What will happen when kinetic energy of the reacting molecules increases

1 Essential Ideas • Introduction • 1.1 Chemistry in Context • 1.2 Phases and Classification of Matter • 1.3 Physical and Chemical Properties • 1.4 Measurements • 1.5 Measurement Uncertainty, Accuracy, and Precision • 1.6 Mathematical Treatment of Measurement Results • Key Terms • Key Equations • Summary • Exercises • 2 Atoms, Molecules, and Ions • Introduction • 2.1 Early Ideas in Atomic Theory • 2.2 Evolution of Atomic Theory • 2.3 Atomic Structure and Symbolism • 2.4 Chemical Formulas • 2.5 The Periodic Table • 2.6 Ionic and Molecular Compounds • 2.7 Chemical Nomenclature • Key Terms • Key Equations • Summary • Exercises • 6 Electronic Structure and Periodic Properties of Elements • Introduction • 6.1 Electromagnetic Energy • 6.2 The Bohr Model • 6.3 Development of Quantum Theory • 6.4 Electronic Structure of Atoms (Electron Configurations) • 6.5 Periodic Variations in Element Properties • Key Terms • Key Equations • Summary • Exercises • 7 Chemical Bonding and Molecular Geometry • Introduction • 7.1 Ionic Bonding • 7.2 Covalent Bonding • 7.3 Lewis Symbols and Structures • 7.4 Formal Charges and Resonance • 7.5 Strengths of Ionic and Covalent Bonds • 7.6 Molecular Structure and Polarity • Key Terms • Key Equations • Summary • Exercises • 9 Gases • Introduction • 9.1 Gas Pressure • 9.2 Relating Pressure, Volume, Amount, and Temperature: The Ideal Gas Law • 9.3 Stoichiometry of Gaseous Substances, Mixtures, and Reactions • 9.4 Effusion and Diffusion of Gases • 9.5 The Kine...

Factors affecting enzyme action Physical factors affect enzyme activity. Temperature At low temperatures, the number of collisions between the enzyme and substrate are reduced because molecules have low kinetic energy. Fewer collisions result in fewer successful collisions in a given time and the reaction is slow. As the temperature and therefore kinetic energy of the molecules increases, the enzymes and substrates will collide more often which results in an increased chance of a successful collision between the enzymes active site and the substrate. This will result in more enzyme/substrate complexes forming in a given time and the rate of the reaction is increased. Very high temperatures disrupt the shape of the active site, which will reduce its activity by preventing the formation of enzyme/substrate complexes. The enzyme will have been denatured . Enzymes therefore work best at a particular temperature called the optimum temperature. A graph to show the effect of temperature on enzyme activity: The effect of pH Enzymes are also sensitive to pH . Changing the pH of its surroundings will also change the shape of the active site of an enzyme. Many amino acids in an enzyme molecule carry a charge . Within the enzyme molecule, positively and negatively charged amino acids will attract. This contributes to the folding of the enzyme molecule, its shape, and the shape of the active site. Changing the pH will affect the charges on the amino acid molecules. Amino acids that att...

Learning Objectives • State the postulates of the kinetic-molecular theory • Use this theory’s postulates to explain the gas laws The gas laws that we have seen to this point, as well as the ideal gas equation, are empirical, that is, they have been derived from experimental observations. The mathematical forms of these laws closely describe the macroscopic behavior of most gases at pressures less than about 1 or 2 atm. Although the gas laws describe relationships that have been verified by many experiments, they do not tell us why gases follow these relationships. The kinetic molecular theory (KMT) is a simple microscopic model that effectively explains the gas laws described in previous modules of this chapter. This theory is based on the following five postulates described here. (Note: The term “molecule” will be used to refer to the individual chemical species that compose the gas, although some gases are composed of atomic species, for example, the noble gases.) • Gases are composed of molecules that are in continuous motion, travelling in straight lines and changing direction only when they collide with other molecules or with the walls of a container. • The molecules composing the gas are negligibly small compared to the distances between them. • The pressure exerted by a gas in a container results from collisions between the gas molecules and the container walls. • Gas molecules exert no attractive or repulsive forces on each other or the container walls; therefore...

Kinetics is the study of reaction rates and how they are affected. Many factors, such as concentration, pressure, temperature, and enzyme activity, can impact the rate of a reaction. For example, a molecule's kinetic energy is directly proportional to its temperature, so increasing the temperature will result in an increase in reaction rate. Created by Sal Khan. Yes, if it is a reaction between gases. If you increase the partial pressure of each reactant, you will increase the collision rate between molecules, since you will be increasing the gas activity, but it only works for gaseous reactions ! However, you have to be careful by using this information, because if you analyze a reaction between two aquous reactants, depending on the circumstances there can be an equilibrium between liquid and gasous states of a reactant, so increasing its the vapour pressure might increase its aquous concentration and then affect the reaction rate. Its most of the time related to the concentration and molecules quadratic speeds. Is it fair to think about this in terms of velocities of molecules? So if you add heat to the system (increase the velocities of the molecules), then molecules of H2 and I2 will collide at higher velocities (higher energies). My question is: How do all the speeds of the particles change from before reaction, during reaction, and after reaction? Which is moving faster: a H2, I2, or HI after the reaction? The average kinetic energies of the molecules are all the sa...

Learning Outcomes • Use kinetic molecular theory to explain the properties of gases The gas laws that we have seen to this point, as well as the ideal gas equation, are empirical, that is, they have been derived from experimental observations. The mathematical forms of these laws closely describe the macroscopic behavior of most gases at pressures less than about 1 or 2 atm. Although the gas laws describe relationships that have been verified by many experiments, they do not tell us why gases follow these relationships. The kinetic molecular theory (KMT) is a simple microscopic model that effectively explains the gas laws described in the previous sections of this chapter. This theory is based on the following five postulates described here. (Note: The term “molecule” will be used to refer to the individual chemical species that compose the gas, although some gases are composed of atomic species, for example, the noble gases.) • Gases are composed of molecules that are in continuous motion, traveling in straight lines and changing direction only when they collide with other molecules or with the walls of a container. • The molecules composing the gas are negligibly small compared to the distances between them. • The pressure exerted by a gas in a container results from collisions between the gas molecules and the container walls. • Gas molecules exert no attractive or repulsive forces on each other or the container walls; therefore, their collisions are elastic (do not inv...

Learning Objectives • State the postulates of the kinetic-molecular theory • Use this theory’s postulates to explain the gas laws The gas laws that we have seen to this point, as well as the ideal gas equation, are empirical, that is, they have been derived from experimental observations. The mathematical forms of these laws closely describe the macroscopic behavior of most gases at pressures less than about 1 or 2 atm. Although the gas laws describe relationships that have been verified by many experiments, they do not tell us why gases follow these relationships. The kinetic molecular theory (KMT) is a simple microscopic model that effectively explains the gas laws described in previous modules of this chapter. This theory is based on the following five postulates described here. (Note: The term “molecule” will be used to refer to the individual chemical species that compose the gas, although some gases are composed of atomic species, for example, the noble gases.) • Gases are composed of molecules that are in continuous motion, travelling in straight lines and changing direction only when they collide with other molecules or with the walls of a container. • The molecules composing the gas are negligibly small compared to the distances between them. • The pressure exerted by a gas in a container results from collisions between the gas molecules and the container walls. • Gas molecules exert no attractive or repulsive forces on each other or the container walls; the...