A study of the gas-phase oxidation of nitrogen monoxide at 25°C and 1.00 atm pressure gave the following results:\[ 2\text{NO}(g) + \text{O}_2(g) \rightarrow \text{NO}_2(g) \]| Experiment | Conc. NO (mol/L) | Conc. O\[_2\] (mol/L) | Initial Rate (mol/(L · s)) ||------------|------------------|----------------------|--------------------------|| Exp. 1 | \(8.4 \times 10^{-2}\) | 7.1 \(\times 10^{-2}\) | \(9.0 \times 10^{-2}\) || Exp. 2 | \(8.4 \times 10^{-2}\) | 0.14 | 0.18 || Exp. 3 | 0.17 | 0.28 | 1.5 || Exp. 4 | 0.76 | 7.4 \(\times 10^{-3}\) | ? |**Question:**What is the experimental rate law for the reaction above? (Use \( k \) for the rate constant.)**Answer:**Rate law = \( k[\text{NO}]^2[\text{O}_2] \)**Question:**What is the initial rate of the reaction in Experiment 4?**Answer:**Initial rate = \_\_\_\_\_\_\_\_ mol/(L · s)

Chemical kinetics is the study of the reaction that how fast or slow a reaction is taking place. The…

A study of the gas-phase oxidation of nitrogen monoxide at 25°C and 1.00 atm pressure gave the following results: 2NO(9) + O2 (9) → NO2(9) Сonc. NO, mol/ Conc. O2, molL Initial Rate Exp. 1 8.4 x 10-2 7.1 x 10-2 9.0 x 10-2 mol/(L -s) Еxp. 2 8.4 x 10-2 0.14 0.18 mol/(L · 8) Exp. 0.17 0.28 1.5 mol/(L · s) Еxp. 4 0.76 7.4 x 10-3 ? What is the experimental rate law for the reaction above? (Use k for the rate constant.) Rate law = k[NO]°[0,] What is the initial rate of the reaction in Experiment 4? Initial rate = | ] mol/(L - s)

A study of the gas-phase oxidation of nitrogen monoxide at 25°C and 1.00 atm pressure gave the following results: 2NO(9) + O2 (9) → NO2(9) Сonc. NO, mol/ Conc. O2, molL Initial Rate Exp. 1 8.4 x 10-2 7.1 x 10-2 9.0 x 10-2 mol/(L -s) Еxp. 2 8.4 x 10-2 0.14 0.18 mol/(L · 8) Exp. 0.17 0.28 1.5 mol/(L · s) Еxp. 4 0.76 7.4 x 10-3 ? What is the experimental rate law for the reaction above? (Use k for the rate constant.) Rate law = k[NO]°[0,] What is the initial rate of the reaction in Experiment 4? Initial rate = | ] mol/(L - s)

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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Reaction CaCO3(s) Ca²+ (aq) + CO3²- (aq) AgCl(s) Ag+ (aq) + Cl(aq) AgBr(s) = Ag*(aq) + Br(aq) Agl(s) Ag+ (aq) + I¯(aq) Initial Concentrations ← [Ca²+] = 1.0 x 10-⁹ M [CO32] = 1.0 x 10⁹ M Ksp = [Ca²+][CO3²-1 X = 3.8 x 10-9 Initial Conditions Q = [1.0 × 10-⁹][1.0 × 10-⁹] = 1.0 x 10-18 Equilibrium Conditions [Ca2+] = 1.0 x 10⁹ M [CO32] 1.0 x 10.⁹ M Mass of CaCO3(s) = 0.0 g 42 of 7 What is the value of the reaction quotient, Q, which is calculated by substituting the actual initial values of [Ca²+] and [CO32] into the equilibrium expression?
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3. The following reaction: A' (a) + B (ag + C (an)→ G* (ae) +2 H ) AH = -250 kJ There are two proposed mechanism: Mechanism 1 A' () + B aa) AB' a) + D (a) Step 1 AB" (a) (fast) + E (a) + Hm → G' sae) + H ) + D² (n) Step 2 (slow) Step 3 E (agi+ C (a) (fast) Mechanism 2: Step 1 AB' (a) A' (an) + B (ag) AB' (a) + C ja) (fast) Step 2 + G' (a) + 2 H() (slow) The reactions was determined to have the following rate law: r= k[A'][B] a) Which of the two proposed mechanisms is valid? Explain. b) List any reaction intermediates: catalysts: c) What is a rate determining step? d) If the activation energy for the overall forward reaction is 150 kJ, sketch the potential energy diagram for the above reaction; showing the overall reaction, the reaction mechanism, labelling the AHu, AHy, Eapu, Eag, reaction intermediates, and activated complex. rvs fwd drvs/
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(5) IV. Hydrogen and carbon monoxide react to give formaldehyde under certain conditions. H2(g) + CO(g) = HCHO(g) The mechanism proposed for this reaction is H2(g) = 2 H(g) H(g) + CO(g) H(g),+ HCO(g) → HCHO What rate law is derived from this mechanism? Step 1 Step 2 Step 3 fast HCO(g) slow > fast