Resisitivity Through Copper Wire

Answer: Increasing the resistivity the resistor gets bigger, which directly effects the current by making it smaller. Indirectly the voltage to push the current through has to be stronger to push the current through. The value of R gets larger, you can change the resistance, but you would have to change out the resistor element to do this.

XIV. Record your observations of the dried, cooled copper metal and weigh the recovered copper.

16) Place the container in the drying oven. It must be dried overnight. DAY THREE: 17) Weigh the dried silver product and beaker 18) Record this into the quantitative data table V. Data Results: Raw Data: Table 1. Qualitative Data: Day 1 to 3 Observations DAY 1 | DAY 2 | DAY 3 | | | | Copper wire turned white when submerged in distilled water, little crystal-like substances forming on copper

• Weight is a vital factor to take into consideration for the product. • When tested in the lab, it was found that Advance Wire was mediocre in conductivity & abrasiveness, while also being heavier than all other samples.

Should We Mine This Ore? Names CHM113 TA Name Class Time Introduction One of the most important skills to have in the chemistry lab is the understanding of how chemicals will react. Knowing for example, how a chemical will react with a metal, is an excellent way of determining the amount of a particular metal in a deposit. This knowledge was used in this lab to determine the amount of copper in an unknown sample mixture. It is also known that the determination of the percent concentration of a certain solution, will directly effect the percent transmission and absorption of a solution, dependent upon its dilution. By first testing known concentrations of a solution, and plotting this information graphically, a line is formed

According to the data I collected, accuracy and precision do remain for the most part constant for the different volumes. I was the most accurate during one of my measurements of 200 µL, but I was the most precise with my measurements of 25 µL and 50 µL.

The Cu Later lab experiment is designed to allow you to practice lab skills in implementing and performing a series of reactions. Specifically, four types of chemical reactions will occur: oxidation/reduction; double replacement; single replacement; and decomposition. You will begin with a known amount of copper metal, which, after progressing through several steps, is reproduced. In this experiment you will observe and record the various changes such as heat, color changes, and production that occur. This procedure is used to observe some chemical reactions of copper and its compounds while also performing the lab appropriately as to retain the copper as much as

The objective of analytical procedures is to identify the existence of unusual transactions and events, and amounts, ratios and trends that might indicate matters that have financial statement and audit planning ramifications*. First, the auditors should consider information regarding the industry in which the client operates**. In this case, average machine setup time from start to finish is approximately six hours, which is slightly below the industry average. It means the company is efficient in preparation for production. Also, the auditors should compare client data with prior period data***. For example, days sales in receivables increased from 48.4 days (2004) to 56.3 days (2005). Though sales didn't increase a lot ,but days sales

Procedure: Begin this In the hood, place the copper wire in 10mL of nitric acid and wait for it to dissolve. Afterwards, add 100mL of deionized water to the solution and boil the solution, so all the nitrogen oxides are removed. Place the solution to a 250.0mL volumetric flask and add deionized water to the flask until the solution is 250.0mL. When the solution in the flask is at 250.0mL place the solution in a clean plastic bottle. Now cut a penny into four pieces, and measure the mass of all the pieces together. Go back to the hood, and place the pieces of the penny into a 250mL beaker. Afterwards, add 20mL of concentrated hydrochloric acid. Wait for the hydrochloric acid to dissolve the zinc core. When the zinc has dissolved, filter the solution through the filter paper, and place the copper metal pieces into a clean 150mL beaker. In the hood, place 4mL of concentrated nitric acid in the beaker, and when the copper dissolves add, one drop at a time, 30mL of 6 M ammonium hydroxide to neutralize the nitric acid. Transfer the copper/ammonia solution to a 100.00mL volumetric flask. Prepare four different calibration

