How does the rate of reaction in Task 2 compare with the rate in Task 1? Suggest a reason for the change. By comparing the two curves and the times taken to reach 0.0 g (the last times on the list), predict the time it would take for the reaction to finish if 100 chips were used. Task 3 Press back but not clear and change the number of chips to 100 but leave the acid concentration at 1.0 mol/dm3 . Click start and take readings as often as possible (by clicking the take readings button) until the mass reaches 0.0 g. Stop the reaction immediately.
Then you place another 200 gram mass on the 210 degree mark. Then we have to replace the mass at the 30 degree mark with two masses, one at the 0 degree mark and one at the 80 degree mark. Essentially we are trying to calculate the x and y component vectors of a 200g mass at 30 degrees. So what we did was we just guess and checked the variables of weight at the 0 degree mark and at the 90 degree mark’s pullys until the ring was centered. You can us+e the weight on each pully to calculate the magnitude and the direction of the component vectors at 90 and 0 degrees.
Adam Workman Lab, Week #1 Balance Lab Introduction The purpose of the Balance Lab experiment was to become familiar with the ChemLab software and to become familiar with different mass measurement methods. During the experiment, three different mass measurement methods were used to determine the mass of copper slugs as well as the mass of two different unknown weights: the direct weight method, the weighing by difference method, and the average mass method using both a centigram balance and an electronic balance. Using the centigram balance, the weight of a single copper slug, in grams, is determined using both the direct weight and weight by difference methods. Likewise, using the electronic balance, the same copper slug is measured by direct weight and weighing by difference methods. Using the same electronic balance, the average mass of five copper slugs, in grams, will be determined.
Then multiply this by the molar mass of NaClO which has a label of g/mol so all labels cancel. Finally multiply by 100 to get a percent!) 6. The label on the commercial bleach reports the percent by mass NaClO to be 6.0%. Calculate the percent error of your value, assuming that the
The purpose of the experiment was to do a solution, which molarity is 0.20 mol/l, from water and an ionic compound. Our ionic compound was zinc sulfate (ZnSO4). Our task was to make one hundred milliliters (100 ml) of the solution. Materials To execute the experiment we used the following equipment: - a beaker - a volumetric flask - a plastic spoon - a scale - a pipette - a funnel - a cork cap We also used solid zinc sulfate (ZnSO4), and distilled and deionized water to make the solution. Calculations To figure out the amount of zinc sulfate that we had to add to the water, so that the molarity of the solution would be 0.20 g/mol, we did the following steps: First we calculated the amount of the zinc sulfate to add in moles.
Year 11 Chemistry Electrochemical Cells Purpose To determine the order of reactivity for the metals copper, iron, lead and zinc using the least amount of electrochemical cells as possible. Materials List • Four 100ml beakers • 4 strips of filter paper approximately 15cm in length • Voltmeter • Sodium Chloride solution at 10% concentration • Zinc, Copper, Lead and Iron metal strips (approximately 10 cm) • 50 ml of Copper sulphate, Zinc sulphate, Lead nitrate and Iron nitrate solutions • Scissors Procedure - Place the 50ml solution of zinc sulphate in a 100ml beaker, and 50ml solution of copper sulphate in a different 100ml beaker. Place the zinc metal strip in the zinc sulphate beaker and the copper metal strip with the copper sulphate beaker.
Determining the Percent of Copper and Zinc in Pennies Objective: * Find a way to measure the percent of density of the zinc and copper in pennies * Use best-fit straight line to examine linear relationships, and use it to create a predictive model to determine the percents * Learn to record lab data and observations, and practice with safe procedures in the lab. Background: As we know of today pennies are not made with just copper, they are made with many different metals and have a copper coating. To find the percent of copper you need to find the densities of the materials that make up a penny and then find the mass of just the copper and you can find a percent. Experiment Procedure: Determine the density of the following percentages of Zinc and Copper mixtures. Then compare the precision and accuracy of the data to the literature values for pre and post 1892 pennies when using various numbers of coins.
How many moles of zinc are in a penny? Purpose: This lab is being performed so students can visualize a single-replacement reaction and calculate how much zinc is in a post-1982 penny. Materials: A post- 1982 penny steel wool 3 M HCl graduated cylinder small beaker tongs balance paper towels sharp edge Safety: 3 M hydrochloric acid (HCl) is fairly caustic. Wash hands immediately if you spill on them. Wear goggles.
Single Replacement Reaction Laboratory Modified from Glencoe Chemistry - Matter and Change, Glencoe McGraw-Hill, 2002 Objectives Observe a single replacement reaction Measure the masses of iron and copper Determine the mole ratios and the limiting reactant Chemicals Iron filings (Fe) – 20 mesh Copper(II) sulfate pentahydrate, (CuSO4·5H2O) Distilled water Materials Stir rod 100-mL beaker 250-mL beaker 25-mL graduated cylinder Weigh paper Balance Hot plate Beaker tongs Wire mesh insulated pad screen Distilled water wash bottles |Lab Data - Reaction of Copper(II) Sulfate and Iron | | Mass of empty 100-mL beaker |(g) | | | Mass of 100-mL beaker
We rotated the ray table clockwise by increments of 10̊ again. We repeated the same measurements but instead with counterclockwise angles. From the two angles of refraction we were able to calculate the average angles of refraction. Finally, we aligned the flat side of the lens so that incoming light ray struck the cylindrical surface. We rotated the ray table until the refracted ray disappeared completely and only the reflected ray was visible.