The following data may be used for the questions that follow: NH 3(g) + BF 3(g) →F 3BNH 3(s). Experiment [BF3] [NH3](M) Initial Rate (M/s) 1 0.250 0.250 0.2130 0.250 0.125 0.1065 0.200 0.100 0.0682 4 0.350 0.100 0.1193 0.175 0.100 0.0596 Based on the data in the preceding table, what is the reaction order with respect to NH 3? Zero order First order Second order Cannot be determined QUESTION 2 Click Save and Submit to save and submit. Click Save All Answers to save all answers. 3.

The following data may be used for the questions that follow: NH 3(g) + BF 3(g) →F 3BNH 3(s). Experiment [BF3] [NH3](M) Initial Rate (M/s) 1 0.250 0.250 0.2130 0.250 0.125 0.1065 0.200 0.100 0.0682 4 0.350 0.100 0.1193 0.175 0.100 0.0596 Based on the data in the preceding table, what is the reaction order with respect to NH 3? Zero order First order Second order Cannot be determined QUESTION 2 Click Save and Submit to save and submit. Click Save All Answers to save all answers. 3.

Chemistry & Chemical Reactivity

9th Edition

ISBN:9781133949640

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter14: Chemical Kinetics: The Rates Of Chemical Reactions

Section14.1: Rates Of Chemical Reactions

Problem 2RC: 2. Use the graph provided in Example 14.1 to estimate the average rate of disappearance of dye for...

See similar textbooks

Similar questions

2AB2(g) = A2(g) + 2B2(g) A 500,0 ml ask is filled with 0,384 mol of AB2. the appearance of A2 is monitored at timed intervals. assume that temprature and volume are kept constant. the data obtained are shown in the table below. time/min : 0 10 20 30 40 50 moles of A2 : 0 0,0541 0,0833 0,1221 0,1432 0,1567 a. make a similiar table for the dissapearance of AB2 b. what is the average rate of dissapearance of AB2 over the second and the third 10 minutes intervals? c. what is the average rate of appearance of A2 between t=30 and t=50?
For the gas phase decomposition of dinitrogen pentoxide at 335 K 2 N₂05 4 NO2 + O2 the following data have been obtained: [N₂05], M time, s 0.175 0 Submit Answer 9.06x10-2 140 4.69x10-2 280 2.43x10-2 420 The average rate of disappearance of N₂O5 over the time period from t = 280 s to t = 420 s is
If Δ[Br2]ΔtΔ[Br2]Δ� = 4.7×10−6 M/sM/s , what is the value of Δ[ClO−2]ΔtΔ[ClO2−]Δ� during the same time interval? Express your answer to two significant figures and include the appropriate units. What is the average rate of consumption of Br−Br− during the same time interval? Express your answer to two significant figures and include the appropriate units.
how we can calculate the actual dissolved Oxygen concentration (cL) in oxygen transfer rate (OTR) formula .whenwe have cL than we can calculate the KLa value we find OTR from graph slope . cS =468/(31.6+T) T= 23 KLa = OTR/(cL- cS) cS = oxygen saturation concentration time(h) Dissolved oxygen(mg/l) 3.264 4.326 3.2818 3.697 3.29537 3.674 3.31445 3.268 3.33385 2.858 3.35218 2.475 3.37633 1.994 3.42174 1.15 3.4376 0.89 3.48951 0.249 3.54265 0.028
Calcium oxide, an important ingredient in cement, is produced by decomposing calcium carbonate at high temperature: CaCO3(s) → CaO(s) + CO2(g) In one reaction, 3.9 kg of calcium carbonate is heated at 589 °C in a 20.0-L vessel. The pressure of CO2 is 0.18 bar after 6.5 minutes. question 1. What is the average rate of CO2 production in mol/min during the 6.5-minute interval? question 2. How many moles of calcium carbonate consumed in the 6.5-minute interval?
Consider the following complex reaction: A + 2B → C whose initial rate at 25 °C was measured using three different sets of initial concentrations as listed in the following table: Trial [A](M) [B](M) Rate(M/s) 1 0.400 0.050 9.60 × 10−3 2 0.400 0.100 1.92 × 10−2 3 0.800 0.050 3.84 × 10−2 A) Write the rate law for this reaction. Use k to represent the rate constant. B) Solve for k in the above rate law. Express your answer to three significant figures. Include units for k.
Determine the average rate of change of BB from ?=0 st=0 s to ?=272 s.t=272 s. A⟶2BA⟶2B Time (s) Concentration of A (M) 0 0.7300.730 136136 0.4450.445 272272 0.1600.160 rateB= __________M/s
Nitric Oxide, NO , reacts with hydrogen to give nitrous oxide, N2O, and water. 2NO(g) +H2(g) → N2O(g) + H2O(g) In a series of experiments, the following initial rates of disappearance of NO were obtained: Expriment Initial Conc. of NO Initial Conc. of H2 Initial Rate Exp. 1 6.4x10-3 M 2.2x10-3 M 2.6x10-5 M/s Exp. 2 12.8x10-3 M 2.2x10-3 M 1.0x10-4 M/s Exp. 3 6.4x10-3 M 4.5x10-3 M 5.1x10-5 M/s What is the value of the rate constant for the reaction? Express your answer to three significant figures. Just enter the number (e.g. 2.48x10^-4) and the unit.
Nitric Oxide, NO , reacts with hydrogen to give nitrous oxide, N2O, and water. 2NO(g) +H2(g) → N2O(g) + H2O(g) In a series of experiments, the following initial rates of disappearance of NO were obtained: Expriment Initial Conc. of NO Initial Conc. of H2 Initial Rate Exp. 1 6.4x10-3 M 2.2x10-3 M 2.6x10-5 M/s Exp. 2 12.8x10-3 M 2.2x10-3 M 1.0x10-4 M/s Exp. 3 6.4x10-3 M 4.5x10-3 M 5.1x10-5 M/s What is the rate law for the reaction? Input the answer in the form rate = k[A]2[B]
Hello, I am having trouble with this lab question. 3. Calculate the rate for 40 years (from 1980 to 2020) – change of the rate in a year.( Y2-Y1) / (X2-X1) = (CO2_end – CO2_begin) / (Yearend – Yearbegin)What is the rate? Im not sure if I am doing it correctly ( 412.46 - 338.91) 40 years - 0 ? year mean 1980 338.91 1981 340.11 1982 340.86 1983 342.53 1984 344.08 1985 345.55 1986 346.96 1987 348.68 1988 351.16 1989 352.79 1990 354.05 1991 355.39 1992 356.1 1993 356.83 1994 358.33 1995 360.18 1996 361.93 1997 363.05 1998 365.7 1999 367.8 2000 368.98 2001 370.57 2002 372.59 2003 375.14 2004 376.95 2005 378.97 2006 381.13 2007 382.9 2008 385.01 2009 386.5 2010 388.76 2011 390.64 2012 392.65 2013 395.39 2014 397.34 2015 399.65 2016 403.09 2017 405.22 2018 407.61 2019 410.07 2020 412.46
An unknown gas, D, reacts with fluorine gas to form the compound DF4 (g), as represented by the following equation: D(g) + 2F 2 (g) --> DF4 (g) B. What is the initial rate of disappearance of F2 (g) in trial 1. Justify.
Trial [?] (?)[A] (M) [?] (?)[B] (M) Rate (M/s) 1 0.310 0.370 0.0139 2 0.310 0.740 0.0139 3 0.620 0.370 0.0556 Using the data in the table, determine the rate constant of the reaction and select the appropriate units. A+2B⟶C+D ?= Units: