Write the balanced chemical equation for the second step - Inorganic Chemistry

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Consider the reaction
NO₂ (g) + CO(g) CO₂ (E) + NO(g)
for which the rate equation has been shown by experiment to be
Rate = k[NO2]²
_{The first step of the two-step reaction is the rate-determining step. The equation for this step is}
NO₂(g) + NO₂(g) -> NO₂ (g) + NO(g)
(a) Write the balanced chemical equation for the second step, which completes the reaction
(b) The table below gives the kinetic data for the above reaction at a constant temperature

Determine the values of x and y in the table. Show detailed workings.
8. The rate of consumption of B in the reaction A + 3B C +2E is 2.0 mol.dm ⁼³.s⁼¹
(i) Determine the rate of the reaction. Show detailed workings.
(ii) Determine the rates of formation and consumption of A, C and E. Show detailed workings.
9. A certain reaction has a rate law of the form: v = k[A]*[B] )
(i) If tripling the initial concentration of reactant A multiplies the initial rate by 27, calculate the order of the reaction with respect to A. i.e. solve for x. Show detailed workings.
(ii) Determine the overall order of the reaction Show how the answer was obtained
10. Consider the reaction showing the decomposition of C₂ H₅ Cl(g)
C₂H₅Cl(g) -> C₂H₄(g) + HCl(g)
The above reaction follows first-order kinetics with respect to C₂H₅Cl. The rate constant is
1.60 x 10-6-1 for the reaction conducted at 650 K. In an investigation of the decomposition of
C₂ H₅ Cl (g) it was found that it takes 87.0 hrs for the concentration of C₂ H₅ Cl to drop to 0.100 mol L ^-1
(a) Calculate the initial concentration of C₂H₅Cl. Show detailed workings
(b) Calculate the concentration of C₂H₅Cl after 125 hrs. Show detailed workings
(c) Calculate the time in hrs) that it will take for 75.0% of the C₂H₅Cl to decompose. Show detailed workings.

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