Decomposition of H2O2 follows a first order reaction. In fifty minutes the concentration of H2O2 decreases from 0.5 to 0.125 M in one such decomposition. When the concentration of H2O2 reaches 0.05 M, the rate of formation of O2 will be:

Hydrogen peroxide decomposes in a first order reaction according to:2 H 2 O 2 (aq) ® H 2 O (l) + O 2 (g)The half-life for the decomposition process is t 1/2 = 360 minutes at 38.0 ℃i. (2 marks)Calculate the value for the rate constant, k 1 for the forward reaction at 38.0 ℃ii. (2 marks)If after 1080 mins, the concentration of H 2 O 2 in a sample is measured to be0.154 mol L-1 , calculate the initial concentration of the H 2 O 2 in this sample.iii. (1 mark)Assuming the decomposition follows Arrhenius behaviour, calculate the Arrheniusconstant for this decomposition process if the activation energy is 42 kJ mol -1 .k1

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

Oxygen and water are produced when hydrogen peroxide breaks down. The chemical term for this process is decomposition. The decomposition of H2O2 happens naturally at a slow rate, as shown in the equation below:2H2O2 (aq) → 2H2O (l) + O2 (g)Outline how you would test that oxygen was produced.

Suppose the decomposition of ozone proceeds by the following mechanism:step elementary reaction rate constant1 O3(g) → O2(g) + O(g) k12 O3(g) + O(g) → 2O2(g) k2Suppose also k1≫k2. That is, the first step is much faster than the second.Write the balanced chemical equation for the overall chemical reaction: Write the experimentally-observable rate law for the overall chemical reaction. =ratek Note: your answer should not contain the concentrations of any intermediates.Express the rate constant k for the overall chemical reaction in terms of k1, k2, and (if necessary) the rate constants k-1 and k-2 for the reverse of the two elementary reactions in the mechanism. =k

You are asked to investigate the effect of temperature on the rate of decomposition of aqueoushydrogen peroxide.Aqueous hydrogen peroxide decomposes to make oxygen gas.hydrogen peroxide , water + oxygenThe reaction is very slow unless a catalyst is added to the hydrogen peroxide.Manganese(IV) oxide is a catalyst for this reaction.Plan an investigation to find how the temperature of the aqueous hydrogen peroxide afects the rate of the catalysed reaction. Your answer should include an explanation of how your resul's wil tell you how the rate of reaction has changed.You are provided with aqueous hydrogen peroxide, manganese(IV) oxide and common laboratoryapparatus.