Using nanotechnology for new drug discovery Article

Using nanotechnology for new drug discovery - Article Example Drug discovery is a growing paradigm that is increasingly in need of better technologies to improve the effectiveness, efficiency and cost effectiveness of the various processes involved in the drug discovery processes. For example, it is currently estimated that the full process of new drug discovery typically takes a period of not less than 10years and costs approximately $800 million. Many researchers however agree that a number of nanotechnology applications have a potential to address some of the challenges commonly met during the drug development process. One of the potential uses of nanotechnology in new drug discovery is the analysis of signaling pathways using various nanobiotechnology techniques such as proteomics which enable researchers to gain new insights regarding the disease processes. In this regard, nanotechnologies not only help drug scientists to identify more efficient biomarkers, but such techniques can also enhance their understanding of the drug action mechanisms during their drug discovery processes. Refining the application of proteomics using nanotechnologies is particularly play a critical role in the identification of drug targets as well validation phases during the drug discovery process. For instance, nanodevices such as nanotube electronic biosensors are increasingly being used in proteomics to enhance the investigation of protein –protein and surface protein binding as well as in the development of highly accurate electronic biomolecule detectors (Lynn, 128). Consequently such devices provide effective alternatives of detecting important biomolecules such as antibodies during the drug discovery process. Another important use of nanotechnology for new drug discovery involves the application of nanoparticles such as quantum dots (QDs) in tracking single drug molecules. Although the tracking of single drug molecules has been previously been done using the old

Rules to Teamwork :: essays research papers

The Challenges of Teamwork Working on teams can normally prove very challenging, with all of the variations in personalities, strengths, and weaknesses, most of these issues are raised face to face with individuals, and can be resolved by finding a room to sit and talk them out. Working on virtual teams is more challenging, since there are a lot of things missing from the person-to- person contact, such as: †¢Lack of visual cues to understanding context. Many people write email and talk on the telephone in a manner which is completely different than they would talk in person; things that are taken as insults could actually be jokes, or things that are taken as jokes could actually be insults. †¢Lack of a communication mesh. Generally, teams work well when ‘cubicle to cubicle talk’ occurs; when people wander around asking questions. It’s difficult to wander from place to place all the time when your team is scattered all over the world. At the same time, virtual teams have some advantages. For instance, it’s easier to think through your response when writing an email than when talking in a meeting, which is a good and a bad thing. It’s harder to brainstorm when you aren’t willing to just throw out ideas (people are often afraid of saying things that make them look stupid in email, because they think about it before they send it). But it’s easier to have rational discussion when everyone can (not that they always do) let things sit for some time rather than replying in emotion. Several things that came up in our discussion are that virtual teams are also like normal teams in many ways, so many of the normal team rules apply. Web Research Several links came up dealing with virtual teams when searching the Internet.

