(a) Methanol is manufactured from carbon (IV) oxide and hydrogen gas according to the equation:
The reaction is carried out in the presence of a chromium catalyst at 700K and 30kPa. Under these conditions, equilibrium is reacted when 2% of the carbon (IV) oxide is converted to methanol
(i) How does the rate of the forward reaction compare with that of the reverse reaction when 2% of the carbon (IV) oxide is converted to methanol?
(ii) Explain how each of the following would affect the yield of methanol:
II Using a more efficient catalyst
(iii) If the reaction is carried out at 500K and 30kPa, the percentage of carbon (IV) oxide converted to methanol is higher than 2%
I what is the sign of ΔH for the reaction? Give a reason
II Explain why in practice the reaction is carried out at 700K but NOT at 500K
(b) Hydrogen peroxide decomposes according to the following equation
: 2H2O2(aq) →2H2O(l) + O2 (g)
In an experiment, the rate of decomposition of hydrogen peroxide was found to be 6.0 x 10-8 mol dm-3 S-1.
(i) Calculate the number of moles per dm3 of hydrogen peroxide that had decomposed within the first 2 minutes
(ii) In another experiment, the rate of decomposition was found to be 1.8 x 10-7 mol dm-3S-1. The difference in two rates could have been caused by addition of a catalyst. State, giving reasons, one other factor that may have caused the difference in two rates of decomposition
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Maurice Atika is a teacher and a netprenuer.