Domanda del libro di testo
The tabulated data were collected for this reaction at 500 °C: CH3CN(g) → CH3NC( g) a. Determine the order of the reaction and the value of the rate constant at this temperature.
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Ch.14 - Chemical Kinetics
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831
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TOC.tableOfContents
- Ch.1 - Matter, Measurement & Problem Solving136
- Ch.2 - Atoms & Elements112
- Ch.3 - Molecules, Compounds & Chemical Equations159
- Ch.4 - Chemical Quantities & Aqueous Reactions140
- Ch.5 - Gases118
- Ch.6 - Thermochemistry106
- Ch.7 - Quantum-Mechanical Model of the Atom62
- Ch.8 - Periodic Properties of the Elements103
- Ch.9 - Chemical Bonding I: The Lewis Model104
- Ch.10 - Chemical Bonding II: Molecular Shapes & Valence Bond Theory89
- Ch.11 - Liquids, Solids & Intermolecular Forces73
- Ch.12 - Solids and Modern Material59
- Ch.13 - Solutions110
- Ch.14 - Chemical Kinetics140
- Ch.15 - Chemical Equilibrium78
- Ch.16 - Acids and Bases155
- Ch.17 - Aqueous Ionic Equilibrium176
- Ch.18 - Free Energy and Thermodynamics108
- Ch.19 - Electrochemistry118
- Ch.20 - Radioactivity and Nuclear Chemistry82
- Ch.21 - Organic Chemistry150
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831Non è quello che usi tu?Cambia libro di testo
Capitolo 14, Problema 82
The activation barrier for the hydrolysis of sucrose into glucose and fructose is 108 kJ/mol. If an enzyme increases the rate of the hydrolysis reaction by a factor of 1 million, how much lower must the activation barrier be when sucrose is in the active site of the enzyme? (Assume that the frequency factors for the catalyzed and uncatalyzed reactions are identical and a temperature of 25 °C.)
Guida verificata passo dopo passo1
Identify the given information: the activation energy for the uncatalyzed reaction is 108 kJ/mol, the rate increase factor is 1 million, and the temperature is 25 °C.
Use the Arrhenius equation: k = A * e^(-Ea/(RT)), where k is the rate constant, A is the frequency factor, Ea is the activation energy, R is the gas constant (8.314 J/(mol·K)), and T is the temperature in Kelvin.
Convert the temperature from Celsius to Kelvin: T = 25 + 273.15 = 298.15 K.
Set up the ratio of the rate constants for the catalyzed (k_cat) and uncatalyzed (k_uncat) reactions: k_cat / k_uncat = 1,000,000 = e^(-(Ea_cat - Ea_uncat)/(RT)).
Solve for the difference in activation energies (Ea_uncat - Ea_cat) using the natural logarithm: Ea_uncat - Ea_cat = RT * ln(1,000,000).
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Activation Energy
Activation energy is the minimum energy required for a chemical reaction to occur. It represents the energy barrier that reactants must overcome to transform into products. In the context of enzyme-catalyzed reactions, enzymes lower the activation energy, allowing reactions to proceed more quickly at lower temperatures.
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Percorso guidato
02:02
Activity Series Chart
Enzyme Catalysis
Enzyme catalysis involves the acceleration of a chemical reaction by a catalyst, which in biological systems is typically an enzyme. Enzymes work by providing an alternative reaction pathway with a lower activation energy, thus increasing the reaction rate significantly. The effectiveness of an enzyme can be quantified by how much it reduces the activation energy compared to the uncatalyzed reaction.
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01:59Catalyzed vs. Uncatalyzed Reactions
Arrhenius Equation
The Arrhenius equation describes the temperature dependence of reaction rates and relates the rate constant of a reaction to its activation energy. It is expressed as k = A * e^(-Ea/RT), where k is the rate constant, A is the frequency factor, Ea is the activation energy, R is the gas constant, and T is the temperature in Kelvin. This equation is crucial for understanding how changes in activation energy affect reaction rates, especially in the context of enzyme activity.
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01:20Arrhenius Equation
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Suppose that the reaction A¡products is exothermic and has an activation barrier of 75 kJ/mol. Sketch an energy diagram showing the energy of the reaction as a function of the progress of the reaction. Draw a second energy curve showing the effect of a catalyst.
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Domanda del libro di testo
The tabulated data were collected for this reaction at 500 °C: CH3CN(g) → CH3NC( g) b. What is the half-life for this reaction (at the initial concentration)?
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