EXPERIMENT NO. 7
CALORIMETRY
OBJECTIVES
To compute the heat capacity of a styrofoam-cup calorimeter
To compute the heat of neutralization of 1.0 M hydrochloric acid and 1.0 M sodium hydroxide, the heat of dilution of concentrated sulfuric acid, and the heat of solution of solid ammonium chloride
CONCLUSION
heat capacity of a styrofoam-cup calorimeter
(write the computation here)
heat of neutralization
(write the computation here)
Showing posts with label Chemistry. Show all posts
Showing posts with label Chemistry. Show all posts
GAS LAWS
EXPERIMENT NO. 6
GAS LAWS
OBJECTIVES
To demonstrate the combined gas law
To compute the molar mass of ammonia by using Grahams law of diffusion
CONCLUSION
Conclusion of this experiment no. 6 about gas laws can be stated that the combined gas law combines Charles’s law, Boyle’s law, and Gay-Lussac’s law. These laws each relate one thermodynamic variable to another mathematically while holding everything else constant. Charles’s law states that volume and temperature are directly proportional to each other as long as pressure is held constant. Boyle's law asserts that pressure and volume are inversely proportional to each other at fixed temperature. Finally, Gay-Lussac's law introduces a direct proportionality between temperature and pressure as long as it is at a constant volume.
Grahams law of diffusion states that the rates of diffusion for gases are inversely proportional to the square roots of their molar masses under the same conditions of temperature and pressure. The rate of diffusion is equal to the distance traveled divided by the time of travel of the gas. Since temperatures are equal to each other, we can wire the equation as:
M d
=
M d
We can substitute the chemical equation HCl + NH ® NH Cl and simplify the equation as and compute for the experimental Molar Mass of Ammonia.
MHCl(dHCl)² 36.46g/mol (12.3cm)²
MNH = = = 17.60 g/mol
(dNH )² (17.7cm)²
The computed experimental Molar Mass of the ammonia is 17.60 g/mol and the given molar mass of hydrogen chloride is 36.46 g/mol. The ammonia traveled on the glass tubing longer distance because the mass of the hydrogen chloride is heavier compared to the mass of ammonia.
GAS LAWS
OBJECTIVES
To demonstrate the combined gas law
To compute the molar mass of ammonia by using Grahams law of diffusion
CONCLUSION
Conclusion of this experiment no. 6 about gas laws can be stated that the combined gas law combines Charles’s law, Boyle’s law, and Gay-Lussac’s law. These laws each relate one thermodynamic variable to another mathematically while holding everything else constant. Charles’s law states that volume and temperature are directly proportional to each other as long as pressure is held constant. Boyle's law asserts that pressure and volume are inversely proportional to each other at fixed temperature. Finally, Gay-Lussac's law introduces a direct proportionality between temperature and pressure as long as it is at a constant volume.
Grahams law of diffusion states that the rates of diffusion for gases are inversely proportional to the square roots of their molar masses under the same conditions of temperature and pressure. The rate of diffusion is equal to the distance traveled divided by the time of travel of the gas. Since temperatures are equal to each other, we can wire the equation as:
M d
=
M d
We can substitute the chemical equation HCl + NH ® NH Cl and simplify the equation as and compute for the experimental Molar Mass of Ammonia.
MHCl(dHCl)² 36.46g/mol (12.3cm)²
MNH = = = 17.60 g/mol
(dNH )² (17.7cm)²
The computed experimental Molar Mass of the ammonia is 17.60 g/mol and the given molar mass of hydrogen chloride is 36.46 g/mol. The ammonia traveled on the glass tubing longer distance because the mass of the hydrogen chloride is heavier compared to the mass of ammonia.
STOICHIOMETRY
EXPERIMENT NO. 5
STOICHIOMETRY
OBJECTIVES
1. To differentiate limiting reactant and excess reactant
2. To compute the theoretical yield and the percent yield of a chemical reaction.
CONCLUSION
Stoichiometry is the quantitative study of reactants and products in a chemical reactions. In this experiment, we can conclude that Limiting reactant is the reactant in a chemical reaction that limits the amount of product that can be formed. Therefore, whenever all of the limiting reactant is consumed, the reaction will stop. The chemical reaction that remains when a reaction stops and the limiting reactant is completely consumed is called Excess Reactant. The Excess reactant remains because there is nothing with which it can react.
Theoretical Yield of a reaction is the amount of product that would be formed if the reaction went to completion. It is calculated from the balanced equation based on the amount of reactants used. First, you must balance the reaction and determine the stoichiometry or ratios of reactants to products. Then assume that each reactant is a limiting reactant and compute the amount of product. Next, determine which reactant is limiting, this has a smaller amount of product. Lastly, calculate the grams of product corresponding to the number of moles expected by converting the moles to grams.
To compute the percent yield, divide the actual yield, amount based on the experiment, by the theoretical yield, computed product, and multiply the product by 100%. Percent yield is the efficiency of a chemical reaction.
STOICHIOMETRY
OBJECTIVES
1. To differentiate limiting reactant and excess reactant
2. To compute the theoretical yield and the percent yield of a chemical reaction.
CONCLUSION
Stoichiometry is the quantitative study of reactants and products in a chemical reactions. In this experiment, we can conclude that Limiting reactant is the reactant in a chemical reaction that limits the amount of product that can be formed. Therefore, whenever all of the limiting reactant is consumed, the reaction will stop. The chemical reaction that remains when a reaction stops and the limiting reactant is completely consumed is called Excess Reactant. The Excess reactant remains because there is nothing with which it can react.
