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5 marksMole Concept

CSEC Chemistry · January 2006 · Paper 2 · Question 3(b)(ii)b)

Figure 4 shows the rate of hydrogen peroxide decomposition as a plot of grams of oxygen liberated per second against mass of catalyst for both 0.40 and 0.80 mol dm⁻³ hydrogen peroxide.

For 0.80 mol dm⁻³ H₂O₂ and 4.0 g of catalyst, determine the number of moles of O₂ produced in 16 seconds. [Atomic mass: O = 16]

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Other parts of this question

  1. 3(a)(i)Name THREE factors OTHER THAN a catalyst, which can affect the rate of a chemical reaction.[3 marks]
  2. 3(a)(ii)Write a balanced equation to show the decomposition of hydrogen peroxide by manganese (IV) oxide, MnO₂.[2 marks]
  3. 3(b)(i)Explain why the plots in Figure 4 are different.[2 marks]
  4. 3(b)(ii)a)For 0.80 mol dm⁻³ H₂O₂ and 4.0 g of catalyst, determine the quantity of O₂ produced in 16 seconds.[5 marks]
  5. 3(b)(ii)c)For 0.80 mol dm⁻³ H₂O₂ and 4.0 g of catalyst, determine the volume of O₂ produced at S.T.P. in 16 seconds. [1 mole of gas occupies 22.4 dm³ at S.T.P.][5 marks]
  6. 3(c)Draw a fully labelled energy profile diagram to illustrate how the catalyst affects the rate of decomposition of hydrogen peroxide.[3 marks]

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