The magnitude of the specific rate constant is dependent on the conditions at which the concentration of a reactant must be raised to give the experimentally observed relationship between: concentration and products concentration and rate concentration and temperature products and rate

The magnitude of the specific rate constant is dependent on the conditions at which the concentration of a reactant must be raised to give the experimentally observed relationship between: concentration and products concentration and rate concentration and temperature products and rate

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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T = Chemical reactions produce one or more product substances from one or more reactant substances. If x molecules of reactant X combine with y molecules of reactant Y to produce z molecules of product Z, we write xX+yY→ ZZ. The reaction rater is the rate of change of concentration of 1 dz 1 dX one of the products over time; for this example, r = 1 dy z dt x dt dY dt dX dt Nitrogen gas N₂ and hydrogen gas H₂ combine to produce ammonia NH3 according to dY dX dt 1N₂ + 3H₂ → 2NH3. Find r, and if ammonia is being produced at a rate of 5 moles dt per liter per hour. = esc T M Question Help: Message instructor Submit Question K 8366-SUMMER2023 / June 5- June 11 / Practice: Derivative mol Lh mol Lh → # C - $ y dt M % O Oll
Please answer these questions in an essay form.
Can you help me correcting this questions in the picture with the notes below please? Notes: In question 1a, the rate law is fine but should have partial pressures, not concentrations. In 1b, the units of the answer are incorrect; they should have "atm" in it. Hint: in the denominator of the calculation is atm^3.
the change in temp from 10°C to 20°C is found to double the rate of a particular chemical reaction how did the chnage in temp affect the reaction
(a) Select all of the correct statements about reaction rates from the choices below. The lower the rate of a reaction the longer it takes to reach completion. A balanced chemical reaction is necessary to relate the rate of reaction to the concentration of a reactant. As a reaction progresses its rate goes down. The rate of a slow step has more effect on the overall reaction rate than the rate of a fast step. Reaction rates are determined by reactant concentrations, temperatures, and reactant stabilities. Reaction rates increase with increasing temperature. Reactions involving very unstable combinations of chemicals have large rate constants.
Which of the following statements is true about a catalyzed reaction? * A catalyzed reaction makes the reaction to proceed at a slower rate which is about 10^2 to 10^8 times than an uncatalyzed one. When a catalyst is applied in a reaction, the reaction produced additional derivatives of the primary product. A catalyzed reaction only occurs when the condition of the reaction is in acidic medium. A catalyzed reaction makes the reaction to proceed at a faster rate than an uncatalyzed reaction.
Which of the following statements is true about a catalyzed reaction? * A catalyzed reaction makes the reaction to proceed at a slower rate which is about 10^2 to 10^8 times than an uncatalyzed one. When a catalyst is applied in a reaction, the reaction produced additional derivatives of the primary product. A catalyzed reaction only occurs when the condition of the reaction is in acidic medium. A catalyzed reaction makes the reaction to proceed at a faster rate than an uncatalyzed reaction.
Peroxynitric acid (HOONO2) is an unstable molecule that decomposes to nitric acid and oxygen: 2HOONO2(aq) → 2HNO3(aq) + O2(g)When the concentration of peroxynitic acid is graphed against time, the resulting plot is curved, but if the logarithm of this concentration is plotted, we instead get a straight line. Based on this, which statement is true? a) This decay is a second order in peroxynitric acid. b) The slope of the straight-line graph is the rate constant. c) One needs the concentration of peroxynitric acid to calculate its half-life. d) The rate law appears to be of the form -Δ[HOONO2]/Δt = k[HOONO2].
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
Consider the experimental data collected for the following chemical reaction: 2H2(g) + 2NO(g) → N2(g) + 2H2O(g) Trial Initial [H2] (mol/L) Initial [NO] (mol/L) Rate of Reaction (mol/L∙s) 1 0.031 0.0025 2.0 x 10-3 2 0.062 0.0025 4.0 x 10-3 3 0.031 0.0050 8.0 x 10-3 4 0.062 0.0050 1.6 x 10-2 Which action will have more effect on the rate of this reaction; changing the concentration of H2(g) or that of NO(g)? Explain your reasoning by considering the orders of reactants and writing the corresponding rate law equation.
Increasing the temperature of a reaction increases the speed at which the reaction occurs. Identify the statements that explain the correlation between the increase in temperature and the increase in reaction rate. More atom-atom stretching and bending within the molecules occurs at higher temperatures, which creates more reactive molecular configurations. Added heat decreases the activation energy of a reaction and has a similar effect as adding a catalyst. ✔ Molecules at higher temperatures have greater kinetic energy, which results in more frequent and higher energy collisions. An increased temperature improves the reaction pathway by decreasing the energy difference between reactants and products.