100 80 60 40 20 AB+ C ABC Progress of Reaction A + BC The answers for the above question is exact. You must determine what each dash is worth to determine the scale. If the line looks a bit off that is because it is. All answers will be on a dash. The activation energy for the forward reaction is enthalpy change for the forward reaction is the reverse reaction is The reverse reaction is . The activation energy for the reverse reaction is The The enthalpy change for thermic. . The forward reaction is thermic. The chemicals that forms the activated complex is . The requirement besides energy that must be met before a collision between two reactant particles is considered effective is the correct

100 80 60 40 20 AB+ C ABC Progress of Reaction A + BC The answers for the above question is exact. You must determine what each dash is worth to determine the scale. If the line looks a bit off that is because it is. All answers will be on a dash. The activation energy for the forward reaction is enthalpy change for the forward reaction is the reverse reaction is The reverse reaction is . The activation energy for the reverse reaction is The The enthalpy change for thermic. . The forward reaction is thermic. The chemicals that forms the activated complex is . The requirement besides energy that must be met before a collision between two reactant particles is considered effective is the correct

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...

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A scientist is studying how certain factors affect the rate of a particular reaction. She observes that under one set of conditions, the reaction proceeded much faster than under a different set of conditions. Identify the most likely sets of conditions that produced each reaction rate. Drag each item to the appropriate bin. • View Available Hint(s) Reset Help lower temperature larger quantities of reactants smaller quantities of reactants higher temperature Faster reaction Slower reaction
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A certain catalyzed reaction is known to have an activation energy E 9.0 kJmol. Furthermore, the rate of this reaction is measured at 354. K and found to be 4.7 x 10 M/s. Use this information to answer the questions in the table below. Suppose the concentrations of all reactants is kept the same, but the temperature 5% from 354. K to 372. K. raised by choose one The rate will How will the rate of the reaction change? Suppose the concentrations of all reactants is kept the same, but the catalyst is removed, which has the effect of raising the activation energy by 5%, from 9.0 kJ/mol to 9.45 kJmol choose one The rate will choose one How will the rate of the reaction change? stay the same rise about 5% rise more than 5% rise less than 5% fall about 5% fall more than 5% fall less than 5%
Comment how the temperature affects the rate. a. Temperature definitely has an affect on the rate. When there is an increase in temperature, the rate at which the reaction occurs also increases. This is proved through my data. As each experiment had an increasing temperature, here are my rates that go from lowest to highest temperature: 3.25*10 M/s, 4.15*10 M/s, 6.85*10 M/s, 9.17*10* M/s. With this increase in temperature, there is therefore an increase in the energy of molecules in the solution. With this increase in energy, there is an increase in collisions with enough energy, and this ultimately leads to the rate increasing.
The rate of a certain reaction was studied at various T(K) k (s-1) temperatures. The table shows temperature (T) and rate 400 0.000108 constant (k) data collected during the experiments. Plot the 420 0.000626 data to answer the questions. 440 0.00310 What is the value of the activation energy, E, for 460 0.0134 this reaction? 480 0.0511 500 0.175 520 0.547 E, = kJ - mol- 1108.79 540 1.57 560 4.18 Incorrect 580 10.4 What is the value of the pre-exponential factor (sometimes called the frequency factor), A, for this reaction? A = 140 6.79 x10 Incorrect
Which of the following reactions is the slowest at room temperature? a. Na(s)+ Cl(g)—> 2NaCl(s) b. C2H4O2(aq) + NaHCO3(s) —-> NaC2H3O2(aq)+ H2O(l)+ CO2(g) C. I2(aq) + 2S2O3^2- (aq)——- > 2I^- (aq) + S4O6^2- (aq) d. not enough data to determine Please show your solution.
Label the reaction profiles below as exothermic or endothermic and use them to calculate the activation energy of the forward and reverse reactions and the value of AH for the reaction. This is a reaction of profile of an 250 exothermic/endothermic reaction 200 PE 150 (kJ) Eaf = ...... 100 Ea, = 50 AH = Reaction pathway 100 This is a reaction of profile of an 80 exothermic/endothermic reaction 60 PE (kJ) A+B 40 Ear = C+D 20 Ear = ΔΗ Progress of the reaction
Which of the following will lower the activation energy for a reaction? Group of answer choices raising the temperature of the reaction. increasing the concentrations of reactants. increasing the surface area of the reactants. adding a suitable catalyst.
For the following reaction 5 experiments have been run and the data collected is in the following table: 4 HBr(g) + O2(g)--->2 Br2(g) + 2 H2O(g) Experiment [HBr], M [O2 ], M Rate, M/s (aka mol/L.s) 1 0.120 0.490 0.0267 2 0.142 0.120 0.00190 3 0.120 0.630 0.0442 4 0.230 0.630 0.0846 5 0.630 0.863 0.435 a)Write the rate expression. b) Calculate the rate constant, k c) If the concentration of HBr and O2 are 1.5 x 10-3 M and 3.25 x 10-3 respectively, what is the rate of the reaction?
Initial-rate data at a certain temperature is given in the table for the reaction SO₂Cl₂(g) SO₂(g) + Cl₂(g) [SO₂Cl₂], (M) k= 0.100 0.200 0.300 Initial rate (M/s) 2.00 x 10-6 4.00 x 10-6 6.00 x 10-6 Determine the value and units of the rate constant. units:
3) Which of the following is NOT true about a catalyst? A.It may be homogeneous B. It speeds up the reverse reaction C. It is consumed D. It speeds up the forward reaction E. it may be heterogeneous
Consider the two-step mechanism for the destruction of ozone. step 1: 0,(g) + HO(g) HO, (g) + 0,(g) > step 2: HO, (g) + O(g) → HO(g) + 0,(g) Identify the type of catalyst. Identify the catalyst in the two-step mechanism. homogeneous catalyst O heterogeneous catalyst O, НО HO2