Use Games to Improve Your SAT Score

Have Some Fun and Prep for the SAT With These Games When it comes to improving SAT scores, there's no substitute for comprehensive test prep. However, thereareactivities you can do outside of studying to help reframe how you approach certain test problems and concepts. Games in particularare an excellent way to practice setting and achievinggoals, as well as problem solving under pressure. SAT or ACT prep can become boring and exhausting pretty quickly if students aren’t able to switch up their approach every now and then. Especially if students are just working through and endless series of problems, or taking excessive practice tests, they can quickly lose interest and motivation. This is a recipe for trouble, as students need to sustain their test prep throughout their testing timeline in order to reach their goal scores. This is where introducing some new and fun study activities can be extremely useful. If you are looking to spice up your studying routine, try these activities to help sharpen your test-taking mindset. Crack Open a Copy ofWhere's Waldo?Waldo is hidden among the morass of a Roman coliseum. There are red-and-white striped blankets draped everywhere. Characters like â€Å"Wenda† (Waldo's girlfriend) are dressed nearly identically to him. It can be overwhelming, but also surprisingly similar to the SAT’s Reading section, which is a mess of words and graphs cascading into one another. Certain multiple-choice options are phrased to appear to bealmost exactly correct—except for a single word or two that that makes them wrong. To excel, students need to learn to tune out the extraneous information and focus in on reference words that will steer them towards the answer they are looking for. Much like Waldo, the Reading Test is a puzzle book that is best solved by sharpening your ability to pay close attention to small details. Watch a Few Episodes ofWho Wants to Be a Millionaire?This game show offers more than fun trivia facts – it provides insight into how to successfully answer tricky multiple-choice questions. You’ll notice that successful contestants use each possible answer as a tool, weighing its individual likelihood instead of just trying to get the correct answer on the first guess. Learning to mentally talk through problems will help improve your efficiency and accuracy. Additionally, the concept of â€Å"lifelines† is a great one to bring into SAT preparation: â€Å"50:50,† in particular, demonstrates the usefulness of being able to increase your odds of selecting the correct answer byeliminating even just one or two incorrect responses. (Remember, there's no penalty for wrong guesses—don't leave any bubbles blank!) Kick Back withVideo Games or AppsGames likeBrain Age: Concentration Trainingfor the Nintendo 3DS and apps likeElevateare great supplements to SAT preparation. These games can help you prep for the â€Å"No Calculator† portion of the SAT's Math section bygiving you opportunities to drillyour arithmetic. Additionally, these games can boost your work on the Reading section by having you choose between commonly confused words or find the best fit for filling in a sentence. This kind of â€Å"brain-training† is fantastic forimproving memory,concentration, and the ability to perform under the pressure of a timed environment—all crucial skills for boosting SAT scores. Ultimately, the most effective way to improve your SAT score is through proper test preparation. But supplemental test prep doesn’t have to be boring or just drilling different problems day-in and day-out. By utilizing games and other creative strategies to liven up your test prep, you’re exercising your brain while also allowing it to recharge and take a break from more intensive test prep. Want to learn more about where you should be in the test prep process and how to get ahead? Download our free Academics and Test Prep Checklist below! //

