Skip to main content
Ch.14 - Chemical Kinetics
Brown - Chemistry: The Central Science 14th Edition
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232당신이 사용하는 게 아니라요?교과서 변경
모든 교과서Brown 14th EditionCh.14 - Chemical Kinetics문제 48
14장, 문제 48

Consider the data presented in Exercise 14.20. (a) Determine whether the reaction is first order or second order.

검증된 단계별 안내
1
Step 1: Review the data from Exercise 14.20, which should include concentration and time information for the reaction. This data is crucial for determining the order of the reaction.
Step 2: Plot the concentration of the reactant versus time to visually inspect if the reaction follows a first-order or second-order kinetic model. For a first-order reaction, a plot of ln(concentration) versus time should yield a straight line.
Step 3: Alternatively, plot 1/concentration versus time. For a second-order reaction, this plot should yield a straight line.
Step 4: Calculate the slope of the line from the plot that appears linear. For a first-order reaction, the slope of the ln(concentration) versus time plot is equal to -k, where k is the rate constant. For a second-order reaction, the slope of the 1/concentration versus time plot is equal to k.
Step 5: Compare the linearity of the two plots to determine the order of the reaction. The plot that results in a straight line indicates the order of the reaction: first-order if ln(concentration) versus time is linear, and second-order if 1/concentration versus time is linear.

주요 개념

질문에 올바르게 답하기 위해 반드시 이해해야 하는 핵심 개념들은 다음과 같습니다.

Reaction Order

Reaction order refers to the power to which the concentration of a reactant is raised in the rate law of a chemical reaction. It indicates how the rate of reaction depends on the concentration of reactants. A first-order reaction depends linearly on the concentration of one reactant, while a second-order reaction depends on the square of the concentration of one reactant or the product of the concentrations of two reactants.
추천 영상:
가이드 코스
00:36
Average Bond Order

Rate Law

The rate law is an equation that relates the rate of a chemical reaction to the concentration of its reactants. It is typically expressed in the form Rate = k[A]^m[B]^n, where k is the rate constant, and m and n are the orders of the reaction with respect to reactants A and B, respectively. Analyzing the rate law helps determine the reaction order by examining how changes in concentration affect the reaction rate.
추천 영상:
가이드 코스
01:52
Rate Law Fundamentals

Integrated Rate Laws

Integrated rate laws provide a mathematical relationship between the concentration of reactants and time for different orders of reactions. For first-order reactions, the integrated rate law is ln[A] = -kt + ln[A]₀, while for second-order reactions, it is 1/[A] = kt + 1/[A]₀. By plotting concentration data over time and analyzing the resulting graphs, one can determine the order of the reaction based on which plot yields a straight line.
추천 영상:
가이드 코스
01:52
Rate Law Fundamentals
관련 실천
교과서 질문

From the following data for the first-order gas-phase isomerization of CH3NC at 215 C, calculate the firstorder rate constant and half-life for the reaction: Time (s) Pressure CH3nC (torr) 0 502 2000 335 5000 180 8000 95.5 12,000 41.7 15,000 22.4

1191
views
교과서 질문

The gas-phase decomposition of NO2, 2 NO2(g) → 2 NO(g) + O2(g), is studied at 383°C, giving the following data:

Time (s) [NO2] (M)

0.0 0.100

5.0 0.017

10.0 0.0090

15.0 0.0062

20.0 0.0047 

(a) Is the reaction first order or second order with respect to the concentration of NO2?

(c) Predict the reaction rates at the beginning of the reaction for initial concentrations of 0.200 M, 0.100 M, and 0.050 M NO2.

1744
views
교과서 질문

Consider the data presented in Exercise 14.19. (a) By using appropriate graphs, determine whether the reaction is first order or second order.

교과서 질문

Consider the data presented in Exercise 14.19. (c) What is the half-life for the reaction?

724
views
교과서 질문

Sucrose 1C12H22O112, commonly known as table sugar, reacts in dilute acid solutions to form two simpler sugars, glucose and fructose, both of which have the formula C6H12O6. At 23 C and in 0.5 M HCl, the following data were obtained for the disappearance of sucrose: Time (min) 3C12H22o11 4 1M2 0 0.316 39 0.274 80 0.238 140 0.190 210 0.146 (a) Is the reaction first order or second order with respect to 3C12H22O114?

2567
views