Your friend is looking at your graph and states that she believes that step (ii) is the rate determining step. Do you agree with her? If you do not agree with her, what step would you pick as the RDS:
#(b):
The overall chemical equation can be obtained by adding the three elementary step reactions and canceling the common species like "Pt(s)", "Cl(g)" and "ClCO(g)"
(i): Cl2(g) + Pt(s) 2Cl(g) + Pt(s)
(ii): Cl(g) + CO(g) + Pt(s) ClCO(g) + Pt(s)
(iii): Cl(g) + ClCO(g) Cl2CO(g)
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Adding the above 3 equations and canceling the common species like "Pt(s)", "Cl(g)" and "ClCO(g)" gives:
Overall chemical equation, Cl2(g) + CO(g) Cl2CO(g) (Answer)
#(c):
Initial enthalpy, H(Initial) = 600 kJ
The final enthalpy can be obtained by adding the enthalpies of all the 3 elementary reactions.
Hence the final enthalpy, H(Final)
= H(i) + H(ii) + H(iii)
= - 950 kJ + 575 kJ - 825 kJ
= -1200 kJ
Overall change in enthalpy, H = H(Final) - H(Initial) = - 1200 kJ - 600 kJ = - 1800 kJ
Overall change in enthalpy = - 1800 kJ (Answer)
#(d):
Overall activation energy can be obtained by adding the activation energy(Ea) of all the elementary reactions.
Overall activation energy, Ea = Ea(i) + Ea(ii) +Ea(iii) = 1550 kJ + 2240 kJ + 2350 kJ = 6140 kJ
Overall activation energy = 6140 kJ (Answer)
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