What has a density of 2.65?

Please help me find the density of Copper, Aluminum, Lead, and Nickel ?

• Experiment 1 - The Density of Solids Cylinder 1 Volume 31.12mL Mass 40g 30mL of water 10g copper Cylinder 2 Volume 33.57mL Mass 40g 30mL of water 10g Aluminum Cylinder 3 Volume 30.88mL Mass 40g 30mL of water 10g lead Cylinder 4 Volume 31.12mL Mass 40g 30mL of water 10g nickel 1. Record your data for each of the four metals from the density measurements in your answers, where a sample layout is provided. Copper: (a) mass (g): (b) volume water add (mL): (c) total volume of water and metal (mL): ----------------------------------------… (d) density of the metal (g/mL): (e) error bounds: 2. Calculate the density by dividing the mass of each metal by its volume, where the volume of the metal is the total volume in the flask minus the volume of water. A Hypothesis Based on this experiment, we may think that density measurements are sufficient to allow us to identify any metal, and so a hypothesis may be stated as follows: "It is possible to identify any unknown metal by measuring the mass and volume of a sample, calculating its density, and then comparing it with a list of known metal densities." First, let’s look at the results for the four metals that you tested. Without getting into the statistical analysis of the data, we can still estimate the errors involved in the measurements that you made. The mass was measured by a balance that reads to .01g (10 mg) and the accuracy as stated by the manufacturer is +/- 0.2g. Each metal sample was 10 g, so the error is +/- (0.2/10) = 0.02 or 2%. The flask reads to 0.1 mL and it is said to be accurate to 0.2 mL. The volume varied from metal to metal, but we can use an average value of 30mL. The error is +/- (.2/30) = .0067 or 0.67%. In calculating density, the measured mass is divided by the measured volume. By the rules for handling measurement errors, the fractional errors are added together. This gives us: Density error = +/- (2% + .67%) = +/- 2.7% The density calculations, then, should be reported as the calculated value plus or minus the error of 2.7%. 3. Calculate the error bounds for the four density values by adding and subtracting 2.7% from the actual density values. For example, for a density of 10g/mL and an error of 2%, you would write: error bounds = 9.8 - 10.2 Add the error bounds to the data for the four metals. 4. Which metals can clearly be identified, one from the others, according to its density? 5. Which metals cannot be clearly identified one from the others? 6. Open the lab manual to the procedures of Experiment 1 and look at the graph of the densities of many common metals. Use the graph to answer the following questions: It is clear from the graph that the density of a great many metals falls within the range of 8-9 g/mL. Consider carefully now the original hypothesis that density can be used to identify a metal sample. (a) Is the hypothesis true for all metals? (b) For which metals is the hypothesis true? (Don’t give names, but rather a statement such as “the set of metals whose density is…”) (c) For which metals is the hypothesis NOT true? (Again, use a statement of the form ““the set of metals whose density is…”) (d) What is your conclusion regarding the validity of the hypothesis? How would you restate it?

• Answer:

  D=m/v so divide mass of substance by the change in water 1mL = 1 cc (cubic centimeter) the directions say exactly how to do it