The combustion of ammonia is shown below: 4NH:(g) + 50:(g) → 4NO(g) + 6H;O(g) Write an equation that relates the rates of consumption of the reactants and the rates of formation of the products. (i) At 298 °C, the rate of reaction (v) is 2.7 x 10 mol L-'s. Find the rate change of NH3, O2, NO and H;O. (ii)

The reaction C,H¿(g) 2C,H,(g) has an activation energy of 262 kJ/mol. At 600.0 K, the rate constant, k, is 6.1 x 10-8 s-!. What is the value of the rate constant at 770.0 K? k = * TOOLS х10

The reaction 2 NO(g) + O2(g) --> 2 NO2(g) proceeds through the following mechanism: 2 NO(g) --> N2O2(g)N2O2(g) + O2(g) --> 2 NO2(g) (a) The second step of this mechanism is rate-determining (slow). What is the rate law for this reaction? Rate = k [NO] [O2] Rate = k [NO]2 [O2]     Rate = k [NO] [O2]2 Rate = k [NO]1/2 [O2] Rate = k [NO] [O2]1/2 Rate = k [NO]2 Rate = k [NO]2 [O2]1/2 (b) What would the rate law be if the first step of this mechanism were rate-determining? Rate = k [NO] [O2] Rate = k [NO]2 [O2]     Rate = k [NO] [O2]2 Rate = k [NO]1/2 [O2] Rate = k [NO] [O2]1/2 Rate = k [NO]2 Rate = k [NO]2 [O2]1/2 Rate = k [NO]

The reaction described by the equation O3 (g) + NO(g) 0,(g) + NO,(g) has, at 310 K, the rate law rate of reaction = k[O¸][NO] k = 3.0 x 106 M-1-s-! Given that [O,] = 8.0 x 10-4 M and [NO] = 3.0 x 10-3 M at t = :0, calculate the rate of the reaction at t = 0. rate: M/s What is the overall order of this reaction? 3

1a)  A(g) + B(g)  C(g) The rate law for the above reaction is: -d[A]/dt = k[A][B] The rate constant is 1.13×102 L mol-1 s-1 at 346.0°C and 3.55×103 L mol-1 s-1 at 548.0°C. Use the Arrhenius equation k = Ae-Ea/RT to: Calculate Ea for this reaction. 1b) Calculate the rate constant k at 416.0°C for this reaction. 1c) Calculate the pre-exponential factor A for this reaction.

(a) Consider the combustion of ammonia, given below: 4 NH3(g) + 5 O2(g)  --------> 4 NO(g) + 6 H2O(g) If NH3(g) is decreasing at the rate of 0.130 mol/s, what are the rates of change of O2(g), NO(g), and H2O(g)?O2(g)/t =  _____ mol/s

Consider the following reaction in aqueous solution: 5Br-(aq) +BrO3-(aq) +6H+(aq)→ 3Br2(aq) + 3H2O(l) If the rate of disappearance of Br–(aq) at a particular moment during the reaction is 2.5 x 10–4 mol L–1 s–1, what is the rate of appearance of Br2(aq) at that moment?   Question 2 options:   a)  2.1 x 10–4 mol L–1 s–1   b)  1.5 x 10–4 mol L–1 s–1   c)  7.2 x 10–4 mol L–1 s–1   d)  9.4 x 10–4 mol L–1 s–1