Chem 211 1st Edition Lecture 10Outline of Last Lecture I. Osmotic PressureII. Volatile Nonelectrolyte SolutionsIII. Strong Electrolyte SolutionsIV. Colligative Properties of Electrolyte SolutionsV. Non-ideal behavior of strong electrolyte solutionsOutline of Current Lecture I. Factors That Influence Reaction RateII. Expressing the Reaction RateIII. The Rate LawIV. Reaction OrdersV. Individual and Overall Reaction OrdersCurrent LectureI. Factors That Influence Reaction RateA. Particles must collide in order to react.B. The higher the concentration of reactants; the greater the reaction rate.C. A higher concentration of reactant particles allows a greater number of collisions.D. The physical state of the reactants influences reaction rate.E. Substances must mix in order for particles to collide.F. The higher the temperature, the greater the reaction rate.G. At higher temperatures particles have more energy and therefore collide more often andmore effectively.H. Sufficient collision energy is required for areaction to occur.II. Expressing the Reaction RateA. Reaction rate is measured in terms of the changes in concentrations of reactants or products per unit time.B. For the general reaction A → B, we measure the concentration of A at t1 and at t2:C. Square brackets indicate a concentration in moles per literThese notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute.D. The negative sign is used because the concentration of A is decreasing. This gives the rate a positive value.III. The Rate LawA. For any general reaction occurring at a fixedtemperatureB. aA + bB → cC + dDC. The term k is the rate constant, which is specific for a given reaction at a given temperature.D. The exponents m and n are reaction orders and are determined by experiment.E. The values of m and n are not necessarily related in any way to the coefficients a and b.IV. Reaction OrdersA. A reaction has an individual order “with respect to” or “in” each reactant.B. For the simple reaction A → productsC. If the rate doubles when [A] doubles, the rate depends on [A]1 and the reaction is first order with respect to A.D. If the rate quadruples when [A] doubles, the rate depends on [A]2 and the reaction is second order with respect to [A].E. If the rate does not change when [A] doubles, the rate does not depend on [A], and the reaction is zero order with respect to A.V. Individual and Overall Reaction OrdersA. For the reaction 2NO(g) + 2H2(g) → N2(g) + 2H2O(g):B. The rate law is rate = k[NO]2[H2]C. The reaction is second order with respect to NO, first order with respect to H2 and third order overall.D. Note that the reaction is first order with respect to H2 even though the coefficient for H2in the balanced equation is 2.E. Reaction orders must be determined from experimental data and cannot be deduced from the balanced