School Safety essays

School Safety essays In recent years, tragedies have been visited upon schools across the country. From Kentucky to Oregon to Colorado, the notion of schools as safe havens has been shattered by the sound of gunfire. These acts are not limited to any geographic regions or family backgrounds, nor do they have a single catalyst. Those who have committed such heinous acts have done so for different reasons, at different times, in different schools. But these acts of school violence have at least one thing in common- they have spurred all of us to take a look at what can be done to better protect children and teachers at school. Protecting our children is not simply a matter of public policy. It is a matter of strengthening basic values, of teaching children right from wrong, of instilling in them respect for others. We each have a responsibility to work to end youth violence and to keep schools safe for children and for those who teach them. Youth violence in many schools has reached universal proportions. It is not only happening in our high schools, it has also made its way into our elementary and middle schools. Everyone seems to have a different perspective on why there is such a problem with school safety. Some say it is the parents fault, some say it is the media, and others blame the schools. Yet, the question still remains. What can be done to make schools safer for the children and staff? One thing we need to do is learn to listen to our children and observe their behavior. According to Dr. Ronald D. Stephens, Executive Director of the National School Safety Center, there are some common characteristics among youth who have caused school- associated violent deaths. Accounts of these tragic incidents repeatedly indicate that in most cases, a troubled youth has demonstrated or has talked about problems with bullying and feelings of isolation, anger, depression, and frustration. Some of the characteristics that Dr. Stephens provides on his che...

Boyles Law Worked Sample Chemistry Problem

Boyle's Law Worked Sample Chemistry Problem If you trap a sample of air and measure its volume at different pressures (constant temperature), then you can determine a relation between volume and pressure. If you do this experiment, you will find that as the pressure of a gas sample increases, its volume decreases. In other words, the volume of a gas sample at constant temperature is inversely proportional to its pressure. The product of the pressure multiplied by the volume is a constant: PV k or V k/P or P k/V where P is pressure, V is volume, k is a constant, and the temperature and quantity of gas are held constant. This relationship is called Boyles Law, after Robert Boyle, who discovered it in 1660. Key Takeaways: Boyle's Law Chemistry Problems Simply put, Boyles states that for a gas at constant temperature, pressure multiplied by volume is a constant value. The equation for this is PV k, where k is a constant.At a constant temperature, if you increase the pressure of a gas, its volume decreases. If you increase its volume, the pressure decreases.The volume of a gas is inversely proportional to its pressure.Boyles law is a form of the Ideal Gas Law. At normal temperatures and pressures, it works well for real gases. However, at high temperature or pressure, it is not a valid approximation. Worked Example Problem The sections on the General Properties of Gases and Ideal Gas Law Problems may also be helpful when attempting to work Boyles Law problems. Problem A sample of helium gas at 25Â °C is compressed from 200 cm3 to 0.240 cm3. Its pressure is now 3.00 cm Hg. What was the original pressure of the helium? Solution Its always a good idea to write down the values of all known variables, indicating whether the values are for initial or final states. Boyles Law problems are essentially special cases of the Ideal Gas Law: Initial: P1 ?; V1 200 cm3; n1 n; T1 T Final: P2 3.00 cm Hg; V2 0.240 cm3; n2 n; T2 T P1V1 nRT (Ideal Gas Law) P2V2 nRT so, P1V1 P2V2 P1 P2V2/V1 P1 3.00 cm Hg x 0.240 cm3/200 cm3 P1 3.60 x 10-3 cm Hg Did you notice that the units for the pressure are in cm Hg? You may wish to convert this to a more common unit, such as millimeters of mercury, atmospheres, or pascals. 3.60 x 10-3 Hg x 10mm/1 cm 3.60 x 10-2 mm Hg 3.60 x 10-3 Hg x 1 atm/76.0 cm Hg 4.74 x 10-5 atm Source Levine, Ira N. (1978). Physical Chemistry. University of Brooklyn: McGraw-Hill.