Washington essays

Washington essays George Washington is best known as the first president of the United States, and a man of moral fortitude with his famous cherry tree legend. However, there is much more to Washingtons extensive character and contribution that give him the legacy of being, perhaps the most influential leader in the creation of the American nation. Through his achievements as commander-in-chief during the Revolution, in support of the drafting and ratification of the Constitution, and as first president, Washington was instrumental in transforming the ideals of the Revolution into reality. His career as soldier, revolutionary, constitution-maker, and chief executive of a new nation demanded a range of skills and talents with few precedents in history. Washington proved himself to be a firm, dignified, conscientious, yet cautious president. He did not want the central government to become too strong and meticulously avoided getting too involved with Congress, since he was a firm believer of separation of powers. In addition he was not biased or prejudice against any faction of the parties. He also always tried to commit every action with proper reason, and to set a precedent with each action for the presidents that would hold office after him. He did not believe in pushing or proposing any legislation or anything that undemocratic, or unconstitutional. Washington, along with others help then was able to stabilize the government after the adoption of the Constitution. One of the precedents that Washington established was The Presidential Cabinet, which was later used by future presidents as well. Whenever, he had any doubts about a decision he would consult his cabinet, an assembly that he himself chose. While appointing the members of the Cabinet, Washington did not favor any faction of a party, and assigned several positions to different political people. He gave Alexander Hamilton the position of Secretary of Treasury, who was confer...

Percent Yield Definition and Formula

Percent Yield Definition and Formula Percent yield is the percent ratio of actual yield to the theoretical yield. It is calculated to be the experimental yield divided by theoretical yield multiplied by 100%. If the actual and theoretical yield ​are the same, the percent yield is 100%. Usually, percent yield is lower than 100% because the actual yield is often less than the theoretical value. Reasons for this can include incomplete or competing reactions and loss of sample during recovery. Its possible for percent yield to be over 100%, which means more sample was recovered from a reaction than predicted. This can happen when other reactions were occurring that also formed the product. It can also be a source of error if the excess is due to incomplete removal of water or other impurities from the sample. Percent yield is always a positive value. Also Known As: percentage yield Percent Yield Formula The equation for percent yield is: percent yield (actual yield/theoretical yield) x 100% Where: actual yield is the amount of product obtained from a chemical reactiontheoretical yield is the amount of product obtained from the stoichiometric or balanced equation, using the limiting reactant to determine product Units for both actual and theoretical yield need to be the same (moles or grams). Example Percent Yield Calculation For example, the decomposition of magnesium carbonate forms 15 grams of magnesium oxide in an experiment. The theoretical yield is known to be 19 grams. What is the percent yield of magnesium oxide? MgCO3 → MgO CO2 The calculation is simple if you know the actual and theoretical yields. All you need to do is plug the values into the formula: percent yield actual yield / theoretical yield x 100% percent yield 15 g / 19 g x 100% percent yield 79% Usually, you have to calculate the theoretical yield based on the balanced equation. In this equation, the reactant and the product have a 1:1 mole ratio, so if you know the amount of reactant, you know the theoretical yield is the same value in moles (not grams!). You take the number of grams of reactant you have, convert it to moles, and then use this number of moles to find out how many grams of product to expect.