2. Consider the following reaction: Time b) What is the rate law? 0 1000 2000 3000 4000 5000 A B [A] (M) 0.475 0.350 0.277 0.230 0.196 0.171 a) Determine the order of the reaction by graphing the data appropriately. You may create graphs by hand using the graph paper provided or by using Excel or Google Sheets (be sure to include an image of your graph). Explain your answer. c) What is the rate constant? Provide appropriate units.

2. Consider the following reaction: Time b) What is the rate law? 0 1000 2000 3000 4000 5000 A B [A] (M) 0.475 0.350 0.277 0.230 0.196 0.171 a) Determine the order of the reaction by graphing the data appropriately. You may create graphs by hand using the graph paper provided or by using Excel or Google Sheets (be sure to include an image of your graph). Explain your answer. c) What is the rate constant? Provide appropriate units.

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

The following data were collected for a certain reaction of the type A → products. Determine the overall order of this reaction. Time t, min [A]t, mol L–1 0 0.500 10 0.463 20 0.426 60 0.278 A. 3 B. 2 C. 4 D. 0 E. 1
For A⟶products, time and concentration data were collected and plotted as shown. [A] (M) t (s) 0.750 00.0 0.596 30.0 0.473 60.0 0.376 90.0 Determine the reaction order, the rate constant, and the units of the rate constant. order= k= units
The reaction described by the equation 0,(g) + NO(g) → 0,(g) + NO,(g) has, at 310 K, the rate law rate of reaction = k[O,][NO] k = 3.0 × 106 M-!·s-! Given that [O,] = 4.0 × 10-4 M and [NO] = 2.0 × 10-³ M at t = 0, calculate the rate of the reaction at t = 0. %3D rate: M/s What is the overall order of this reaction? 3
The following mechanism has been suggested for a reaction: NO(g) + Br2(g) → NOBR2(g) fast NOBR2(g) + NO(g) 2 NOBr(g) slow (a) What is the overall reaction? (b) What are the intermediates in the mechanism? (c) What is the rate law for the reaction? Edit View Insert Format Tools Table 12pt v Paragraph B IUA IMG F4 F5 F6 E10
The rate of a certain reaction was studied at various temperatures. The table shows temperature (?) and rate constant (?) data collected during the experiments. Plot the data to answer the questions. What is the value of the activation energy, ?a , for this reaction? What is the value of the pre‑exponential factor (sometimes called the frequency factor), ? , for this reaction? Temperature (K) k (s^-1) 400 0.0000173 580 7.43
3. Consider NO₂ (g) + CO (g) → NO (g) + CO₂ (g). The initial rates are shown in the table below. Please compute (a) the rate law for the reaction and (b) compute the value of k. [CO] 0.050 0.050 0.100 0.100 [NO₂] 0.050 0.100 0.200 0.100 Initial Rate (M/s) 0.0040 0.016 0.256 0.0640
The following initial rate data are for the reaction for the formation of phosgene from carbon monoxide and chlorine: Co + Cl, → COCI, Experiment [CO],, M [Cl], M Initial Rate, Ms1 1.32x10-29 lo1 0.757 0.116 2.63x10-29 2.63x1 5.25x10-29 0.757 0.232 3 1.51 0.116 -29 4 1.51 0.232 Complete the rate law for this reaction in the box below. Use the form k[A]"[B]" , where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n Rate = From these data, the rate constant is му1
For the reaction A → products, concentration and time data were collected. t (s) [A] (M) Enter these data into the graphing tool to determine the reaction order. 0.0 3.40 25.0 2.28 50.0 1.53 75.0 1.02 Graphing Tool Clear All Data [A] vs. t In[A] vs. t 1/[A] vs. t [A] In[A] 1/[A] Add Row 10 total rows What is the reaction order? Calculate the concentration of A after 127 s. [A]]27s = M [V)
4. The common sugar sucrose breaks down in dilute acid solutions to form glucose and fructose. The rate of this reaction has been studied and the data in the table below: Time (min) [Sucrose] (mol.L') 0.316 39 0.274 80 0.238 140 0.190 210 0.146 a) Plot In[sucrose] versus time and 1/[sucrose] versus time. b) What is the order of the reaction? c) Write the rate law and calculate the rate constant, k. d) Estimate the concentration of sucrose after 175 min.
59.)
(d) Decreasing the pressure of NO, from 0.50 atm to 0.250 atm. (b) Increasing the concentration of CO from 0.01 M to 0.03 M. 16. How will each of the following affect the rate of the reaction: CO(g)+ NO2(8) → CO2(8) + NO(6) se. -> rate law for the reaction is rate = K[NO2][CO] ? (a) Increasing the pressure of NO, from 0.1 atm to 0.3 atm (b) Increasing the concentration of CO from 0.02 M to 0.06 M. 17 Reaul
For the reaction A → products, concentration and time data were collected. t (s) [A] (M) Enter these data into the graphing tool to determine the reaction order. 0.0 3.40 25.0 2.28 50.0 1.53 75.0 1.02 Graphing Tool Clear All Data [A] vs. t In[A] vs. t 1/[A] vs. t t [A] In[A] 1/[A] 3.4 3.4 1.223775 0.294118 25 2.28 0.824175 0.438596 2.822 + 50 1.53 0.425268 0.653595 2.244 + 75 1.02 0.019803 0.980392 1.666 - 1.088 - 0.51 - 15 30 45 60 75 t y=-0.03156 x + 3.241000 2= 0.971 Add Row 10 total rows What is the reaction order? O 1 Calculate the concentration of A after 127 s. [A]127 s = M [V)