The reaction A → C was performed and the concentration vs. time data below collected. time, s 0 3 [A], mol/L 1 2 5 6 7 8 0.7983 0.1898 0.1077 0.07517 0.05774 0.04687 0.03944 Complete the rate law for the reaction by filling in the values for the rate constant and reaction order. Rate = K[A]* rate constant (without units) = reaction order = 0.03405 0.0299 A least squares line gives the best straight- line fit through any set of points but to get the right answer you need to figure out which plot gives the straight line.

The reaction A → C was performed and the concentration vs. time data below collected. time, s 0 3 [A], mol/L 1 2 5 6 7 8 0.7983 0.1898 0.1077 0.07517 0.05774 0.04687 0.03944 Complete the rate law for the reaction by filling in the values for the rate constant and reaction order. Rate = K[A]* rate constant (without units) = reaction order = 0.03405 0.0299 A least squares line gives the best straight- line fit through any set of points but to get the right answer you need to figure out which plot gives the straight line.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Some measurements of the initial rate of a certain reaction are given in the table below. [N] N2 H, initial rate of reaction 1.89M |0.180M 0.848 M/s 1.89М |0.686M 12.3 M/s 0.689M| 0.180M 0.113 M/s Use this information to write a rate law for this reaction, and calculate the value of the rate constant k. Round your value for the rate constant to 3 significant digits. Also be sure your answer has the correct unit symbol. rate = k|| х10 k =
For A products, time and concentration data were collected and plotted as shown. [A] (M) t (s) 0.900 00.0 0.474 30.0 0.321 60.0 0.243 90.0 t Determine the reaction order, the rate constant, and the units of the rate constant. order= *k = [A] MacBook Pro In[A] t (units) 1/[A] t
Please don't provide handwritten solution ....
Some measurements of the initial rate of a certain reaction are given in the table below. alo N2| |H2 initial rate of reaction 0.875 M 1.32M 0.0545 M/s 0.875 M 0.342M 0.0141 M/s 3.25 M 1.32 M 0.752 M/s Use this information to write a rate law for this reaction, and calculate the value of the rate constant k. Round your value for the rate constant to 3 significant digits. Also be sure your answer has the correct unit symbol. rate = k O k = 0
A kinetics experiment was conducted based on the reaction: 2NO + H2 - N20 + H20 Use the following data from the experiment to determine the rate law for the reaction. Expt. # Initial rate 1.46 M/min INO]. [H:]0 1 0.021 0.065 2 0.021 0.260 1.46 M/min 3 0.042 0.065 5.84 M/min rate = k[NO] 2[H 2) 2 rate = k[NO] rate = k[NO] 2[H 2] rate = k[NO][H 2] rate = k[NO] 2
For the chemical reaction NO2(g) + CO(g) → NO(g) + CO2(g) The following initial rate data were obtained Initial [NO₂] Initial [CO] Initial Rate Experiment (mol/L) (mol/L) (mol/L.s) 1 0.10 0.10 0.0050 2 0.40 0.10 0.080 3 0.10 0.20 0.0050 What is the rate law for the reaction? R = k [NO₂]4[CO] R = k [NO₂][CO] R = k [NO₂]²[CO] none of the answers are correct OR = K [NO₂]²
38. Time and concentration data were collected for the reaction A → B. t (s) [A] (M) 0.600 30.0 0.484 60.0 0.405 90.0 0.349 a. Determine the reaction order with respect to A. b. Calculate the rate constant for the reaction. 0.00
Initial rates were measured for the following reaction and are listed in the table. A + 2B ⎯→ products Expt. Initial Concentrations Initial Rate (mol/L·s) [A] [B] 1 0.115 0.135 2.70 × 10−3 2 0.115 0.270 2.16 × 10−2 3 0.345 0.135 8.10 × 10−3 Determine the rate law for the reaction including the value of the rate constant with the correct units.
In a study of the gas phase decomposition of dinitrogen pentoxide at 335 K N2O5(g) 2 NO2(g) + ½ O2(g) the concentration of N2O5 was followed as a function of time. It was found that a graph of In[N,05] versus time in seconds gave a straight line with a slope of -6.82x103 s and a y-intercept of -2.58 . Based on this plot, the reaction is first order in N205 and the half life for the reaction is seconds.
The data below were collected for this reaction: CH3Cl (g) + 3 Cl2(g) → CCl4 (g) + 3 HCl (g) Expt. [CH3Cl] (M) [Cl2] (M) Initial Rate (M/s) 1 0.050 0.050 0.014 2 0.100 0.050 0.029 3 0.100 0.100 0.057 Provide the rate law for this reaction. Include the numerical value of the specific rate constant, k. Rate = - Δ [Cl2]3 / Δ t Rate = Δ [HCl] / 3 Δ t Rate = k [CH3Cl] [Cl2]2 Rate = -Δ [CH3Cl] / 3 Δ t Rate = 5.7 [CH3Cl] [Cl2]
Some measurements of the initial rate of a certain reaction are given in the table below. [N:] N2| |H2| initial rate of reaction 0.768 M 2.48M 0.0363 M/s 0.768 M 0.466M 0.00128M/s 0.209M 2.48M 0.00988 M/s Use this information to write a rate law for this reaction, and calculate the value of the rate constant k. Round your value for the rate constant to 3 significant digits. Also be sure your answer has the correct unit symbol. rate = k ||| x10 k =
Kinetic data are normally presented as graphs. The following questions test your knowledge about labeling and interpreting graphs correctly. [B] is used to represent the concentration of a reactant B in a reaction. y y LLLE 44 X X B с Decide if each of the following statements is True or False. y A y Consider graph D: if y = 1/[B] and x = time, the graph could represent a first order reaction. Consider graph A: if y = [B] and x = time, the graph could represent a first order reaction. ✓Consider graph C: if y = In[B] and x = time, the graph could represent a second order reaction. ✓Consider graph C: if y = [B] and x = time, the graph could represent a zero order reaction. ✓Consider graph D: if y = 1/[B] and = time, the slope is equal to -k. ✓ Consider graph B: if y = [B] and x = time, the graph could represent a second order reaction. X D