How Do The Social Media Affect Our Culture Media Essay

How Do The Social Media Affect Our Culture Media Essay Ill just quickly go to Erics house to see if Erics Home, and ask what hes doing tonight. I hope that Monica is not involved with Eric, although I often see her talking to that guy. Or shall I call Amber, because I heard she likes me. That was a typical youngster life about 50 years ago. When you wanted to talk to someone, you went to him or her, or gave them a phone call. That was our way of interacting with people in our culture back then. Quickly looking if Eric has posted something this night on Twitter. Hoping that Monica isnt doing something this evening, although she often sends messages to that guy on Facebook. Or shall I talk to Amber on Facebook chat? She likes all my pictures, maybe she fancies me? This is a more modern approach which we would use nowadays. Just compare the two examples, and you see the big difference. Therefore we can ask ourselves the question: Are we connected better nowadays with social media, or are we worse off? ~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~ Our culture has norms and values. It makes us who we are, what we feel connected to and how we behave. One of the aspects of culture is social interaction between people. How we behave to one another and in which way we do that. Social media has taken a big role in our social interaction. We no longer have to speak to a person to know what they are doing. We just look on twitter of Facebook. Or we give them a quick message on MSN or Whatsapp. This leads to less real-life or physical contact. This could be seen in a negative and in a positive way. The real connection such as visual and emotional expressions arent shown anymore, because you both look at a computerized display. This way messages could be understood differently than they should be, because they dont get to know the real meaning behind the message. Social media can create a gap between generations. The majority of social media users are teenagers or young adults. [fact1: 50% of the world population is under 30 years of age] Although more and more people start to use this type of media, it are especially younger people who start using social media, not adults. People who are for example 50 years or older do have trouble to keep updated with all modern technology like computers, not even mentioning the social media use on these computers. We dont have a choice on whether we DO social media, the question is how well DO it Erik Qualman Social media can also be dangerous. That might sound odd, but you all might have experienced the dangers of social media before. When you posted something on Facebook or Twitter, and after that you regret that you made that post. Thats a negative side of internet. We all have to be careful now with what we do or what we say. When things are put on the internet, it can stay there forever. When there was no internet, words that were said would just be forgotten after a certain time, and people couldnt copy it. Now with social media, messages can be copied, duplicated and spread so easily that you really have to be careful with what you say. Your privacy can also be put to the test by showing and sharing all the things you do. People know what you are doing, where you are and what your status is. [fact1: there are over 110 million updates posted on Facebook and Twitter every day] Many people dont do anything with it, but some will use that information for purposes you dont want them to use. So called leaking info can also be dangerous. For example in important negations or other meetings, there have been multiple people who accidentally leaked important and secret information which were shown in such meetings. There are other things important too for our culture. Our very own Dutch language for example. Its used less and less on social media. This is due to the globalization and English being used more and more often as an lingua franca. [fact1: if Facebook were a country, it would be worlds 3rd largest country in terms of population] Nowadays you see and increasing use of English: English quotes, abbreviations (brb = be right back, omwt = on my way to.. and ftw = for the win) or complete English sentences. There are multiple reasons for this: English sounds a lot cooler than some Dutch words. Some jokes are only funny in English or you have an audience in mind that doesnt speak your language, but who do speak English. Social media is not only negative. On the other hand contact is made easier, because you have a sort of safety behind your computer or mobile phone. Nobody sees you. You can act out who you want (remember though: this can be deceiving too). You also make contact easier via social media. Many