Gone in 60 Seconds essays

Gone in 60 Seconds essays Gone in 60 Seconds reunites actor Nicolas Cage with producer Jerry Bruckheimer. The two are known for some of the best action movies ever, including The Rock and Con Air. Gone in 60 Seconds carries on that very same tradition with fast high speed action and fast high speed car chases. Gone in 60 Seconds tells the story of Randall Memphis Raines (Cage), a retired car thief who has given up the life of crime and has settled down. His younger brother (Ribisi), is still very much into the car stealing scene, and has gotten himself into trouble with his boss by botching a high priced boost. The boss then sends an ultimatum to Memphis: either he comes back to the business and lifts 50 cars in 4 days, or his brother dies. Memphis decides to return to his former profession for the sake of his brother, and gathers some old friends and forms a crew of car boosting experts. The chemistry between most of the characters works. Cage plays the protective older brother to Ribisi, a kid whos gotten into the life too deep and finds himself in more trouble than he can handle. Robert Duvall is the veteran who masterminds the whole The supporting cast is there for some comic relief. They fill the movie with many cliches and stereotypes. Ribisis young friends are the exact opposite of Cages crew. They are using their new high tech gadgets to steal cars for the money, unlike Cage and his crew who do it for the rush. In one of the funnier scenes, a member of Cages team is car-jacked while he is driving away with a stolen car. Instead of surrendering, he curses, gets out of his car, beats down the car-jacker, and lectures him that hes an amateur who doesnt know the first thing about reall ...

Mixture Definition and Examples in Science

Mixture Definition and Examples in Science In chemistry, a mixture forms when  two or more substances are combined such that each substance retains its own chemical identity. Chemical bonds between the components are neither broken nor formed. Note that even though the chemical properties of the components havent changed, a mixture may exhibit new physical properties, like boiling point and melting point. For example, mixing together water and alcohol produces a mixture that has a higher boiling point and lower melting point than alcohol (lower boiling point and higher boiling point than water). Key Takeaways: Mixtures A mixture is defined as the result of combining two or more substances, such that each maintains its chemical identity. In other words, a chemical reaction does not occur between components of a mixture.Examples include combinations of salt and sand, sugar and water, and blood.Mixtures are classified based on how uniform they are and on the particle size of components relative to each other.Homogeneous mixtures have a uniform composition and phase throughout their volume, while heterogeneous mixtures do not appear uniform and may consist of different phases (e.g., liquid and gas).Examples of types of mixtures defined by particle size include colloids, solutions, and suspensions. Examples of Mixtures Flour and sugar may be combined to form a mixture.Sugar and water form a mixture.Marbles and salt may be combined to form a mixture.Smoke is a mixture of solid particles and gases. Types of Mixtures Two broad categories of mixtures are heterogeneous and homogeneous mixtures. Heterogeneous mixtures are not uniform throughout the composition (e.g. gravel), while homogeneous mixtures have the same phase and composition, no matter where you sample them (e.g., air). The distinction between heterogeneous and homogeneous mixtures is a matter of magnification or scale. For example, even air can appear to be heterogeneous if your sample only contains a few molecules, while a bag of mixed vegetables may appear homogeneous if your sample is an entire truckload full of them. Also note, even if a sample consists of a single element, it may form a heterogeneous mixture. One example would be a mixture of pencil lead and diamonds (both carbon). Another example could be a mixture of gold powder and nuggets. Besides being classified as heterogeneous or homogeneous, mixtures may also be described according to the particle size of the components: Solution: A chemical solution contains very small particle sizes (less than 1 nanometer in diameter). A solution is physically stable and the components cannot be separated by decanting or centrifuging the sample. Examples of solutions include air (gas), dissolved oxygen in water (liquid), and mercury in gold amalgam (solid), opal (solid), and gelatin (solid). Colloid: A colloidal solution appears homogeneous to the naked eye, but particles are apparent under microscope magnification. Particle sizes range from 1 nanometer to 1 micrometer. Like solutions, colloids are physically stable. They exhibit the Tyndall effect. Colloid components cant be separated using decantation, but may be isolated by centrifugation. Examples of colloids include hair spray (gas), smoke (gas), whipped cream (liquid foam), blood (liquid),   Suspension: Particles in a suspension are often large enough that the mixture appears heterogeneous. Stabilizing agents are required to keep the particles from separating. Like colloids, suspensions exhibit the Tyndall effect. Suspensions may be separated using either decantation or centrifugation. Examples of suspensions include dust in air (solid in gas), vinaigrette (liquid in liquid), mud (solid in liquid), sand (solids blended together), and granite (blended solids). Examples That Are Not Mixtures Just because you mix two chemicals together, dont expect youll always get a mixture! If a chemical reaction occurs, the identity of a reactant changes. This is not a mixture. Combining vinegar and baking soda results in a reaction to produce carbon dioxide and water. So, you dont have a mixture. Combining an acid and a base also does not produce a mixture. Sources De Paula, Julio; Atkins, P. W.  Atkins Physical Chemistry  (7th ed.).Petrucci R. H., Harwood W. S., Herring F. G. (2002).  General Chemistry, 8th Ed. New York: Prentice-Hall.Weast R. C., Ed. (1990).  CRC Handbook of chemistry and physics. Boca Raton: Chemical Rubber Publishing Company.Whitten K.W., Gailey K. D. and Davis R. E. (1992).  General chemistry, 4th Ed. Philadelphia: Saunders College Publishing.