Determination of a Rate Law Lab Report

Determination of a Rate Law Megan Gilleland 10. 11. 2012 Dr. Charles J. Horn Abstract: This two part experiment is designed to determine the rate law of the following reaction, 2I-(aq) + H2O2(aq) + 2H+I2(aq) + 2H2O(L), and to then determine if a change in temperature has an effect on that rate of this reaction. It was found that the reaction rate=k[I-]^1[H2O2+]^1, and the experimental activation energy is 60. 62 KJ/mol. Introduction The rate of a chemical reaction often depends on reactant concentrations, temperature, and if there’s presence of a catalyst.The rate of reaction for this experiment can be determined by analyzing the amount of iodine (I2) formed. Two chemical reactions are useful to determining the amount of iodine is produced. 1) I2(aq) + 2S2O32-(aq) 2I-(aq)+S4O62-(aq) 2) I2(aq) + starch Reaction 2 is used only to determine when the production of iodine is occurring by turning a clear colorless solution to a blue color. Without this reaction it would be very diff icult to determine how much iodine is being produced, due to how quickly thiosulfate and iodine react. Related article: Measuring Reaction Rate Using Volume of Gas Produced Lab AnswersHowever this reaction does not determine the amount of iodine produced, it only determines when/if iodine is present in solution. Reaction 1 is used to determine how much iodine is produced. To understand how the rate constant (k) is temperature dependent, another set of data is recorded in week two’s experiment using six trials and three different temperatures(two trials per temperature change). Using the graph of this data we determine the energy required to bend of stretch the reactant molecules to the point where bonds can break or form, and then assemble products (Activation Energy, Ea).Methods To perform the experiment for week 1, we first prepare two solutions, A and B, as shown in the data. After preparing the mixtures, we mix them together in a flask and carefully observe the solution, while timing, to see how long it takes for the solution to change from clear to blue. We use this method for all 5 trials, and record the time it takes to change color, indicating the reaction has taken place fully. This data is used to find p (trials1-3) and q (trials3-5), to use in our rate law. This experiment concluded that both p and q are first order.The rate constant average of all five trials is used as just one point on the Arrhenius Plot. In week 2, we perform the experiment to test the relation of temperature to the rate of reaction. We start by again, preparing six solutions. We prepared two trials/solutions at 0 degrees Celsius, two and 40 degrees Celsius, and two at 30 degrees Celsius. Again, for each trial we mixed solution A with B, and carefully timed the reaction to look for a color change that indicates the reaction is complete. The interpretation of this data indicated out results of whether temperature has an effect on the rate of this reaction.Results- It is determined that the rate of reaction is dependent on the temperature in which the reaction occurs. The sol utions observed at 40 degrees Celsius reacted at a quicker rate, than those at lesser temperatures, in a linear manor. Data Week 1 Table 1: Solution Concentrations Week 1- Room Temperature trial #| solution A| | | | | Solution B| | | | | | buffer| 0. 3MKI| starch| 0. 02MNa2S2O3| Distilled water| 0. 1MH2O2| time(s)| total volume(mL)| | 1| 5. 01| 2. 0| 0. 4| 5. 0| 21. 68| 6. 0| 585| 40. 01| | | 2| 5. 0| 4. 0| 0. 4| 5. 0| 19. 60| 6. 0| 287| 40. 00| | | 3| 5. 2| 6. 0| 0. 4| 5. 0| 17. 60| 6. 0| 131| 40. 02| | | 4| 5. 0| 6. 0| 0. 4| 5. 0| 13. 62| 10. 0| 114| 40. 02| | | 5| 5. 0| 6. 02| 0. 4| 5. 0| 9. 60| 14. 0| 80| 40. 