Rate Laws Quiz

PDF page 676: As described in the previous module, the rate of a reaction is often affected by the concentrations of reactants. Rate laws (sometimes called differential rate laws) or rate equations are mathematical expressions that describe the relationship between the rate of a chemical reaction and the concentration of its reactants. As an example, consider the reaction described by the chemical equation aA + bB ⟶ products where a and b are stoichiometric coefficients. The rate law for this reaction is written as: m n rate = k[A] [B] in which [A] and [B] represent the molar concentrations of reactants, and k is the rate constant, which is specific for a particular reaction at a particular temperature. The exponents m and n are the reaction orders and are typically positive integers, though they can be fractions, negative, or zero. The rate constant k and the reaction orders m and n must be determined experimentally by observing how the rate of a reaction changes as the concentrations of the reactants are changed. The rate constant k is independent of the reactant concentrations, but it does vary with temperature. The reaction orders in a rate law describe the mathematical dependence of the rate on reactant concentrations. Referring to the generic rate law above, the reaction is m order with respect to A and n order with respect to B. For example, if m = 1 and n = 2, the reaction is first order in A and second order in B. The overall reaction order is simply the sum of orders for each reactant. For the example rate law here, the reaction is third order overall (1 + 2 = 3). A few specific examples are shown below to further illustrate this concept. The rate law:

PDF page 676: As described in the previous module, the rate of a reaction is often affected by the concentrations of reactants. Rate laws (sometimes called differential rate laws) or rate equations are mathematical expressions that describe the relationship between the rate of a chemical reaction and the concentration of its reactants. As an example, consider the reaction described by the chemical equation aA + bB ⟶ products where a and b are stoichiometric coefficients. The rate law for this reaction is written as: m n rate = k[A] [B] in which [A] and [B] represent the molar concentrations of reactants, and k is the rate constant, which is specific for a particular reaction at a particular temperature. The exponents m and n are the reaction orders and are typically positive integers, though they can be fractions, negative, or zero. The rate constant k and the reaction orders m and n must be determined experimentally by observing how the rate of a reaction changes as the concentrations of the reactants are changed. The rate constant k is independent of the reactant concentrations, but it does vary with temperature. The reaction orders in a rate law describe the mathematical dependence of the rate on reactant concentrations. Referring to the generic rate law above, the reaction is m order with respect to A and n order with respect to B. For example, if m = 1 and n = 2, the reaction is first order in A and second order in B. The overall reaction order is simply the sum of orders for each reactant. For the example rate law here, the reaction is third order overall (1 + 2 = 3). A few specific examples are shown below to further illustrate this concept. The rate law:

PDF page 676: As described in the previous module, the rate of a reaction is often affected by the concentrations of reactants. Rate laws (sometimes called differential rate laws) or rate equations are mathematical expressions that describe the relationship between the rate of a chemical reaction and the concentration of its reactants. As an example, consider the reaction described by the chemical equation aA + bB ⟶ products where a and b are stoichiometric coefficients. The rate law for this reaction is written as: m n rate = k[A] [B] in which [A] and [B] represent the molar concentrations of reactants, and k is the rate constant, which is specific for a particular reaction at a particular temperature. The exponents m and n are the reaction orders and are typically positive integers, though they can be fractions, negative, or zero. The rate constant k and the reaction orders m and n must be determined experimentally by observing how the rate of a reaction changes as the concentrations of the reactants are changed. The rate constant k is independent of the reactant concentrations, but it does vary with temperature. The reaction orders in a rate law describe the mathematical dependence of the rate on reactant concentrations. Referring to the generic rate law above, the reaction is m order with respect to A and n order with respect to B. For example, if m = 1 and n = 2, the reaction is first order in A and second order in B. The overall reaction order is simply the sum of orders for each reactant. For the example rate law here, the reaction is third order overall (1 + 2 = 3). A few specific examples are shown below to further illustrate this concept. The rate law:

