8. If, for the reaction aX + bY → products, the rate law is determined to be r = k[X]'[Y]², then the overall order of reaction is а. 1 d. 4 b. 2 e. С. 3 f.
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![8. If, for the reaction ax + bY
products, the rate law is determined to be r=
K[X]'[Y]², then the overall
order of reaction is
a.
1
d. 4
b. 2
е.
f. 6
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- 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 10‒5If the volume of a container for the reaction A+2B=C is suddenly reduced to ½ its original volume with the moles of A, B and C maintained constant, the rate will increase by a factor ofA. 2B. 4C. 8D. 16Please help me find the value of k' p= -1.41 q= -0.2 Substitution of p and q into rate law. Use the values of p and q (from Part C) and the rate law, rate = ∆(mol I2)/∆t = k ́ [I–]p [H2 O2 ]q, to determine k ́ for the solutions.
- 25) Consider the following set of reactions. Assume that A, B, C and D are atoms. (1) A + A → B (2) А-В + С-D А-С-D-B (3) A + B-C → A-B-C Order these reactions in terms of increasing significance of the orientation probability (that is the A in the Arrhenius equation). А. (1) (2) < (3) В. (3) < (2) <(1) C. (1) < (3) <(2) D. (1) = (2) = (3) E. (1) < (2) = (3)Write down the kinetic equation for a simple reaction in a homogeneous medium 2A + B = 2C. Indicate the general and in relati on to all reactants reaction orders7) 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) 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.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?The rate law for the reaction A + 3B → 2C + D was found to be v = k[A]2[B]2. (a) What are the units of k? (b) Express the rate law in terms of the rates of formation and consumption of A and C, respectively.
- 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 M1s1Derive the integrated form of a third-order rate law v = kr[A]2[B] in which the stoichiometry is 2 A + B → P and the reactants are initially present in (a) their stoichiometric proportions ([B]0 = 12[A]0); (b) with B present initially in twice that amount ([B]0 = [A]0). Express your rate law in terms of [A]0, [B]0, and x, where [A] = [A]0 − 2x.naction quotient Qc ,and the equi librium cons tant follo wing Write the Ke, for each the reactions. of 2CoH 8(G) +1003(9) → 6CO2G) +8H 20 (9)