02| | | Calculations Week 1 1. Find the moles of S2O3-2 Take the value from NaS2O3 *(0. 2)/1000 (5)*(0. 2)/1000= 0. 001 mol of S2O32- 2. Find moles of I2 Take S2O32- /2 (0. 001)/2=0. 0005mol 3. Find I2 Mol I2*1000/vol mL (0. 0005)*1000/40)= 0. 000799885 mol 4. Find the rate of change Take (I2)/ (seconds) (0. 000799885)/(585)= 1. 36732Ãâ€"10-6 M/s 5. Find [I-]0 (0. 300 M KI )*(2. 00mL)/( the final volume)=0. 015 M 6.Find the Ln of [I-]0 Ln(0. 015)=-4. 19970508 7. Find [H2O2]0 Take (0. 10 M H2O2)*(6. 00mL)/ ( final volume)=0. 015 M 8. Ln of [H2O2]0 Ln(0. 015)= -4. 19970508 9. Find the Ln of rate: Ln(2. 13675Ãâ€"10-5)=-10. 753638 10. The last step for week one calculations is to calculate the average value of k. Rate= k [I-]1[H2O2]. (2. 13675*10-5 ) = k [0. 015] [0. 015] then solve for k. For this trial, k=0. 09497. This is then done for all trials. Then, once all five values of k are found, the average is taken by adding all five values of k and dividing by 5. The experimental k average is 0. 05894M/s. Table 2: Calculations Week 1 | | | | | | | | | | | | solution#| mol s2O3-2| mol I2| I2| (rate) changeI2/change in temp| [I-]o| ln[I-]o| [H2O2]0| ln[H2O2]o| ln rate| k | | 1| 0. 001| 0. 0005| 0. 0125| 2. 13675E-05| 0. 015| -4. 19970| 0. 015| -4. 19971| -10. 753| 0. 0949| | 2| 0. 001| 0. 0005| 0. 0125| 4. 3554E-05| 0. 030| -3. 50655| 0. 015| -4. 19971| -10 . 041| 0. 0967| | 3| 0. 001| 0. 0005| 0. 0125| 9. 54198E-05| 0. 045| -3. 10109| 0. 015| -4. 19971| -9. 2572| 0. 1413| | 4| 0. 001| 0. 0005| 0. 0125| 0. 000109649| 0. 045| -3. 10109| 0. 025| -3. 68888| -9. 1182| 0. 974| | 5| 0. 001| 0. 0005| 0. 0125| 0. 00015625| 0. 045| -3. 09776| 0. 035| -3. 35241| -8. 7640| 0. 0988| | | | | | | | | | | k avg| 0. 1059| | | | | | | | | | | | | | Data Week 2 Table 3: Solution Concentrations Week 2- Varied Temperatures trial #| solution A| | | | | Solution B| | | Temp(C)| | | buffer| 0. 3MKI| starch| 0. 02MNa2S2O3| Distilled water| 0. 1MH2O2| time(s)| total volume (mL)| | 1| 5. 00| 6. 01| 0. 42| 5. 00| 13. 60| 10. 00| 692| 40. 03| 1. 0| | 2| 5. 00| 6. 00| 0. 40| 5. 00| 9. 60| 14. 00| 522| 40. 00| 1. 0| | 3| 5. 00| 2. 00| 0. 40| 5. 02| 21. 0| 6. 00| 152| 40. 02| 40. 0| | 4| 5. 00| 4. 00| 0. 40| 5. 02| 19. 60| 6. 00| 97| 40. 02| 40. 0| | 5| 5. 00| 6. 00| 0. 40| 5. 02| 17. 60| 6. 00| 110| 40. 02| 30. 0| | 6| 5. 00| 4. 00| 0. 40| 5. 00| 19. 60| 6. 00| 137 | 40. 00| 30. 0| | Calculations Week 2 1) Find amount of I2 moles produced in the main reaction using Volume of Na2SO4 used, stock concentration of Na2SO4 solution, and the Stoichiometry (2mol Na2SO4 to 1 mol I2) for all six trials. Trial 1: (. 005 L Na2SO4)(. 02 moles Na2SO4/1. 0L)(1 mol I2/2 mol Na2SO4)= . 00005 mol I2 Use this method for all six trials ) Find the reaction rate using moles of I2 produced, measured time in seconds, and Volume of total solution for all six trials Trial 1: (. 00005 mol I2/. 0403L)=(. 00124906 mol/L) /(692seconds)= . 00000181mol/L(s) Use this method for all six trials 3) Find the rate constant using the reaction rate, measured volumes used, stock concentrations, and the rate law of the main reaction. Trial 1: K=(. 00000181MOL/L(s))/((. 01 L H2O2)(. 1 M H2O2)/. 0403L total))((. 3MKI)(. 006LKI)/. 0403L total)=. 00107 Use this method for all six trials 4) To graph, we must calculate Ln(k) and 1/Temp(K) for each individual trial.Trial 1: Ln(. 00107)=-6. 8 401 and 1/T = 1/692sec=-. 00365k^-1 Use calculation method 1-4 for all six trials Table 4: Calculations Week 2 solution#| mol I2| Rate (change I/change in time)| K (min-1)| Ln k| Temp (K)| 1/T (k-1)| 1| . 00005| . 00000181| . 00107| -6. 8401| 274| . 00365| 2| . 0000502| . 00000240| . 00152| -6. 48904| 274| . 00365| 3| . 0000502| . 00000825| . 0370| -3. 29684| 313| . 00319| 4| . 0000502| . 0000129| . 0290| -3. 54046| 313| . 00319| 5| . 0000502| . 0000114| . 