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(a)
Interpretation:
The overall reaction needs to be proposed.
Concept introduction:
Reaction mechanism is step by step arrangement of elementary reactions by which overall chemical change arise. A chemical mechanism is a theoretical estimation that tries to depict in detail what happens at each phase of an overall
(b)
Interpretation:
The role of
Concept introduction:
A catalyst is shows up as a reactant first, and afterward as a product.
Intermediates are create in elementary step and consumed in later step of reaction mechanism. It does not take part in overall reaction.
(c)
Interpretation:
Whether in the given reaction mechanism
Concept introduction:
A catalyst is shows up as a reactant first, and afterward as a product.
Intermediates are create in one step and consumed in later step of reaction mechanism. Slowest step in the mechanism is rate determining step.
(d)
Interpretation:
A catalyst needs to be distinguished from an intermediate.
Concept introduction:
A catalyst is shows up as a reactant first, and afterward as a product.
Intermediates are create in elementary step and consumed in later step of reaction mechanism. It does not take part in overall reaction.
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Chapter 14 Solutions
CHEMISTRY-MOD.MASTERING (18W)
- The Raschig reaction produces the industrially important reducing agent hydrazine, N2H4, from ammonia, NH3, and hypochlorite ion, OCl−, in basic aqueous solution. A proposed mechanism is Step 1: Step 2: Step 3: What is the overall stoichiometric equation? Which step is rate-limiting? What reaction intermediates are involved? What rate law is predicted by this mechanism?arrow_forwardThe mechanism for the reaction described by the equation CH,NC(g) CH, CN(g) is suggested to be k1 (1) A(g) + M(g) = A" (g) + M(g) k-1 k2 * (2) А (g) → B(g) where A(g) is CH, NC(g), M(g) is any gas molecule, A* (g) is CH,NC*(g) (an energized gas molecule), and B(g) is CH,CN(g). Assuming that [A* ] is governed by steady-state conditions, derive the rate law for the production of CH, CN(g) in terms of [A], [M], and the appropriate k values.arrow_forwardConsider the following reaction: 2 NO(g) + 2 H2(g) N2(g) + 2 H2O(g) (a) The rate law for this reaction is second order in NO(g) and first-order in H2(g). What is the rate law for this reaction? (b) If the rate constant for this reaction at a certain temperature is 9.70e+04, what is the reaction rate when [NO(g)] = 0.0560 M and [H2(g)] = 0.119 M?Rate = M/s.(c) What is the reaction rate when the concentration of NO(g) is doubled, to 0.112 M while the concentration of H2(g) is 0.119 M?Rate = M/sarrow_forward
- Assume that the formation of nitrogen dioxide: 2NO(g) + O2(g) 2NO2(g) is an elementary reaction. (a) Write the rate law for this reaction. (b) A sample of air at a certain temperature is contaminated with 2.0 ppm of NO by volume. Under these conditions, can the rate law be simplified? If so, write the simplified rate law. (c) Under the conditions described in part (b), the half-life of the reaction has been estimated to be 6.4 × 103 min. What would the half-life be if the initial concentration of NO were 10 ppm?arrow_forwardLanthanum(III) phosphate crystallizes as a hemihydrate, LAPO4 · H20. When it is heated, it loses water to give anhydrous lanthanum(III) phosphate: 2(LAPO4 · H2O(s)) → 2 LaPO4 (s) + H20(g) This reaction is first order in the chemical amount of LAPO, · H2O. The rate constant varies with tempera- ture as follows: Temperature (°C) k (s-1) 205 2.3 x 10-4 219 3.69 x 10-4 246 7.75 x 10-4 260 12.3 x 10-4 Compute the activation energy of this reaction.arrow_forwardThe reaction between nitric oxide and bromine is described by the following chemical equation: 2NO (g) + Br, (g) – 2NOB (g) Suppose a two-step mechanism is proposed for this reaction, beginning with this elementary reaction: NO (g) + Br, (g) NOB12 (g) Suppose also that the second step of the mechanism should be bimolecular. Suggest a reasonable second step. That is, write the balanced chemical equation of a bimolecular elementary reaction that would complete the proposed mechanism.arrow_forward
- The decomposition of dinitrogen monoxide is described by the following chemical equation: 2N₂O(g) → 2N₂(g) + O₂ (g) Suppose a two-step mechanism is proposed for this reaction, beginning with this elementary reaction: N₂O(g) → N₂(g) + 0(g) Suppose also that the second step of the mechanism should be bimolecular. Suggest a reasonable second step. That is, write the balanced chemical equation of a bimolecular elementary reaction that would complete the proposed mechanism. X Śarrow_forwardThe rate constant for the first-order decomposition of N2O5 in the reaction 2 N2O5(g) → 4 NO2(g) + O2(g) is kr = 3.38 × 10−5 s−1 at 25 °C. What is the half-life of N2O5? If the initial partial pressure of N2O5 is 500 Torr, what will its partial pressure be (i) 50 s, (ii) 20 min after initiation of the reaction?arrow_forwardThe formation of nitrosyl chloride is described by the following chemical equation: 2NO(g) + Cl₂ (g) → 2NOCI (g) Suppose a two-step mechanism is proposed for this reaction, beginning with this elementary reaction: NO (g) + Cl₂ (g) → NOCI₂ (g) Suppose also that the second step of the mechanism should be bimolecular. Suggest a reasonable second step. That is, write the balanced chemical equation of a bimolecular elementary reaction that would complete the proposed mechanism.arrow_forward
- The decomposition of dinitrogen monoxide is described by the following chemical equation: 2N₂O (g) → 2N₂ (g) + O₂ (g) Suppose a two-step mechanism is proposed for this reaction, beginning with this elementary reaction: N₂0 (g) → N₂(g) +0 (g) Suppose also that the second step of the mechanism should be bimolecular. Suggest a reasonable second step. That is, write the balanced chemical equation of a bimolecular elementary reaction that would complete the proposed mechanism. 0 0-0 X Text Sarrow_forwardSuppose the formation of dinitrogen pentoxide proceeds by the following mechanism: step elementary reaction 1 NO₂ (g) +03 (g) → NO3 (g) + O₂(g) 2 NO3 (g) + NO₂ (g) → N₂O5 (g) Suppose also k₁ « k₂. That is, the first step is much slower than the second. Write the balanced chemical equation for the overall chemical reaction. Write the experimentally- observable rate law for the overall chemical reaction. Note: your answer should not contain the concentrations of any intermediates. rate = k rate constant k₁ k₂ ロ→ロ X Śarrow_forwardThe formation of tert-butanol is described by the following chemical equation: (CH3)₂CBr (aq) + OH(aq) → Br¨¯ (aq) + (CH3)₂COH(aq) Suppose a two-step mechanism is proposed for this reaction, beginning with this elementary reaction: (CH³)¸CBr (aq) → (CH3)¸₂C² (aq) +Br¯(aq) Suppose also that the second step of the mechanism should be bimolecular. Suggest a reasonable second step. That is, write the balanced chemical equation of a bimolecular elementary reaction that would complete the proposed mechanism. 0 ロ→ロ Śarrow_forward
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