people prefer a message via internet on e.g. Facebook or Twitter than giving them a call or go by and visit them. People are usually more shy in public. Therefore you can say that there could be more social interaction between people, and a reason for that contact is made easier than before. Social media invites people to write more messages, updates or other messaging. You have to keep updated by reading your friends updates, but you have to post what you are doing too; making dinner, going to the beach or just going to sleep. [fact1: visiting social sites is now more popular than checking personal email] It reaches all your updated friends on social media, so the message you sent is multiplied dozens of times. Its like give a speech to a huge square filled with people. The only difference with that speech is that social media messaging happens every minute, those speeches only take place a certain amount of times in a year, because not everybody wants to group-up too often. Focus on how to BE social, not how to DO social Jay Baer Social Media are sometimes called the biggest shift since the industrial revolution. We all notice that social media has turned into something really big. Some use it more often than others, but our culture has changed. There is now more contact via internet. Will this in the end kill our social cohesion and will groups of people be left out? Or will our social interaction become extensive and will our relationships get better? These are all questions which cant be answered yet and can only be answered in the future. The thing we do know is that how social media changes our culture is all in our hands; how we deal with it. Be careful with what you do on social media, because before you know it, social media can blow it. It is a great gift though, and with proper and with humble use, we all can enjoy the use of it; whether Monica is doing something tonight or if Amber is really into me.. -Ivo Brouwer

Chemistry thermo lab, Hess’s Law Essay

Introduction: In this lab, we will be determining the change in enthalpy for the combustion reaction of magnesium (Mg) using Hess’s law. Procedure: 1. React about 100 mL of 1.00 M hydrochloric acid with 0.80 g of MgO. Note the change in temperature and any qualitative data. 2. React about 100 mL of 1.00 M hydrochloric acid with 0.50 g of Mg. Note the change in temperature and any qualitative data. Raw Data: Quantitative: Reaction, trial Mass ( ± 0.01 g) Initial temperature ( ± 0.1à ¢Ã‚ ° C) Final temperature ( ± 0.1à ¢Ã‚ ° C) Volume of HCl ( ± 0.05 mL) Reaction 1, Trial 1 0.80 22.0 26.9 100.00 Reaction 1, Trial 2 0.80 22.2 26.9 100.00 Reaction 2, Trial 1 0.50 21.6 44.4 100.00 Reaction 2, Trial 2 0.50 21.8 43.8 100.00 Qualitative: 1. Hydrochloric acid is colorless and odorless 2. Magnesium tape is shiny after cleaning it from oxidants, increasing its purity. 3. In both reactions, the solution became bubbly. 4. There was a strong odor from the reaction. Data Processing: Trial 1: Reaction 1: First, we have to calculate the ΔT by subtracting the final temperature by initial temperature: 1. 2. 3. Now we calculate the mass of the solution, assuming it has the density as water: 1. 2. 3. 4. Now, we can use q=mc ΔT to calculate the energy gained by the solution: 1. 2. 3. Therefore: 1. Now, we have to calculate the number of moles for MgO: 1. 2. 3. We can now calculate the change in enthalpy by dividing the q of the reaction by the moles of the limiting reagent: 1. Now, we do reaction 2, trial 1 so we can use Hess’s law to calculate the change in enthalpy of formation, but first we are going to calculate the uncertainty in this expression: First, we calculate the uncertainty for the: 1. 2. 3. Now for mass: 1. 2. As for the energy gained: 1. 2. Now for the energy of the reaction: 1. It is multiplied by an integer (-1) so it is the same unc. As for the moles: 1. 2. Finally, the change in enthalpy: 1. 2. 3. Reaction 2: First, we have to calculate the ΔT by subtracting the final temperature by initial temperature: 1. 2. Now we calculate the mass of the solution, assuming it has the density as water: 1. 2. 3. Now, we can use q=mc ΔT to calculate the energy gained by the solution: 1. 2. Therefore: 1. Now, we have to calculate the number of moles for MgO: 1. 2. We can now calculate the change in enthalpy by dividing the q of the reaction by the moles of the limiting reagent: 1. I will now calculate the uncertainties: First, we calculate the uncertainty for the: 1. 2. Now for mass: 1. 2. As for the energy gained: 1. 2. Now for the energy of the reaction: 1. It is multiplied by an integer (-1) so it is the same unc. As for the moles: 1. 2. Finally, the change in enthalpy: 1. 2. 