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Laws of conservation of mass
To verify the law of conservation of mass
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Recommended: Laws of conservation of mass
Introduction:
A balanced chemical equation has reactants and product that has to represent a formulae. The amount of each element, number needs to be the same on either side of the equation. (E.g., HCl(aq)+NaHCO3(s) reacts to produce NaCl(aq)+H2O(I)+CO2(g)). This helps us view the study of the Law of Conservation of Mass, and how it works in this equation.
The calculation for formula, mass helps us to determine if you need to convert grams to a particular substance to moles, from a product. Moles are numbers that are in front of formulae. E.g., 6NaCl(aq), 6 is the mole for this compound. A mole would help you balance a skeleton equation, and also allows you to calculate how many moles are needed to take part in a chemical reaction.
In the laboratory experiment, we are investigating the following equation and
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In the data (Q2) shows that we have approximately 0.0416mols of NaCl(aq), and also approximately 0.0416 of NaHCO3. In the end the yield for NaCl(aq)(product), we got was 3.077%. This percent is lower because of the incident that acquired during the lab. Which leads to possible errors that can happen during the lab. The percent was lower them hundred percent was because of the spill of the solution that happen while working on the lab. We lost a lot solution which affected the amount of mole for NaCl(aq) and the yield drastically from looking at the calculation. Another possible error can be when you are cooking the solution and didn’t get to evaporate all the water that is still visible in our eye, it can cause your calculation to be incorrect and less product you are looking for in the end. Last error can be when the electrical balance can malfunction during your experiment or it doesn’t work or possibly broken. These are some of the possible errors that can happen in the lab that can affect the data
For example, a balanced chemical equation of a certain reaction specifies that an equal number of moles of two substances A and B is required. If there are more moles of B than of A, then A is the limiting reactant because it is completely consumed when the reaction stops and there is an excess of B left over. Increasing the amount of A until there are more moles of A than of B, however, will cause B to become the limiting reactant because the complete consumption of B, not A, forces the reaction to cease. Purpose
Compress the safety bulb, hold it firmly against the end of the pipette. Then release the bulb and allow it to draw the liquid into the pipette.
Thorough analysis of the graph displayed enough evidence suggesting that an increase in substrate concentration will increase the height of bubbles until it reaches the optimum amount of substrate concentration, resulting in a plateau in the graphs (figure 2). Hence; supported the hypothesis.
Also, looking at Table 1, the percent yield is shown to be 44.9%. The percent yield is how much product was recovered after the reaction was carried out. The percent yield can be used to explain why the melting point observed in the experiment didn’t match the known melting point. Obtained melting points are generally lower than the literature value melting points of a substance due to the number of impurities present in the obtained product. The percent yield of 44.9% validates that the product could have had some impurities present, and thus the lower melting point.
This graph shows that as enzyme concentration increases absorption also increases. In this case absorbance can be used to measure the enzyme’s activity, the higher the absorption the higher the activity. Since absorption increases as enzyme concentration increases, enzyme activity is promoted by increased enzyme concentrations. After a certain point enzyme activity would fail to increase as a result of increased enzyme concentration since there wouldn’t be enough substrate for all of the enzymes to react with.
“Enzymes are proteins that have catalytic functions” [1], “that speed up or slow down reactions”[2], “indispensable to maintenance and activity of life”[1]. They are each very specific, and will only work when a particular substrate fits in their active site. An active site is “a region on the surface of an enzyme where the substrate binds, and where the reaction occurs”[2].
The equation shows how 1 mol of Na2CO3 reacts with 1 mol of H2SO4, so
Unit 7: Chemical Reactions: Students will understand the basic concepts of reactions, bonding, the “mole” and how this relates to the law of conversion of matter.
Experimental error is something that always occurs, no matter how hard one tries to prevent it. One situation where error might have occurred would be in the mixing of the water and Pb(NO3)2 and mixing of the water and NaI solutions. The solids were not fully dissolved into the water and when mixed, the yellow solution had all the precipitate at the bottom of the beaker while the clear liquid remained at the top. The mixed solution was still all yellow in color but not all of it was the same shade of yellow. This might have impacted the experiment by producing more PbI2 than it was supposed
In this experiment there were eight different equations used and they were, molecular equation, total ionic equation, net ionic equation, calculating the number of moles, calculating the theoretical yield and limiting reagent, calculating the mass of〖PbCrO〗_4, calculating actual yield, calculating percent yield (Lab Guide pg.83-85).
One possible source of experimental error could be not having a solid measurement of magnesium hydroxide nor citric acid. This is because we were told to measure out between 5.6g-5.8g for magnesium hydroxide and 14g-21g for citric acid. If accuracy measures how closely a measured value is to the accepted value and or true value, then accuracy may not have been an aspect that was achieved in this lab. Therefore, not having a solid precise measurement and accurate measurement was another source of experimental error.
The Gravimetric Stoichiometry lab was a two-week lab in which we tested one of the fundamental laws of chemistry: the Law of Conservation of Mass. The law states that in chemical reactions, when you start with a set amount of reactant, the product should theoretically have the same mass. This can be hard sometimes because in certain reactions, gases are released and it’s hard to measure the mass of a gas. Some common gases released in chemical reactions include hydrogen, carbon dioxide, oxygen and water vapor. One of the best methods for determining mass in chemistry is gravimetric analysis (Lab Handout).
There is also the potential of human error within this experiment for example finding the meniscus is important to get an accurate amount using the graduated pipettes and burettes. There is a possibility that at one point in the experiment a chemical was measured inaccurately affecting the results. To resolve this, the experiment should have been repeated three times.
Stoichiometry is a chemical branch that studies amounts of substances that are involved in reactions. Stoichiometry will help you to find out how much of the mixture you will need, or how much you started with. The calculations of a stoichiometry problem depends on a balanced chemical equations. The factors of the balanced equations signifies the molar ratio (the number of moles of each reactant needed to form a certain numbers of moles of each product) of the reactants and products taking part in the reaction. From the atomic and molecular point of view the stoichiometry in a chemical reaction is very simple. For example, one mole of oxygen reacts with two moles of hydrogen,
For centuries, many scientists and researchers have pondered on the idea of combining two or more substances together to create something new. These explorations have led to the idea of what kind of reactions would occur when diverse elements are combined. This is a concept known as chemistry, a part of science that corresponds with how matter is created from different properties and the process it goes through to create a new substance. Chemistry is a scientific concept that is used in everyday life and is a crucial part in the development of new technology and substances that allow today’s quality of life. The use of chemistry branches off into many different routes, including medical related fields, agriculture, and even in weapons of