide decomposes in the presence of a catalyst, oxygen is produced.H2 O2(aq) H2O(l)+12 O2(g) The ‘volume strength’ of hydrogen peroxide is equal to the volume of oxygen, in dm3 ,produced under room conditions, when 1.00 dm 3 of the solution decomposes.Use your answer to (c)(iv) and the equation above to calculate the volume, in dm3 , ofoxygen produced when 1.00 dm3 of FA 3 decomposes. This is the ‘volume strength’, in vol,of FA 3. (Underroomconditions1.00molofgasoccupiesavolumeof24.0dm3 . If you were unable to calculate the concentration of H2 O2 in FA 3, assume that it is1.02 mol dm –3 . This may not be the correct value.)‘volume strength’ of FA 3 = .............................. vol [2](d) Themaximumerrorinreadinga25.0cm3pipetteis±0.06cm3 . Showbycalculationthatthepipetteismoreaccuratethanaburetteformeasuring25.0cm3 ofsolution................................................................................................................................................................................................................................................................................................... [1] [Total:15]
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