3. Now, we use Hess’s law to calculate the change of enthalpy of formation: 1. MgO(s) + 2HCl(aq) MgCl2(aq) + H2O(l) 2. Mg (s) + 2HCl(aq) MgCl2(aq) + H2 (g) 3. H2(g) + 0.5 O2(g) H2O(l) (given) By reversing reaction number 1, we can get our targeted reaction: Mg (s) + 0.5 O2(g) MgO(s) Now to calculate the change of enthalpy, which will be the change of enthalpy of formation? 1. 2. Our final result is: 1. Mg (s) + 0.5 O2(g) MgO(s) Random error and percent error: We can calculate the random error by just adding the random errors of the component reactions: 1. 2. 3. As for the percent error: 1. 2. 3. Trial 2: Reaction 1: First, we have to calculate the ΔT by subtracting the final temperature by initial temperature: 1. 2. Now we calculate the mass of the solution, assuming it has the density as water: 1. 2. 3. Now, we can use q=mc ΔT to calculate the energy gained by the solution: 1. 2. 3. Therefore: 1. Now, we have to calculate the number of moles for MgO: 1. 2. 3. We can now calculate the change in enthalpy by dividing the q of the reaction by the moles of the limiting reagent: 1. Now, we do reaction 2, trial 1 so we can use Hess’s law to calculate the change in enthalpy of formation, but first we are going to calculate the uncertainty in this expression: First, we calculate the uncertainty for the: 1. 2. 3. Now for mass: 1. 2. As for the energy gained: 1. 2. Now for the energy of the reaction: 1. It is multiplied by an integer (-1) so it is the same unc. As for the moles: 1. 2. Finally, the change in enthalpy: 1. 2. 3. Reaction 2: First, we have to calculate the ΔT by subtracting the final temperature by initial temperature: 1. 2. Now we calculate the mass of the solution, assuming it has the density as water: 1. 2. 3. Now, we can use q=mc ΔT to calculate the energy gained by the solution: 1. 2. Therefore: 1. Now, we have to calculate the number of moles for MgO: 1. 2. We can now calculate the change in enthalpy by dividing the q of the reaction by the moles of the limiting reagent: 1. I will now calculate the uncertainties: First, we calculate the uncertainty for the: 1. 2. Now for mass: 1. 2. As for the energy gained: 1. 2. Now for the energy of the reaction: 1. It is multiplied by an integer (-1) so it is the same unc. As for the moles: 1. 2. Finally, the change in enthalpy: 1. 2. 3. Now to calculate the change of enthalpy, which will be the change of enthalpy of formation: 1. 2. Our final result is: 1. Mg (s) + 0.5 O2(g) MgO(s) Random error and percent error: We can calculate the random error by just adding the random errors of the component reactions: 1. 2. 3. As for the percent error: 1. 2. 3. Processed data: Trial 1 Trial 2 of reaction 1 -104 kJ/mol ( ± 2.10%) -99 kJ/mol ( ± 2.19%) of reaction 2 -463 kJ/mol ( ± 0.509%) -446 kJ/mol ( ± 0.525%) of MgO -645 kJ/mol ( ± 2.61%) -633 kJ/mol ( ± 2.72%) Conclusion and Evaluation: In this lab, we determined the standard enthalpy change of formation of MgO using Hess’s law. First, we reacted HCl with MgO for the first reaction and got -104 kJ/mol ( ± 2.10%) for trial 1 and -99 kJ/mol ( ± 2.19%) for trial 2. As for reaction 2, where you react, I got -463 kJ/mol ( ± 0.509%) for trial 1 and -446 kJ/mol ( ± 0.525%) for trial 2. When we use Hess’s Law, we have to reverse reaction 1 to get the targeted equation, Mg (s) + 0.5 O2(g) MgO(s), and we get an enthalpy change value of -645 kJ/mol ( ± 2.61%) for trial 1, and -633 kJ/mol ( ± 2.72%) for trial 2. For trial 1, my value got a percent error of 7.14%, which is not that bad considering the weaknesses this lab had that will be discussed in the evaluation. However, in trial 2, I got a better percent error, which is 5.15%, we got a better value because we had a bigger ΔH values thus when adding them (since one of them is positive and the other two is negative) we get a smaller value for the enthalpy change of formation thus bringing us closer to the theoretical value. The biggest weakness in this lab was the impurity of the substances, the assumptions that we made about the HCl solution, for example, we assumed that the specific heat capacity of the solution is the same as water, which is an assumption that is not a 100% accurate and affected our ΔH values for both reactions and eventually our final ΔHf value. To fix this, In the different range of specific heat capacity values, 4.10 j/g k would have been more appropriate to get closer to our theoretical values, as you get a bigger qrxn values thus bigger ΔH values. Another thing that I noticed is that the theoretical value that I got was the â€Å"Standard† enthalpy change of formation. Standard meaning at standard conditions which are at 293 K and 101.3 kPa for pressure. These weren’t the conditions in the lab when I did the experiment. This might alter the experimental value closer to the theoretical value reducing the percent error.

