Critical Mistakes to Avoid While Writing Actuarial Science Personal Statement Essays

Critical Mistakes to Avoid While Writing Actuarial Science Personal Statement Essays Critical Mistakes to Avoid While Writing Actuarial Science Personal Statement Essay Critical Mistakes to Avoid While Writing Actuarial Science Personal Statement Essay Actuarial science is the study of appraising risk factors in the finance or insurance industry. The actuaries calculate the risk by using certain mathematical or statistical methodologies. Students who are pursuing this field have to take care of personal statement writing during taking admission in a university for an advance program such as Masters. These days, getting into a prominent university has become difficult than ever. When students apply to any university they are contending against other bright students but only few can avail the limited seats in the university, while the rest have to look for another academia. The personal statement is the only thing that helps the academia in evaluating which applicant is best suited for the program and for the university. Aside from your undergraduate grades, you can convince the admission officers of the university that you deserve a seat in the university by writing a single page but appealing actuarial science personal statement. However, there are certain critical mistakes that every applicant must avoid to solidify their chances of getting into their dream university. Critical Mistakes First of all, never think that the personal statement is an essay or an autobiography. But think it as a marketing statement which you use to market yourself or sell yourself to the university. Keep in mind that this single page statement is the only thing that can help you in distinguishing yourself from other qualified applicants. You can think of it as a product and consider yourself as a marketing agent whose job is to make the audience – the admission officers – want to buy the product, which in this case is YOU. Majority of students don’t make the most from the statement because they don’t highlight their strengths and positive qualities in it. They don’t sell their accomplishments or achievements as they think it as bragging. Remember that every big or little accomplishment which you have worked hard to achieve must be included in the statement. Many students also fail to address the weaknesses in their academic performance or record. Keep in mind that admission officers look for reasons why the applicant has inconsistencies in his/her record. If you don’t address it effectively the admission committee will assume that the applicant doesn’t care and in the end your applicant will most likely be rejected. Students tend to make mistakes while writing any manuscript. However, those grammatical or spelling mistakes can be corrected if proofread thoroughly. Remember that failure to proofread is the most critical mistake that can reject your application no matter how hard you have worked on it. Consider these critical mistakes and try to avoid them as much as possible.

Arrhenius Equation Formula and Example

Arrhenius Equation Formula and Example In 1889, Svante Arrhenius formulated the Arrhenius equation, which relates reaction rate to temperature. A broad generalization of the Arrhenius equation is to say the reaction rate for many chemical reactions doubles for every increase in 10 degrees Celsius or Kelvin. While this rule of thumb isnt always accurate, keeping it in mind is a good way to check whether a calculation made using the Arrhenius equation is reasonable. Formula There are two common forms of the Arrhenius equation. Which one you use depends on whether you have an activation energy in terms of energy per mole (as in chemistry) or energy per molecule (more common in physics). The equations are essentially the same, but the units are different. The Arrhenius equation as its used in chemistry is often stated according to the formula: k Ae-Ea/(RT) k is the rate constantA is an exponential factor that is a constant for a given chemical reaction, relating the frequency of collisions of particlesEa is the activation energy of the reaction (usually given in Joules per mole or J/mol)R is the universal gas constantT is the absolute temperature (in Kelvins) In physics, the more common form of the equation is: k Ae-Ea/(KBT) k, A, and T are the same as beforeEa is the activation energy of the chemical reaction in JouleskB is the Boltzmann constant In both forms of the equation, the units of A are the same as those of the rate constant. The units vary according to the order of the reaction. In a first-order reaction, A has units of per second (s-1), so it may also be called the frequency factor. The constant k is the number of collisions between particles that produce a reaction per second, while A is the number of collisions per second (which may or may not result in a reaction) that are in the proper orientation for a reaction to occur. For most calculations, the temperature change is small enough that the activation energy is not dependent on temperature. In other words, its usually not necessary to know the activation energy to compare the effect of temperature on reaction rate. This makes the math much simpler. From examining the equation, it should be apparent the rate of a chemical reaction may be increased by either increasing the temperature of a reaction or by decreasing its activation energy. This is why catalysts speed up reactions! Example Find the rate coefficient at 273 K for the decomposition of nitrogen dioxide, which has the reaction: 2NO2(g) → 2NO(g) O2(g) You are given that the activation energy of the reaction is 111 kJ/mol, the rate coefficient is 1.0 x 10-10 s-1, and the value of R is 8.314 x 10-3 kJ mol-1K-1. In order to solve the problem, you need to assume A and Ea dont vary significantly with temperature. (A small deviation might be mentioned in an error analysis, if you are asked to identify sources of error.) With these assumptions, you can calculation the value of A at 300 K. Once you have A, you can plug it into the equation to solve for k at the temperature of 273 K. Start by setting up the initial calculation: k Ae-Ea/RT 1.0 x 10-10 s-1 Ae(-111 kJ/mol)/(8.314 x 10-3 kJ mol-1K-1)(300K) Use your scientific calculator to solve for A and then plug in the value for the new temperature. To check your work, notice the temperature decreased by nearly 20 degrees, so the reaction should only be about a fourth as fast (decreased by about half for every 10 degrees). Avoiding Mistakes in Calculations The most common errors made in performing calculations are using constant that have different units from each other and forgetting to convert Celsius (or Fahrenheit) temperature to Kelvin. Its also a good idea to keep the number of significant digits in mind when reporting answers. Arrhenius Plot Taking the natural logarithm of the Arrhenius equation and rearranging the terms yields an equation that has the same form as the equation of a straight line (y mxb): ln(k) -Ea/R (1/T) ln(A) In this case, the x of the line equation is the reciprocal of absolute temperature (1/T). So, when data is taken on the rate of a chemical reaction, a plot of ln(k) versus 1/T produces a straight line. The gradient or slope of the line and its intercept can be used to determine the exponential factor A and the activation energy Ea. This is a common experiment when studying chemical kinetics.