Determination Of Heat Of Neutralization - Free Essay Example

PRACTICAL 15:DETERMINATION OF HEAT OF NEUTRALIZATION Data collection: |Reaction |Initial Temperature/ °C ( ±0. 25) |Final Temperature of Mixture/ °C ( ±0. 25) | | |Acid |Base | | |HNO3 + NaOH |28. 00 |28. 25 |34. 50 | |HNO3 + KOH |28. 25 |28. 25 |34. 00 | |HCl + NaOH |28. 25 |28. 00 |34. 5 | |HCl + KOH |28. 25 |28. 25 |34. 00 | |H2SO4 + NaOH |28. 00 |28. 50 |36. 50 | |H2SO4 + KOH |28. 50 |28. 00 |34. 00 | Volume of acid = 50 cm3  ± 0. 25 Acid concentration = 1. 0 M Volume of base = 50cm3  ± 0. 25 Base concentration = 1. 0 M Number of mole of solution used = [pic] = [pic] = 0. 05 mole  ± 0. 5 % Data Processing: Calculation: Temperature Change, [pic] = Final temperature – Average temperature of Acid and Base |Reaction |Average Temperature of Acid and Base,  °C|Final Temperature,  °C |Change of Temperature,  °C | | |( ±0. 5) |( ±0. 25) |( ±0. 75) | |HNO3 + NaOH |28. 13 |34. 50 |6. 38 | |HNO3 + KOH |28. 25 |34. 00 |5. 5 | |HCl + NaOH |28. 13 |34. 75 |6 . 63 | |HCl + KOH |28. 25 |34. 00 |5. 75 | |H2SO4 + NaOH |28. 25 |35. 00 |6. 75 | |H2SO4 + KOH |28. 25 |34. 00 |5. 75 | Heat Released, Q = [pic] m mass of solution specific heat of water (4. 2 Jmol-1 °C-1) [pic] temperature change of solution Enthalpy of neutralization, ? H = Heat released No of moles [pic]Enthalpy change of each experiment : 1. HNO3(aq) + NaOH(aq) [pic]NaNO3(aq) + H2O(l) Enthalpy of neutralization = [pic] = 53. 55 kJmol-1 Uncertainties: m = 0. 5 . ? 100= 0. 5 % 100 ?T = 0. 75 . ? 100= 11. 76 % 6. 38 no of moles= 0. 5 % Total= 12. 76 % Enthalpy of neutralization= -53. 55 kJmol-1 ± 12. 76 % 2. HNO3(aq) + NaOH(aq) [pic]NaNO3(aq) + H2O(l) Enthalpy of neutralization= [pic] = 48. 30 kJmol-1 Uncertainties: m = 0. 5 . 100= 0. 5 % 100 ?T = 0. 75 . ? 100= 13. 04 % 5. 75 no of moles= 0. 5 % Total= 14. 05 % Enthalpy of neutralization= -48. 30 kJmol-1  ± 14. 05 % 3. HCl(aq) + NaOH(aq) [pic]NaCl(aq) + H2O(l) Enthalpy of neutralization= [pic] = 55. 65 kJmol-1 Uncertainti es: m = 0. 5 . ? 100= 0. 5 % 100 ?T = 0. 75 . ? 100= 11. 31% 6. 63 no of moles= 0. 5 % Total= 12. 31 % Enthalpy of neutralization= -55. 65 kJmol-1  ± 12. 31 % 4. HCl(aq) + KOH(aq) [pic]KCl(aq) + H2O(l) Enthalpy of neutralization= [pic] = 48. 30 kJmol-1 Uncertainties: m = 0. 5 . ? 100= 0. 5 % 100 ?T = 0. 75 . ? 100= 13. 4 % 5. 75 no of moles= 0. 5 % Total= 14. 04 % Enthalpy of neutralization= -48. 30 kJmol-1  ± 14. 04 % 5. H2SO4(aq) + 2NaOH(aq) [pic] Na2SO4(aq) + 2H2O(l) Enthalpy of neutralization= [pic] = 56. 7 kJmol-1 Uncertainties: m = 0. 5 . ? 100= 0. 5 % 100 ?T = 0. 75 . ? 100= 11. 11 % 6. 75 no of moles= 0. 5 % Total= 12. 11 % Enthalpy of neutralization= -56. 7 kJmol-1  ± 12. 11 % 6. H2SO4(aq) + 2KOH(aq) [pic] K2SO4(aq) + 2H2O(l) Enthalpy of neutralization = [pic] = 48. 3 kJmol-1 Uncertainties: m = 0. 5 . ? 100= 0. 5 % 100 ?T = 0. 75 . ? 100= 13. 04 % 5. 75 no of moles= 0. % Total= 14. 04 % Enthalpy of neutralization= -48. 30 kJmol-1  ± 14. 04 % Calculated data: |Reacti on |? H, kJmol-1 | | |53. 55  ± 8. 84 % | |HNO3(aq) + NaOH(aq) NaNO3(aq) + H2O(l) | | | | | | |48. 30  ± 9. 0 % | |HNO3(aq) + NaOH(aq) NaNO3(aq) + H2O(l) | | | | | | |55. 65  ± 8. 54 % | |HCl(aq) + NaOH(aq) NaCl(aq) + H2O(l) | | | | | | |48. 0  ± 9. 70 % | |HCl(aq) + KOH(aq) KCl(aq) + H2O(l) | | | | | | |56. 70  ± 8. 1% | |H2SO4(aq) + 2NaOH(aq) Na2SO4(aq) + 2H2O(l) | | | | | | |48. 30  ± 9. 70 % | |H2SO4(aq) + 2KOH(aq) K2SO4(aq) + 2H2O(l) | | | | | Evaluation: Neutralization is an exothermic NeutralizationNeutralization as heat is released during the reaction. From the experiment, we can see that the enthalpy of neutralization of each reaction is nearly the same. This is because in each neutralization, the same reaction occur: OH- + H+ H2O The reaction can also be presented as: H3O+ + OH- 2H2O The theoretical value for the enthalpy of neutralization is about -57 kJmol-1. However, in this experiment, all values of neutralization enthalpy obtained are smaller than the theoretical ones. This is due to some weakness and limitation. Drawbacks of the experiment: 1. The styrofoam cup used was not closed. As a result, heat can be transfer to the surrounding easily and the temperature of the solution obtained will be lower than the real one. 2. When the experiment was done, the temperature was quite cold as the weather was cloudy. This can also affect the temperature of the solution as heat will be released to the surrounding even faster due to the chill environment. 3. There was also a possibility for parallax error to happen as we human cannot avoid ourselves from making mistakes. 4. Each neutralization was done only once. . For each neutralization, the same styrofoam cup was used. This can cause contamination whereby some solution might be neutralized right after it is poured into the empty cup. Ways to Come Shortcomings: 1. The styrofoam cup should be closed so that heat will not be easily released to the surrounding. 2. If the temperature of th e room where the experiment is to be done is cold, shut off all fans to minimized the loss of heat of the solution to the surrounding. 3. Calculate the uncertainties for each measurement and bring it along till the end of the calculation. 4. To obtained more accurate results, each neutralization should be done more than once so that the average value can be obtained. 5. Using different styrofoam cup for each neutralization can minimize contamination. Conclusion: From the experiment, we can determine the heat of neutralization by calculating the amount of heat released when the reaction occur. The heat of neutralization for one mole of reaction can be done by dividing the heat released to the number of mole of the solution used in the reaction. [pic] [pic] [pic] [pic] [pic] [pic]