Hofstra University Acceptance Rate, SAT/ACT Scores, GPA

Hofstra University is a private university with an acceptance rate of 63%. The 240-acre campus is located in Hempstead, Long Island, within easy reach of New York City. The university has a 13-to-1  student / faculty ratio  and an average class size of 20. Campus life is active, and Hofstra has over 200 student clubs and organizations including an active Greek system. Business majors are popular among undergraduates, but Hofstras strengths in the liberal arts and sciences earned the school a chapter of  Phi Beta Kappa. On the athletic front, the Hofstra Pride competes in the NCAA Division I  Colonial Athletic Association. Popular sports include basketball, track and field, soccer, lacrosse, and field hockey. Considering applying to Hofstra University? Here are the admissions statistics you should know, including average SAT/ACT scores and GPAs of admitted students. Acceptance Rate During the 2017-18 admissions cycle, Hofstra University had an acceptance rate of 63%. This means that for every 100 students who applied, 63 students were admitted, making Hofstras admissions process competitive. Admissions Statistics (2017-18) Number of Applicants 27,620 Percent Admitted 63% Percent Admitted Who Enrolled (Yield) 9% SAT Scores and Requirements Hofstra University has a test-optional standardized testing policy for most applicants. Applicants to Hofstra may submit SAT or ACT scores to the school, but they are not required.  During the 2017-18 admissions cycle, 70% of admitted students submitted SAT scores. SAT Range (Admitted Students) Section 25th Percentile 75th Percentile ERW 580 660 Math 570 670 ERW=Evidence-Based Reading and Writing This admissions data tells us that of those students who submitted scores during the 2017-18 admissions cycle, most of Hofstras admitted students fall within the top 35% nationally on the SAT. For the evidence-based reading and writing section, 50% of students admitted to Hofstra scored between 580 and 660, while 25% scored below 580 and 25% scored above 660. On the math section, 50% of admitted students scored between 570 and 670, while 25% scored below 570 and 25% scored above 670. While the SAT is not required, this data tells us that a composite SAT score of 1330 or higher is competitive for Hofstra University. Requirements Hofstra University does not require SAT scores for admission for most applicants. For students who choose to submit scores, note that Hofstra participates in the scorechoice program, meaning that the admissions office will consider your highest score from each individual section across all SAT test dates. Hofstra recommends that students include the essay portion of the SAT. Note that applicants to particular programs (e.g. Hofstras dual degree physician assistant program and the BS-BA/MD program), home schooled applicants, international students, and students applying for the Hofstra Trustee Scholarship, are required to submit standardized test scores. ACT Scores and Requirements Hofstra University has a test-optional standardized testing policy for most applicants. Applicants to Hofstra may submit SAT or ACT scores to the school, but they are not required.  