PDF page 676: As described in the previous module, the rate of a reaction is often affected by the concentrations of reactants. Rate laws (sometimes called differential rate laws) or rate equations are mathematical expressions that describe the relationship between the rate of a chemical reaction and the concentration of its reactants. As an example, consider the reaction described by the chemical equation aA + bB ⟶ products where a and b are stoichiometric coefficients. The rate law for this reaction is written as: m n rate = k[A] [B] in which [A] and [B] represent the molar concentrations of reactants, and k is the rate constant, which is specific for a particular reaction at a particular temperature. The exponents m and n are the reaction orders and are typically positive integers, though they can be fractions, negative, or zero. The rate constant k and the reaction orders m and n must be determined experimentally by observing how the rate of a reaction changes as the concentrations of the reactants are changed. The rate constant k is independent of the reactant concentrations, but it does vary with temperature. The reaction orders in a rate law describe the mathematical dependence of the rate on reactant concentrations. Referring to the generic rate law above, the reaction is m order with respect to A and n order with respect to B. For example, if m = 1 and n = 2, the reaction is first order in A and second order in B. The overall reaction order is simply the sum of orders for each reactant. For the example rate law here, the reaction is third order overall (1 + 2 = 3). A few specific examples are shown below to further illustrate this concept. The rate law:

PDF page 676: As described in the previous module, the rate of a reaction is often affected by the concentrations of reactants. Rate laws (sometimes called differential rate laws) or rate equations are mathematical expressions that describe the relationship between the rate of a chemical reaction and the concentration of its reactants. As an example, consider the reaction described by the chemical equation aA + bB ⟶ products where a and b are stoichiometric coefficients. The rate law for this reaction is written as: m n rate = k[A] [B] in which [A] and [B] represent the molar concentrations of reactants, and k is the rate constant, which is specific for a particular reaction at a particular temperature. The exponents m and n are the reaction orders and are typically positive integers, though they can be fractions, negative, or zero. The rate constant k and the reaction orders m and n must be determined experimentally by observing how the rate of a reaction changes as the concentrations of the reactants are changed. The rate constant k is independent of the reactant concentrations, but it does vary with temperature. The reaction orders in a rate law describe the mathematical dependence of the rate on reactant concentrations. Referring to the generic rate law above, the reaction is m order with respect to A and n order with respect to B. For example, if m = 1 and n = 2, the reaction is first order in A and second order in B. The overall reaction order is simply the sum of orders for each reactant. For the example rate law here, the reaction is third order overall (1 + 2 = 3). A few specific examples are shown below to further illustrate this concept. The rate law:

PDF page 676: rate = k⎣H O ⎦ 2 2 describes a reaction that is first order in hydrogen peroxide and first order overall. The rate law:

PDF page 676: rate = k⎣C H ⎦ 4 6 describes a reaction that is second order in C4H6 and second order overall. The rate law:

PDF page 677: describes a reaction that is first order in H , first order in OH , and second order overall.

PDF page 677: + − rate = k[H ][OH ]

PDF page 677: An experiment shows that the reaction of nitrogen dioxide with carbon monoxide: NO (g) + CO(g) ⟶ NO(g) + CO (g) 2 2 is second order in NO2 and zero order in CO at 100 °C. What is the rate law for the reaction? Solution The reaction will have the form: m n rate = k[NO ] [CO] 2 The reaction is second order in NO2; thus m = 2. The reaction is zero order in CO; thus n = 0. The rate law is: 0 2 2

PDF page 677: rate = k[NO ] [CO] = k[NO ]

PDF page 677: Remember that a number raised to the zero power is equal to 1, thus [CO] = 1, which is why the CO concentration term may be omitted from the rate law: the rate of reaction is solely dependent on the concentration of NO2. A later chapter section on reaction mechanisms will explain how a reactant’s concentration can have no effect on a reaction rate despite being involved in the reaction. Check Your Learning The rate law for the reaction: H (g) + 2NO(g) ⟶ N O(g) + H O(g) 2 2 2 2

PDF page 677: has been determined to be rate = k[NO] [H2]. What are the orders with respect to each reactant, and what is the overall order of the reaction?

PDF page 677: Answer: order in NO = 2; order in H2 = 1; overall order = 3

PDF page 677: rate = k⎣CH OH⎦ 3 What is the order of reaction with respect to methanol and ethyl acetate, and what is the overall order of reaction?

PDF page 677: Answer: order in CH3OH = 1; order in CH3CH2OCOCH3 = 0; overall order = 1