Consider that for the decomposition reaction of acetaldehyde: CH,CHO →) CH,+CO The following mechanism is proposed: CH3CHO * CH3+CHO CH3 + CH3CHO CH4+CH3CO K CH3CO CO+CH3 2CH34C₂H6 Using the steady state method and the CO concentration as a starting point, answer the following questions: a) What is the total reaction order? b) What is the value of the observed rate constant with the rate constants of the steps of the proposed mechanism?

The decomposition of ammonia is zero order process is with a half-life of 28.3 seconds at a certain temperature. If the pertinent rate constant is 0.00207 M.s1, what was the initial reactant concentration? The half-life of a zero-order reaction is concentration-independent (A) (B) (C) (D) (E) 17.1 M 0.0353 M 0.00207 M 0.117 M

The decomposition reaction of ammonia gas (NH3) into hydrogen gas (H2) and nitrogen (N2) with a Pt catalyst is a zero order reaction at a temperature of 1130 K (i) rate of reaction = rate constant,(ii) reaction rate depends on ammonia concentration,(iii) the rate of decomposition of ammonia becomes constant when the ammonia has completely reacted,(iv) an increase in gas pressure will change the rate of the reaction. A. (ii) and (iv)B. (i) and (ii)C. (i), (ii) and (iii)D. (ii), (iii) and (iv)E. (i), (iii) and (iv)

Nitrification is a biological process for removing NH3 from wastewater as NH4+: NH, +20, → NO3 + 2H + H2O The first-order rate constant is given as k₁ = 0.47e0.095(T-15°C) where k₁ is in day¹ and T is in °C. If the initial concentration of NH3 is 3.0 mol/m³, how long will it take to reduce the concentration to 0.66 mol/m³: (a) in the spring (T = 20°C)? days (b) in the winter (T = 10°C)? days