During the 2017-18 admissions cycle, 29% of admitted students submitted ACT scores. ACT Range (Admitted Students) Section 25th Percentile 75th Percentile English 24 31 Math 24 28 Composite 24 30 This admissions data tells us that of those who submitted scores during the 2017-18 admissions cycle, most of Hofstras admitted students fall within the  top 26% nationally  on the ACT. The middle 50% of students admitted to Hofstra received a composite ACT score between 24 and 30, while 25% scored above 30 and 25% scored below 24. Requirements Note that Hofstra does not require ACT scores for admission for most applicants. For students who choose to submit scores, Hofstra superscores ACT results; your highest subscores from multiple ACT sittings will be considered. Hofstra recommends that students submit the ACT writing section. Note that applicants to particular programs (e.g. Hofstras dual degree physician assistant program and the BS-BA/MD program), home schooled applicants, international students, and students applying for the Hofstra Trustee Scholarship, are required to submit standardized test scores. GPA In 2018, the average high school GPA of Hofstras incoming class was 3.64, and over 90% of students had GPAs of 3.0 and above. These results suggest that most successful applicants to Hofstra University have primarily A and B grades. Self-Reported GPA/SAT/ACT Graph Hofstra University Applicants Self-Reported GPA/SAT/ACT Graph. Data courtesy of Cappex. The admissions data in the graph is self-reported by applicants to Hofstra University. GPAs are unweighted. Find out how you compare to accepted students, see the real-time graph, and calculate your chances of getting in  with a free Cappex account. Admissions Chances Hofstra University, which accepts fewer than two-thirds of applicants, has selective admissions. However, Hofstra also has a  holistic admissions  process and is test-optional, and admissions decisions are based on more than numbers. A strong  application essay  and  glowing letters of recommendation  can strengthen your application, as can participation in meaningful  extracurricular activities  and a  rigorous course schedule. The college is looking for students who will contribute to the campus community in meaningful ways, not just students who show promise in the classroom. Students with particularly compelling stories or achievements can still receive serious consideration even if their grades and scores are outside of Hofstras average range. In the graph above, the blue and green dots represent accepted students. Most admitted students had a high school average of B or better, a combined SAT score of 1050 or higher (ERWM), and an ACT composite score of 23  or higher. Grades are much more important than standardized test scores due to Hofstras test-optional admissions policy. If You Like Hofstra University, You May Also Like These Schools Stony Brook UniversityDrexel UniversityIthaca CollegeTemple UniversityNew York UniversityPennsylvania State UniversitySyracuse UniversityPace UniversityBoston University All admissions data has been sourced from the National Center for Education Statistics and Hofstra University Undergraduate Admissions Office.

Walts Whitmans Vision of America in Leaves of Grass