0171| -4. 06868| 303| . 00330| 6 | . 00005| . 00000912| . 0203| -3. 89713| 303| . 0330| From the graph, we see that the slope is -7291. To Find the Activation Energy we multiply by the rate constant of 8. 314J/mol(K), which equals -60617. 4 J/mol. We then convert this value to kilojoules by dividing by 1000, equaling 60. 62 kJ/mol. Analysis uncertainty- Due to the limit of significant figures in stock solutions used, the resulting data is limited in correctness. Also, temperature fluctuations during the experiment by even a half d egree would obscure the data of the exact rate constant, k. One of our R^2 coefficients for the experiment was in fact greater than 0. , and the other slightly less than 0. 9 meaning the one lesser is not considered a good fit. The deviation in goodness of fit may have been due to our data recording. Discussion- Determination of the rate law and activation energy of a chemical reaction requires a few steps. By varying the concentrations of reactants it was determined that the reaction is first order with respect to both [I-] and [H2O2+]. Measuring the reaction rate at multiple temperatures allows calculation of the activation energy of the process, in this case the activation energy of the reaction is found to be 60. 2 kJ/mol. As you have seen through all the previous data, charts and graphs, this exothermic rate of a reaction is dependent on solution concentrations, a catalyst, and temperature. References 1 Determination of a Rate Law lab document, pages 1-6, Mesa Community College CHM152LL website, www. physci. mc. maricopa. edu/Chemistry/CHM152, accessed 10/9/2012. 2 Temperature Dependence of a Rate Constant lab document, pages 1-3, Mesa Community College CHM152LL website, www. physci. mc. maricopa. edu/Chemistry/CHM152, accessed 10/9/2012.

New Hampshire Colleges and Universities Pursuing Online and Campus Based Education in New Hampshire 2019

New Hampshire has become a haven for its residents and local businesses. Working professionals looking to attend one of its many New Hampshire colleges and universities reap the financial benefits of no state sales or income tax. New Hampshires job market is also ripe with opportunity, thanks to technology firms and other businesses seeking shelter from high tax rates in Boston and surrounding areas. Leading New Hampshire Industries Employ Graduates of New Hampshire Colleges and Universities A diverse selection of businesses and employers are housed in the state of New Hampshire. College graduates can expect to find employment in one of New Hampshires top 6 industries, including: New Hampshire Trade, Transportation, and Utilities. New Hampshire Educational and Health Services. New Hampshire Government. New Hampshire Manufacturing. New Hampshire Leisure and Hospitality. New Hampshire Professional and Business Services. New Hampshire College Graduates Enter an Economy with Top Earnings and Record-Low Unemployment Rates A year-round tourist industry contributes to the economic health of New Hampshire. College students also enjoy local skiing, hiking, rafting, and climbing. In addition to outdoor recreation, New Hampshire university students benefit from the most recent statistics from the U.S. Census Bureau and U.S. Department of Labor: The 2016 2017 New Hampshire median household income was $57,850, over $10,000 above the national average. The 2017 New Hampshire gross state product was $49 billion. The September, 2017 New Hampshire unemployment rate was 3.6%, compared to the national average of 4.8%. 