Suppose it is known that ozone adsorbs on a certain surface in accord with a Langmuir isotherm. How could you use the pressure dependence of the fractional coverage to distinguish between adsorption (i) without dissociation, (ii) with dissociation into O + O2, (c) with dissociation into O + O + O?

In a study of the decomposition of ammonia on a platinum surface at 856 °C NH31/2 N2 + 3/2 H2 the following data were obtained: NH3], M 2.39x10-3 1.20×103 997 6.00x104 1.50x103 3.00x10-4 1.75x103 seconds Hint: It is not necessary to graph these data. (1) The observed half life for this reaction when the starting concentration is 2.39x10-3 M is s and when the starting concentration is 1.20×10-3 M is s. (2) The average rate of disappearance of NH3 from t= 0 s to t= 997 s is Ms!. (3) The average rate of disappearance of NH3 from t= 997 s to t= 1.50×103 s is M s-l. (4) Based on these data, the rate constant for this | order reaction is M s-1.

In a study of the gas phase decomposition of nitrogen dioxide at 383 °C NO₂(g) →→→NO(g) + ½ O₂(g) the concentration of NO₂ was followed as a function of time. It was found that a graph of 1/[NO₂] versus time in seconds gave a straight line with a slope of 0.815 M-¹ s¹ and a y-intercept of 11.5 M-¹. Based on this plot, the reaction is [ ✓order in NO₂ and the rate constant for the reaction is M-¹ S-¹.

Consider the following gas phase reaction at constant volume: 2CH2N2(g) −→ 2N2(g) + C2H4(g) i) Given that the initial pressure is p0 calculate the total pressure after three quarters of the CH2N2(g) has reacted. ii) Derive an equation which shows how the total pressure varies as a function of the fraction, α, of the CH2N2(g) that has reacted. iii) Sketch a graph which shows how the pressure varies as a function of α

In a study of the gas phase decomposition of sulfuryl chloride at 600 KSO2Cl2(g)SO2(g) + Cl2(g)the concentration of SO2Cl2 was followed as a function of time.It was found that a graph of ln[SO2Cl2] versus time in minutes gave a straight line with a slope of -4.28×10-3 min-1 and a y-intercept of -6.95 . Based on this plot, the reaction is________. (firest, zero, or second) order in SO2Cl2 and the rate constant for the reaction is min-1.

Calculate the initial rate for the formation of C at 25 ∘C, if [A]=0.50M and [B]=0.075M Express your answer to two significant figures and include the appropriate units.

Suppose the reduction of nitric oxide proceeds by the following mechanism: step elementary reaction rate constant 1 H,(g) + 2 NO(g) → N,0(g) + H,0(g) k1 2 H2(9) + N,0(9) → N2(9) + H,O(g) Suppose also k, «k,. That is, the first step is much slower than the second. Write the balanced chemical equation for the overall chemical reaction: Write the experimentally- observable rate law for the overall chemical reaction. rate = k U Note: your answer should not contain the concentrations of any intermediates. Express the rate constant k for the overall chemical reaction in terms of k1, k2, and (if necessary) the rate constants k.1 and k-2 for k = the reverse of the two elementary reactions in the mechanism.

The specific rate constant for the first-order decomposition of -1 N₂O5 (9) to NO2 (g) and O₂ (g) is 7.48 × 10-³ s¯ at a given temperature. Find the length of time required for the total pressure in a system containing N₂O5 at an initial pressure of 0.110 atm to rise to 0.150 atm . Express your answer using two significant figures. VE ΑΣΦ t = Submit Part B t = Submit Request Answer Find the length of time required for the total pressure in a system containing N₂O5 at an initial pressure of 0.110 atm to rise to 0.220 atm . Express your answer using two significant figures. ΨΕ ΑΣΦ Part C Request Answer ? Find the total pressure after 120 s of reaction. S S

The Arrhenius parameters for the gas-phase decomposit ion of cyclobutane, C4H8(g)→ 2 C2H4(g). are log(A/s-1) = 15.6 and Ea = 261 kJ mol- 1. What is the ha lf- life of cyclobutane at (a) 20 °C, (b) 500 °C?

Consider the chemical reaction described by 2A(aq) ⇌ D(aq)with rate constants k1 and k-1.  If the reaction is subject to a temperature jump, derive the equation for d[D]/dt in terms of a relaxation constant t.