Walt Whitman’s vision of America in Leaves of Grass Valentine†©Abbet†© TRAVAIL†©DE†©MATURITE†© Sous†©la†©direction†©d’Anne†©Roland†Wurzburger†© Gymnase†©du†©Bugnon,†©Lausanne†© 2012†©  «I have sung the body and the soul, war and peace have I sung, and the songs of life and death, And the songs of birth, and shown that there are many births. I have offerd my style to every one, I have journeyd with confident step; While my pleasure is yet at the full I whisper So long! » Walt Whitman, So Long !, Deathbed edition (1892) 2 Walt†©Whitman’s†©vision†©of†©America†©in†©Leaves†©of†©Grass†© Contents†© I. Introduction†©Ã¢â‚¬ ¦Ã¢â‚¬ ¦Ã¢â‚¬ ¦Ã¢â‚¬ ¦Ã¢â‚¬ ¦Ã¢â‚¬ ¦Ã¢â‚¬ ¦Ã¢â‚¬ ¦Ã¢â‚¬ ¦Ã¢â‚¬ ¦Ã¢â‚¬ ¦Ã¢â‚¬ ¦Ã¢â‚¬ ¦Ã¢â‚¬ ¦Ã¢â‚¬ ¦Ã¢â‚¬ ¦Ã¢â‚¬ ¦Ã¢â‚¬ ¦Ã¢â‚¬ ¦Ã¢â‚¬ ¦Ã¢â‚¬ ¦Ã¢â‚¬ ¦Ã¢â‚¬ ¦Ã¢â‚¬ ¦Ã¢â‚¬ ¦Ã¢â‚¬ ¦Ã¢â‚¬ ¦Ã¢â‚¬ ¦.†©4†© Starting†©point†©Ã¢â‚¬ ¦Ã¢â‚¬ ¦Ã¢â‚¬ ¦Ã¢â‚¬ ¦Ã¢â‚¬ ¦Ã¢â‚¬ ¦Ã¢â‚¬ ¦Ã¢â‚¬ ¦Ã¢â‚¬ ¦Ã¢â‚¬ ¦Ã¢â‚¬ ¦Ã¢â‚¬ ¦Ã¢â‚¬ ¦Ã¢â‚¬ ¦Ã¢â‚¬ ¦Ã¢â‚¬ ¦Ã¢â‚¬ ¦Ã¢â‚¬ ¦Ã¢â‚¬ ¦..†¦Ã¢â‚¬ ¦Ã¢â‚¬ ¦Ã¢â‚¬ ¦..†¦Ã¢â‚¬ ¦.†¦.†©4†© Short†©biography†©Ã¢â‚¬ ¦Ã¢â‚¬ ¦Ã¢â‚¬ ¦Ã¢â‚¬ ¦Ã¢â‚¬ ¦Ã¢â‚¬ ¦Ã¢â‚¬ ¦Ã¢â‚¬ ¦Ã¢â‚¬ ¦Ã¢â‚¬ ¦Ã¢â‚¬ ¦Ã¢â‚¬ ¦Ã¢â‚¬ ¦Ã¢â‚¬ ¦Ã¢â‚¬ ¦Ã¢â‚¬ ¦Ã¢â‚¬ ¦Ã¢â‚¬ ¦Ã¢â‚¬ ¦Ã¢â‚¬ ¦Ã¢â‚¬ ¦Ã¢â‚¬ ¦Ã¢â‚¬ ¦Ã¢â‚¬ ¦Ã¢â‚¬ ¦Ã¢â‚¬ ¦.†©5†© Historical†¦show more content†¦Toward†© the†© end†© of†© his†© life,†© he†© became†© more†© skeptical†© about†© how†© things†© were†© going†© to†© turn†© out,†© which†© is†© why†© he†© tri ed†© to†© reach†© out†© to†© the†© future†© generations.†©Nevertheless,†©unlike†©other†©poets†©of†©the†©the†©same†©era†©who†©lost†©faith†©in†©man’s†© capacity†©to†©change†©like†©Ralph†©Waldo†©Emerson2,†©Walt†©Whitman†©never†©became†©cynical.†©On†© the†© contrary†© he†© hoped†© for†© the†© next†© generations†© to†© be†© able†© to†© carry†© on†© his†© ideas†© and†© perhaps†©even†©understand†©them†©better.†© I†©think†©that†©Walt†©Whitman†©was†©definitely†©a†©poet†©of†©the†©future,†©not†©only†©because†©of†©his†© new†©way†©of†©seeing†©poetry†©but†©also†©because†©his†©ideasà ¢â‚¬ ©about†©what†©a†©country†©and†©its†©people†© should†©be†©like†©were†©groundbreaking†©and†©modern.†©However,†©the†©America†©of†©today†©doesn’t†© exactly†© meet†© the†© poet’s†© expectations†© in†© matters†© such†© as†© justice†© and†© rights†© for†© the†© individuals,†© as†© well†© as†© where†© people’s†© concerns†© lay†© (keeping†© a†© thriving†© economy,†© engaging†©in†©warfare,†©etc.).†©Ã¢â‚¬ © In†©this†©work,†©I†©tried†©to†©give†©an†©overview†©of†©his†©relationship†©with†©his†©country;†©one†©that†© can†© be†© understood†© through†© several†© of†© his†© poems.†© I†© divided†© t he†© main†© theme†© into†© four†© minor†© themes†© and†© for†© each†© one†© of†© them,†© I†© chose†© three†© pieces†© of†© poetry†© I†© thought†© expressed†© it†© best.†© The†© poems†© appear†© in†© this†© order†© either†© according†© to†© their†© dates†© of†© publication,†©or†©for†©the†©sake†©of†©consistency.†©Ã¢â‚¬ © III.†©Short†©biography†© WaltShow MoreRelatedAllen Ginsberg, A Supermarket in California Literary Analysis1669 Words   |  7 PagesJasamyn Wimmer English 1B Professor Kleinman 5 March 2013 Brief Literary Analysis Lost America: An analysis of â€Å"A Supermarket in California† Allen Ginsberg; philosopher, activist, poet, a man highly revered as a groundbreaking figure between the 1950’s Beat Poetry Generation and the counter-cultural revolution of the 1960’s (poetryarchive.org). Ginsberg’s first book â€Å"Howl and Other Poems,† was published in 1955, his work was involved in an illustrious obscenity trial because of the use of