717,300 people are employed in New Hampshire. .ud3b5801225e3acd99601ac1e2f1bcf87 { padding:0px; margin: 0; padding-top:1em!important; padding-bottom:1em!important; width:100%; display: block; font-weight:bold; background-color:#eaeaea; border:0!important; border-left:4px solid #34495E!important; box-shadow: 0 1px 2px rgba(0, 0, 0, 0.17); -moz-box-shadow: 0 1px 2px rgba(0, 0, 0, 0.17); -o-box-shadow: 0 1px 2px rgba(0, 0, 0, 0.17); -webkit-box-shadow: 0 1px 2px rgba(0, 0, 0, 0.17); text-decoration:none; } .ud3b5801225e3acd99601ac1e2f1bcf87:active, .ud3b5801225e3acd99601ac1e2f1bcf87:hover { opacity: 1; transition: opacity 250ms; webkit-transition: opacity 250ms; text-decoration:none; } .ud3b5801225e3acd99601ac1e2f1bcf87 { transition: background-color 250ms; webkit-transition: background-color 250ms; opacity: 1; transition: opacity 250ms; webkit-transition: opacity 250ms; } .ud3b5801225e3acd99601ac1e2f1bcf87 .ctaText { font-weight:bold; color:inherit; text-decoration:none; font-size: 16px; } .ud3b5801225e3acd99601ac1e2f1bcf87 .post Title { color:#000000; text-decoration: underline!important; font-size: 16px; } .ud3b5801225e3acd99601ac1e2f1bcf87:hover .postTitle { text-decoration: underline!important; } READ Top Internship Mistakes to AvoidNew Hampshire Universities and Colleges Allow Working Professionals to Combine Campus-based and Online Education New Hampshire colleges and universities are making it easier than ever for working professionals to return to school. Career advancement programs that utilize a combination of online and campus-based education are available through New Hampshire schools, such as: Kaplan University at Hesser College: Concord College Campus, Manchester University Campus, Nashua College Campus, Portsmouth University Campus, Salem College Campus, and Online Programs. University of Phoenix: New Hampshire Online Programs. ITT Technical Institute: New Hampshire Online Programs. For an extensive list of New Hampshire colleges and universities, students are encouraged to visit College-Pages.com, the leading education and career resource website. Prospective students will also find access to informative articles on making education and career decisions in the state of New Hampshire. Related ArticlesPursuing Advanced Education in the Heartland of Dixie Alabama Colleges and UniversitiesSouth Carolina Colleges and Universities Pursuing Online and Campus Based Education in South Carolina, the Palmetto StateVirginia Colleges and Universities Pursuing Online and Campus Based Education in Virginia, the Old Dominion StateArizona Colleges and Universities Pursing Advanced Education in The Grand Canyon StateStudents of Business AdministrationColleges and Universities in Alberta, Canada Pursuing Online and Campus-based Education in Alberta, Canada .u6741303d358b43a88d1006ce13890ff6 { padding:0px; margin: 0; padding-top:1em!important; padding-bottom:1em!important; width:100%; display: block; font-weight:bold; background-color:#eaeaea; border:0!important; border-left:4px solid #34495E!important; box-shadow: 0 1px 2px rgba(0, 0, 0, 0.17); -moz-box-shadow: 0 1px 2px rgba(0, 0, 0, 0.17); -o-box-shadow: 0 1px 2px rgba(0, 0, 0, 0.17); -webkit-box-shadow: 0 1px 2px rgba(0, 0, 0, 0.17); text-decoration:none; } .u6741303d358b43a88d1006ce13890ff6:active, .u6741303d358b43a88d1006ce13890ff6:hover { opacity: 1; transition: opacity 250ms; webkit-transition: opacity 250ms; text-decoration:none; } .u6741303d358b43a88d1006ce13890ff6 { transition: background-color 250ms; webkit-transition: background-color 250ms; opacity: 1; transition: opacity 250ms; webkit-transition: opacity 250ms; } .u6741303d358b43a88d1006ce13890ff6 .ctaText { font-weight:bold; color:inherit; text-decoration:none; font-size: 16px; } .u6741303d358b43a88d1006ce13890ff6 .postTitle { color:#000000; text-decoration: underline!important; font-size: 16px; } .u6741303d358b43a88d1006ce13890ff6:hover .postTitle { text-decoration: underline!important; } READ Your People Skills and a Career in Human Resources Management