Lab Report Stoichiometry With Kitchen Chemistry

If the amount of baking soda used in this experiment increases (0.2 g, 0.4 g, 0.6 g, 0.8 g, or 1 g), then the volume (mL) of the carbon dioxide released from the decomposition will also increase. In any chemical reaction, the atoms of the reactants are rearranged to form the product. Thus, as particles cannot be created or destroyed, the mass of the carbon dioxide released cannot increase or decrease unless the mass of the baking soda is changed.

In your laboratory notebook sum these two reactions to find the stoichiometric factor that relates moles of

5. Zoom Out by clicking on the green arrow next to the Save button. Click on the Stockroom and then on the Clipboard and select Balloon Experiment N2. Again, set the temperature, pressure, and moles to 298 K, 1.00 atm, and 0.300 moles, respectively. You may have to click on the Units button to change some of the variables to the correct units. Repeat the experiment with this gas labeling the data link ‘Real Gas N2.’

Example problem: How many grams of carbon dioxide are produced when 20.0 g acetylene (C2H2) is burned?

Introduction The purpose of this experiment was to determine the amount of NaHCO3 in Alka-Seltzer tables by calculating the mass of CO2 released by an Alka-Seltzer tablet when dropped into water, vinegar, and various combinations of both. Background Alka-Seltzer is an over the counter drug used to relieve cold symptoms while neutralizing stomach acid. Alka-Seltzer contains anhydrous citric acid (antacid) and sodium bicarbonate (antacid). When the table dissolves in water, NaHCO3 dissociates to form HCO3 and Na.

The relationship between mass of the product and mass of the reactant taken directly from the balanced chemical equation and molar masses of the involved species is used in this experiment to find the mass of the unknown sample. In this experiment the unknown sample is found out ,which will be on of the following salts:NaHCO3,Na2CO3,KHCO3K2CO3.Only the fixed mass of reactant react together to produce fixed mass of products.

21. Quickly inserted the CO2 probe into the bottle to detect how much carbon dioxide will be produced (PPM). 22. Recorded how much carbon dioxide was produced (PPM) during the reaction after 10 minutes for this trial into a data table with significant figures in

CO2's weight will allow me to determine the weight of the sodium bicarbonate by using stoichiometry and will be tested by dissolving Alka Seltzer in water and vinegar to cause the reaction.

Pre-Lab: A) Hydrate- a compound, typically a crystalline one, in which water molecules are chemically bound to another compound or an element. B) Water of hydration (crystallization)- water that is chemically combined with a substance to form a hydrate and can be expelled (as by heating) without essentially altering the composition of the substance. C) Dehydration- the loss or removal of water from something.

Give molecular orbital diagram with drawings of the molecular orbitals. You may have to rerun the calculation with pop=full included.

In this experiment, you will: Observe the reaction which produced the oxygen by KClO_3. Learn how to collect the gas through water displacement method. How to use ideal gas equation to calculate the amount of gas produced. Calculate the percent yield of the reaction. Introduction

To reduce error for this experiment, it was crucial to collect right amounts of gases from the reaction and handle it quickly for the next step due to properties of gases.

Place gum (still in wrapper) onto scale. Measure its mass, and record the mass in the second column.

There is a piece of chalk that is made up of one hundred percent calcium carbonate, or CaCO3, and you must determine the number of atoms of calcium, carbon, and oxygen it takes to write your name on the chalkboard. First, we must determine the mass of the piece of chalk. After the weight is found, you must find the molar mass of the compound, to find the molar mass of CaCO3 you must multiply the amount of each element by its atomic mass and and them all together, for example, there are three oxygens and to find the molar mass of oxygen you must multiply its quantity, three, by its atomic mass, 16.00, and you get the molar mass of oxygen which is 48 grams, you do this to the rest of the compound which will come out to be 100.09 grams. Now that

= (89.14 + 83.72 + 82.7 + 86.54 + 93.87 + 88.88 + 92.5 + 90 + 97.5) ÷ 9