Ruth Habte Lab Partners: John Gould & Ashton Hall TA: Jess Bases Professor Yasmin Jessa Chemistry 144 Section C 11 November 2015 Calculating the Actual Copper Amount in a Penny Introduction: In 1909, on the 100th anniversary of Abraham Lincoln’s birth, the one cent coin (penny) was introduced. Between 1864 and 1982, the penny was made of

Used stirring rods to completely remove copper from that wire. And then completed the removal of copper using 5 drops of 6M HCl, adding it onto copper. There will produced copper in a solution. Connected Buchner flask to the vacuum line and place filter paper in it to completely washed off the copper. Then, add 95% ethanol to copper and leave it for 1 min and turned section back for 5 mins. Measured mass of clean, dry watch glass. Transfer copper to watch glass and dry it under heat lamp for 20 mins, allowed it to cool to room temperature and then accurately determine its mass.

Thermodynamics Laboratory Report Greenwich University By Mussie Gebre 26/01/2011 Content Page Objectives-------------------------------------page3 Introduction----------------------------------page3 Operation (process) ------------------------page3 Result and discussion-----------------------page4 Experimental data and plot-------------page4&5 Conclusion -------------------------------------page6 Mussie Gebre ID 000517715 Thermodynamics laboratory report Objective * Experiment on four different metals on their heat conductivity * To understand thermodynamics * To illustrate the physical concept of thermodynamics and heat However it shows some difference on the actual value of the measurement l = lo (1 + T) Copper: l= 88(1+16.6x10-6x30.3) = 88.044mm lo=88mm | y=16.6x10-6 | ∆T=30.3◦C | l=? | Aluminium lo=79mm | y=25 x 10-6/ºC | ∆T=36 ºC | l=? | l = lo (1 + ∆ T) l=79(1+25 x 10-6/ºC x 36 ºC =79.07mm Brass lo=88mm | y=18.7 x 10-6/ºC | ∆T=47.9 ºC | l=? | l = lo (1 + ∆ T) l=88(1+18.7 x 10-6/ºC x47.9 ºC) =88.07mm Iron lo=88mm | y= 12x 10-6/ºC | ∆T=? | l=88.1 | ∆T=lloy)-1 = 88.1∕88x12x 10-6/ºC -1 Conclusion Overall, the experiment succeeded that the metals show the theoretical properties. Differences existed in the mathematical calculation of the actual length. These differences, however, it can be accounted for by experimental error; more over there are uncertainty on purity of the

Purpose: The purpose of this experiment was to observe the many physical and chemical properties of copper as it undergoes a series of chemical reactions. Throughout this process, one would also need to acknowledge that even though the law of conservation of matter/mass suggests that one should expect to recover the same amount of copper as one started with, inevitable sources of error alter the results and produce different outcomes. The possible sources of error that led to a gain or loss in copper are demonstrated in the calculation of percent yield (percent yield= (actual yield/theoretical yield) x 100.

Copper For our science assessment we had the task to research about a metal of our choice. Since I am really into computers, I chose copper. A metal used in all kinds of wires, cpu’s and other stuff without a computer wouldn’t work. This fits really well into what we have

Bc ≈ Bc(0) * [1 - (T/Tc)^2] In the early 1900's a duch physicist by the name of Heike Kammerlingh Onnes (pictured above), discovered superconductivity. Before his discovery, Onnes had spent most of his scientific career studying extreme cold. The first step he took toward superconductivity was on July 10, 1908 when he liquified helium and cooled it to an astonishing 4 K, which is roughly the temperature of the background radiation in open space. Using this liquid helium, Onnes began experimenting with other materials and their properties when subjected to intense cold. In 1911, he began his research on the electrical properties of these same materials. It was known to Onnes that as materials, particularly metals, cooled, they exhibited less and less resistance. Bringing a mercury wire to as close to absolute zero as possible, Onnes observed that as the temperature dropped, so to did the resistance, until 4.2 K was reached. There resistance vanished and current flowed through the wire unhindered. Below is an approximate graph displaying resistance as a function of temperature for the experiment Onnes conducted with mercury: