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Ch.14 - Chemical Kinetics
Brown - Chemistry: The Central Science 14th Edition
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoBrown 14th EditionCh.14 - Chemical KineticsProblema 41a
Capitolo 14, Problema 41a

(a) The gas-phase decomposition of SO2Cl2, SO2Cl2(g) → SO2(g) + Cl2(g), is first order in SO2Cl2. At 600 K the half-life for this process is 2.3 × 105 s. What is the rate constant at this temperature?

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Step 1: Understand the problem. We are given that the reaction is first order and we are given the half-life. We need to find the rate constant (k).
Step 2: Recall the formula for the rate constant in a first order reaction. The formula is k = ln(2) / t1/2, where t1/2 is the half-life of the reaction.
Step 3: Substitute the given half-life into the formula. The half-life is given as 2.3 * 10^5 s.
Step 4: Calculate the rate constant. Remember that ln(2) is approximately 0.693.
Step 5: The rate constant k is then the result of the calculation from step 4. This is the final answer.

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First-Order Reactions

First-order reactions are chemical reactions where the rate is directly proportional to the concentration of one reactant. This means that as the concentration of the reactant decreases, the rate of the reaction also decreases. The rate law for a first-order reaction can be expressed as rate = k[A], where k is the rate constant and [A] is the concentration of the reactant.
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First-Order Reactions

Half-Life of a Reaction

The half-life of a reaction is the time required for the concentration of a reactant to decrease to half of its initial value. For first-order reactions, the half-life is constant and independent of the initial concentration, calculated using the formula t1/2 = 0.693/k, where k is the rate constant. This relationship is crucial for determining the rate constant from the given half-life.
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First-Order Half-Life

Rate Constant (k)

The rate constant (k) is a proportionality factor in the rate law that quantifies the speed of a reaction at a given temperature. It is specific to each reaction and varies with temperature. For first-order reactions, the rate constant can be derived from the half-life using the equation k = 0.693/t1/2, allowing us to calculate k when the half-life is known.
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Equilibrium Constant K
Pratica correlata
Domanda del libro di testo

As described in Exercise 14.41, the decomposition of sulfuryl chloride (SO2Cl2) is a first-order process. The rate constant for the decomposition at 660 K is 4.5 × 10-2 s-1. (a) If we begin with an initial SO2Cl2 pressure of 450 torr, what is the partial pressure of this substance after 60 s?

Domanda del libro di testo

(b) At 320°C the rate constant is 2.2 × 10-5 s-1. What is the half-life at this temperature?

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Domanda del libro di testo

(a) For the generic reaction A → B what quantity, when graphed versus time, will yield a straight line for a first-order reaction?

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Domanda del libro di testo

(b) How can you calculate the rate constant for a first-order reaction from the graph you made in part (a)?

Domanda del libro di testo

The decomposition of sodium bicarbonate (baking soda), NaHCO3(s), into Na2CO3(s), H2O(l), and CO2(g) at constant pressure requires the addition of 85 kJ of heat per two moles of NaHCO3. (b) Draw an enthalpy diagram for the reaction.

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