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- Nitric oxide reacts with hydrogen to release large amounts of chemiluminescence with the characteristics of the highly cytotoxic species. The following data were measured for the reaction of nitric oxide with hydrogen: Data number 1 2 3 2 NO(g) + 2 H₂(g) → N₂(g) + 2 H₂O(g) [NO] (M) 0.1 0.1 0.2 [H₂] (M) 0.1 0.2 0.1 Based on the data, (a) Determine the rate law for this reaction. (b) Calculate the rate constant. (c) Calculate the rate when [NO] = 0.050 M and [H₂] = 0.150 M Initial rate (M/S) 1.23 x 10-³ 2.46 x 10-³ 4.92 x 10-³1a) The decomposition of ethanol at some constant temperature (above 500°C), over a copper surface, C2H5OH(g)--> CH3CHO(g) + H2(g) was studied by monitoring the total pressure with time.The following data were obtained: t (s) Ptotal (torr) 0 120 45 131 139 154 233 177 376 212 380 213 What will be the total pressure at t = 462 s? 1b) What is the rate constant (k)?(Include appropriate units.)The maximum rate I at which oxygen molecules can be consumed by a bacterium or radius R in a lake where the concentration of oxygen is co = 0.2 mole m³ increases with the first power of R. We might expect the oxygen consumption, however, to increase roughly with an organism's volume. Together, this statements imply an upper limit to the size of a bacterium: If R gets too large, the bacterium would literally suffocate. The actual metabolic activity of a bacterium is about 0.02 mole kg-' sl. What limit do you then get on the size R of a bacterium? Compare to the size of a real bacteria. Can you think of some way for a bacterium to evade this limit?
- In a study of the gas phase decomposition of hydrogen iodide at 700 K HI(g)V½ H2(g) + ½ I½(g) the concentration of HI was followed as a function of time. It was found that a graph of 1/[HI] versus time in seconds gave a straight line with a slope of 1.72×103 M1s1and a y-intercept of 0.667 M1. Based on this plot, the reaction is order in HI and the rate constant for the reaction is M1s1Consider 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(a) Explain the meaning of the sentence:“The velocity laws of reactions are empirical” (b) It can be determined that the velocity law of a generic reaction A +B→Pév = k[A]x[B]y. Plot on a graph the variation of [A] and [P] with time, and explain why v= d[P]/dt = -d[A]/dt. (c) Explain the meaning of the terms k, x and y, in the velocity law, presented in item b: (d) Explain what it means in practice for a velocity law to be of zero order. Plot ,A as a function of t, for the zero-order reaction A→Products. (e) Explain what elementary reactions are and how they can be classified.
- Write the difference between order and molecularity of reaction.7) For the reaction CO(g) + 3 H2(g) = H2O(g) + CH4(g), Kc = 190 at 1000 K. If a vessel is filled with these gases such that the initial concentrations are [CO] = 0.036 M, [H2] = 0.045, [H2O] = 0.020, 7) %3D %3D %3D and [CH4] = 0.031, in which direction will a reaction occur and why? A) it is at equilibrium because Q = 190 B) toward products because Q = 4.1 C) toward reactants because Q = 0.24 D) toward products because Q = 0.38 %3D %3D %3D %3D E) toward reactants because Q = 61 %3D(a) The decomposition of a gas phase reactant, A, into gaseous products, P and Q, proceeds according to the reaction stoichiometry: A (g) P (g) + Q (g) and has been studied by measurement of the pressure increase in a constant volume system. Starting with an initial pressure of 112 torr of pure A at 713 K, the following total pressures, were measured at the times stated: Time (min) Pressure (Torr) | 136 15 30 45 60 75 155 170 181 191 (i) Give a suitable expression for the integrated rate equation by which the tabulated data can be analysed to confirm that the reaction exhibits first order kinetics. (ii) Calculate the rate constant and the half life of the reaction. (ii) If the activation energy of the reaction is given by 120 kJ mol, determine the rate constant and half life at a temperature of 1100 K.
- Suppose that the gas-phase reaction 2 NO(g) + O₂(g) →2 NO₂ (g) were carried out in a constant- volume container at constant temperature.Plot (x/m) versus P for the Freundlich adsorption isotherm Describe how does Freundlich isotherm varies at high pressure and low pressure conditions?Here is the correct statement for Qc and Kc for a certain reaction. Qc value is determined by the concentrations of reactants and products at a particular moment rather than by the temperature, but Kc value stays the same at a certain temperature regardless of the concentrations. For the following reaction at 20oC, the Qc value at a particular time is equal to 3.5 x 10‒5 3A(aq) + B(aq) ⟶ 2C(aq) + D(aq) Kc = 5.5 x 10‒5 If the reaction temperature is suddenly increased to 40oC without affecting the concentration of each component in the system, which of the following is a correct prediction about Qc and Kc at this particular time at 40oC? Q ≠ 3.5 x 10‒5, K = 5.5 x 10‒5 Q ≠ 3.5 x 10‒5, K ≠ 5.5 x 10‒5 Q = 3.5 x 10‒5, K ≠ 5.5 x 10‒5