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CHEM 29402 Chapter Notes - Chapter 17: Chemical Equilibrium, Equilibrium Constant, Reaction Rate

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amberherring211

13 Feb 2016

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Sheridan College

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Therefore, the reaction speeds up: the minimum energy required a reaction to occur is called the activation energy (ea) If a given collision posses an energy, which is greater than the ea, then the collision can result in a reaction. If the temperature gets increased, the speeds of the molecules increase. This increases the reaction rate: catalyst: a substance that speeds up a reaction without being consumed. In the human body, enzymes act as catalysts. Enzymes allow our bodies to speed up complicated reactions. But it can be included in if it"s a gas, as the concentration of water vapour can change. Le chatelier"s principle: le chatelier"s principle states that when a change is imposed on a system as equilibrium, the position of the equilibrium shifts in a direction that tends to reduce the effect of that change. Or: when a reactant / product is added to a system at equilibrium, it shifts away from the added component.

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Related Questions

1a. Collision theory helps us to explain the factors affecting the rate of reactions between molecules. Select all of the following that should increase the rate of a reaction.

Increasing the concentration of the reactants.

Using complex molecules that have a limited number of sites where a collision will be successful.

Adding a catalyst that decreases the size of E_a.

Increasing the volume of the solution by dilution.

Decreasing the temperature of the reaction.

1b. Select all of the following that would act to make the value of k become smaller.

The temperature of the reaction is decreased.

The reactant has many sites for a successful collision to occur.

A catalyst is used which acts to lower the activation energy for the reaction.

The mobility of the molecules is decreased so that there are fewer collisions.

The reaction is heated.

The concentration of the reactant is increased.

Help with these

In the collision model it is assumed that reactions occur as a result of collisions between molecules with the correct kinetic energy and orientation. The minimum energy required for a reaction to occur when molecules collide is called the activation energy, E_a. The number of collisions that are favorably oriented for a reaction is described by the frequency factor, A. The Arrhenius equation relates both of these factors to the rate constant, k. k = A middot e^-E_a/(R middot T) where R = 8.314 J/(mol middot K) and T is the temperature in kelvins. Based on the activation energies and frequency factors, rank the following reactions from fastest to slowest reaction rate, assuming they are all at the same temperature. Rank from fastest to slowest reaction rate. To rank items as equivalent, overlap them. Fraction of molecules The exponential term in the Arrhenius equation is equal to the fraction of molecules, f, with kinetic energy greater than or equal to the activation energy: f = e^-E_a/(R middot T) Most scientific calculators have an e^x function as the second function of the LN button. Part B A certain reaction with an activation energy of 145 kJ/mol was run at 495 K and again at 515 K. What is the ratio of f at the higher temperature to f at the lower temperature? Express your answer numerically using one significant figure. In the collision model it is assumed that reactions occur as a result of collisions between molecules with the correct kinetic energy and orientation. The minimum energy required for a reaction to occur when molecules collide is called the activation energy, E_a. The number of collisions that are favorably oriented for a reaction is described by the frequency factor, A. The Arrhenius equation relates both of these factors to the rate constant, k: k = A middot e^-E_a/(R middot T) where R = 8.314 J/(mol middot K) and T is the temperature in kelvins. Part A Based on the activation energies and frequency factors, rank the following reactions from fastest to slowest reaction rate, assuming they are all at the same temperature. Rank from fastest to slowest reaction rate. To rank items as equivalent, overlap them. Fraction of molecules The exponential term in the Arrhenius equation is equal to the fraction of molecules, f, with kinetic energy greater than or equal to the activation energy: f = e^E_a/(R middot T) Most scientific calculators have an e^x function as the second function of the LN button. Part B A certain reaction with an activation energy of 145 kJ/mol was run at 495 K and again at 515 K. What is the ratio of f at the higher temperature to f at the lower temperature? Express your answer numerically using one significant figure. In the collision model it is assumed that reactions occur as a result of collisions between molecules with the correct kinetic energy and orientation. The minimum energy required for a reaction to occur when molecules collide is called the activation energy, Ea. The number of collisions that are favorably oriented for a reaction is described by the frequency factor, A. The Arrhenius equation relates both of these factors to the rate constant, k: k = A middot e^-E_a/(R middot T) where R = 8.314 J/(mol middot K) and T is the temperature in kelvins. Fraction of molecules The exponential term in the Arrhenius equation is equal to the fraction of molecules, f, with kinetic energy greater than or equal to the activation energy: f = e^-E_a/(R middot T) Most scientific calculators have an e^x function as the second function of the LN button. Part B A certain reaction with an activation energy of 14 kJ/mol was run at 495 K and again at 515 K. What is the ratio of f at the higher temperature to f at the lower temperature? Express your answer numerically using one significant figure.