Lab Title: Mole-to-Mole relationships and Empirical Formulas
Purpose: The objective of lab four was to use the website Late Nite Labs to determine mole-to-mole relationships and empirical formulas in chemical reactions. Combining and/or heating various compounds, observing the reactions and then calculating the moles revealed the balanced chemical reactions.
Materials: For the virtual experiment, a computer, Internet, calculator and access to Late Nite Labs were needed.
If one were to do the mole-to-mole relationship lab with actual materials they would need copper (s), a Bunsen burner, a crucible, a scale, 0.2 M silver nitrate (AgNO3)(l), and beakers.
If one were to do the empirical formula lab with materials that are physically present
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93g – 88 g = 5 g
Grams to moles = Grams used divided by moles per gram e.g. 1.000 g Cu / 63.546 g of copper in 1 mole = .01574 mol
Results: The purpose of experiment 5a was to determine the molar ratio between copper and silver. It was found that 2 moles of silver nitrate combine with one mole of copper to yield two moles of silver and 1 mole of copper (II)
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Experiment 2
1. Write the equation for the decomposition of the hydrate, MgCl2 MgCl2*XH2O (s) −> MgCl2 (s) + XH2O (g) 2. Record the following masses:
a. mass of the crucible and hydrate (g)
b. mass of the crucible and pure salt (g)
The information requested is found in the following table:
Mass of the crucible and hydrate (g) 93.000 g
Mass of the crucible and pure salt (g) 90.342 g
3. Calculate the following:
a. mass of water in the hydrate sample (g)
b. number of moles of water in the sample c. mass of pure salt in the sample (g)
d. number of moles of salt in the sample
e. molar ratio of water to salt in the sample
The results of the calculations requested are found in the following table:
Mass of water in the hydrate sample (g) 2.658 g
Number of moles of water in the sample .1475 mol
Mass of pure salt in the sample (g) 2.342 g
Number of moles of salt in the sample 0.02460 mol
Molar ratio of water to salt in the sample 6 moles of water to 1 mole of salt
4. From your calculations, what is the empirical formula of magnesium chloride hydrate? MgCl2*6H2O (s) −> MgCl2(s) + 6H2O(g)
2. Cooper, M. M., Cooperative Chemistry Laboratory Manual, McGraw-Hill: New York, NY, 2009, p. 60.
Number of moles of〖 K_2 CrO〗_4, mol = (4.0 ×〖10〗^(-2) mol L^(-1))(5.0×〖10〗^(-2) L)= 2.0×〖10〗^(-3) mol
The procedure of the lab on day one was to get a ring stand and clamp, then put the substance in the test tube. Then put the test tube in the clamp and then get a Bunsen burner. After that put the Bunsen burner underneath the test tube to heat it. The procedure of the lab for day two was almost exactly the same, except the substances that were used were different. The
The objective of this experiment will be to combine various substances, liquids and metals, and to observe their behavior when they are combined. The types of reactions observed shall determine the nature of these reactions: physical or chemical.
Mass of O = Mass of crucible, cover, KClO3 and MnO2 after heating (Step # 11) - Mass of crucible, cover, KClO3 and MnO2 before heating (Step # 5)
The results of this experiment are shown in the compiled student data in Table 1 below.
Experimental: The experimental procedure outlined in the OU Physical Chemistry Laboratory Manual was followed without any deviations.
The purpose of this lab was to to cycle solid copper through a series of chemical forms and return it to its original form. A specific quantity of copper undergo many types of reactions and went through its whole cycle, then returned to its solid copper to be weighted. We observed 5 chemical reactions involving copper which are: Redox reaction (which includes all chemical reactions in which atoms have their oxidation state changed), double displacement reaction, precipitation reaction, decomposition reaction, and single displacement reaction.
Equipment = == == == == § Hydrochloric Acid § Gelatine § Tile § Test tube § Rubber Bung § Scalpel § Ruler § Stop Clock § Goggles § Measuring Cylinder Experiment =
== Refer to Chemistry Lab # 2 – Investigating Changes. No changes have been made in this experiment. Results = ==
Planning Firstly here is a list of equipment I used. Boiling tubes Weighing scales Knife Paper towels 100% solution 0% solution (distilled water) measuring beakers potato chips Cork borer. We planned to start our experiment by doing some preliminary work. We planned to set up our experiment in the following way.
== § Test tubes X 11 § 0.10 molar dm -3 Copper (II) Sulphate solution § distilled water § egg albumen from 3 eggs. § Syringe X 12 § colorimeter § tripod § 100ml beaker § Bunsen burner § test tube holder § safety glasses § gloves § test tube pen § test tube method = == = =
I hypothesize that by titrating a known amount of a substance in a solution, I can use the data from the experiment to calculate how many moles of the solution of the known concentration were required to completely react with the titrant and then using the formula C=n/V(in liters) to calculate the molarity of NaOH.
Since I am making a 0.1 Mconcentration, I will need 0.001 moles of each sugar.