Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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- 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 =arrow_forwardFor 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] tarrow_forwardPlease don't provide handwritten solution ....arrow_forward
- 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 = 0arrow_forwardA 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] 2arrow_forwardFor 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]²arrow_forward
- 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.arrow_forwardIn 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.arrow_forwardThe 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]arrow_forward
- 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 =arrow_forwardKinetic 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 Darrow_forwardFrom the data given in the table below, determine the rate law for the following chemical equation. NH4+(aq) + NO2-(aq) → N2(g) + 2 H2O(l) Experiment [NH4+]o [NO2-]o Initial Rate (consumption of NH4+) 1 0.24 0.10 7.2 x 10-6 M/s 2 0.12 0.10 3.6 x 10-6 M/s 3 0.12 0.15 5.4 x 10-6 M/s Select one: a. Rate = k[NH4+][NO2-]2 b. Rate = k[NH4+]2[NO2-] c. Rate = k[NH4+]2 d. Rate =k[NH4+]2[NO2-]2 e. Rate = k[NO2-] f. Rate = k[NO2-]2 g. Rate = k[NH4+] h. Rate = k[NH4+][NO2-]arrow_forward
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