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

The rate of reaction is not dependent on the volume of hydrogen peroxide solution. 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

Based on your results, how does increasing the concentration of hydrogen peroxide affect the rate of reaction?

You decomposed hydrogen peroxide in the lab. You and your partner do not agree on what the chemical reaction is. The following are the proposed reactions: Your reaction:H2 O2 → H2 + O2 Your partner’s reaction: 2 H2 O2 → 2 H2 O + O2 The following data was collected: Mass of Beaker36.39 g Mass of Beaker and H2 O2 before Rxn 41.31 g Mass of O2 gas Collected during Rxn 2.32 g Using the data above, prove which reaction is correct. Support your answer with stoichiometry.

*19* Turn over ► IB/M/Jun23/8464/C/2H Do not write outside the box 0 6 . 1 The equation for the decomposition of hydrogen peroxide is: 2 H2O2 → 2 H2O + O2 Describe a test to identify the gas produced in the reaction. [2 marks] Test Result