Theoretical Yield of a reaction is the amount of product that would be formed if the reaction went to completion. It is calculated from the balanced equation based on the amount of reactants used. First, you must balance the reaction and determine the stoichiometry or ratios of reactants to products. Then assume that each reactant is a limiting reactant and compute the amount of product. Next, determine which reactant is limiting, this has a smaller amount of product. Lastly, calculate the grams of product corresponding to the number of moles expected by converting the moles to grams.
To compute the percent yield, divide the actual yield, amount based on the experiment, by the theoretical yield, computed product, and multiply the product by 100%. Percent yield is the efficiency of a chemical reaction.
CHANGES OF MATTER AND ENERGY TRANSFORMATION
EXPERIMENT NO. 4
CHANGES OF MATTER AND ENERGY TRANSFORMATION
OBJECTIVES
1. To compare a physical change and a chemical change
2. To illustrate the law of conservation of mass
3. To differentiate the different types of chemical reactions
CONCLUSION
In performing the 4th experiment, Changes of Matter and Energy Transformation, I conclude that Matter can be Physically or Chemically change. In Physical change of matter, it only change the extensive property of matter while in Chemical change, changes occur on the intensive property of matter and forming a new and different product.
The Law of Conservation of Mass states that the mass of substances in a closed system will remain constant no matter what processes are acting inside the system. Matter may change form, it can neither be created or destroyed thus the mass of the reactants must always be equal to the mass of the products.
Chemical reactions can be place into 4 general categories naming Combination, Decomposition, Single Replacement and Double Replacement.
In Combination, also known as synthesis, 2 or more element or compounds combine to form a more complex substance while in Decomposition, a compound or complex substance is broken down into two or more elements or/and compounds. Combination and Decomposition is the exact opposite or each other.
Single replacement / Substitution / Single displacement is a reaction in which a free element, more active than the element to be replaced, replaces another element is a compound. In Double replacement / Metathesis / Double displacement / Double decomposition, two compounds exchange metallic and nonmetallic portions to form two new compounds.
General Forms
Combination Decomposition Substitution Metathesis
A + B ® C C ® A + B A + BC ® B + AC AB + CD ® AD + CB
CHANGES OF MATTER AND ENERGY TRANSFORMATION
OBJECTIVES
1. To compare a physical change and a chemical change
2. To illustrate the law of conservation of mass
3. To differentiate the different types of chemical reactions
CONCLUSION
In performing the 4th experiment, Changes of Matter and Energy Transformation, I conclude that Matter can be Physically or Chemically change. In Physical change of matter, it only change the extensive property of matter while in Chemical change, changes occur on the intensive property of matter and forming a new and different product.
The Law of Conservation of Mass states that the mass of substances in a closed system will remain constant no matter what processes are acting inside the system. Matter may change form, it can neither be created or destroyed thus the mass of the reactants must always be equal to the mass of the products.
Chemical reactions can be place into 4 general categories naming Combination, Decomposition, Single Replacement and Double Replacement.
In Combination, also known as synthesis, 2 or more element or compounds combine to form a more complex substance while in Decomposition, a compound or complex substance is broken down into two or more elements or/and compounds. Combination and Decomposition is the exact opposite or each other.
Single replacement / Substitution / Single displacement is a reaction in which a free element, more active than the element to be replaced, replaces another element is a compound. In Double replacement / Metathesis / Double displacement / Double decomposition, two compounds exchange metallic and nonmetallic portions to form two new compounds.
General Forms
Combination Decomposition Substitution Metathesis
A + B ® C C ® A + B A + BC ® B + AC AB + CD ® AD + CB
CLASSIFICATION OF MATTER
EXPERIMENT NO. 3
CLASSIFICATION OF MATTER
OBJECTIVES
1. To differentiate an element from a compound
2. To identify an electrolyte and a non-electrolyte
3. To examine the color reactions of different acids and bases to different indicators
4. To define neutralization
5 To prepare ferric oxide sol, sulfur sol, and coconut oil-water emulsion
6. To illustrate Tyndall effect and coagulation of colloidal systems
CONCLUSION
CLASSIFICATION OF MATTER
OBJECTIVES
1. To differentiate an element from a compound
2. To identify an electrolyte and a non-electrolyte
3. To examine the color reactions of different acids and bases to different indicators
4. To define neutralization
5 To prepare ferric oxide sol, sulfur sol, and coconut oil-water emulsion
6. To illustrate Tyndall effect and coagulation of colloidal systems
CONCLUSION
Upon performing the 3rd experiment, Classification of Matter, I conclude that Elements are the simplest form of atoms and compound is compose of two or more elements through chemical reaction. Where some compounds are Electrolyte, conduct electricity, because they are ionic which allow charges to pass through.
I also conclude that neutralization between acid and base, which can be indicated by the use of different indicators like cabbage and nitromine, reacts to form water and salt.
Tyndall Effect is the scattering of light by a colloidal dispersion. Brownian Movement is a movement which the particles changes speed and direction erratically. Which, colloidal systems can be stable or unstable depending on the tendency of the colloidal system to remaun a true solution.
Matter occupies space and has mass and can be classified as pure substance or a mixture where colloid is a type of mixture and pure substance can either be a element of a compound. Electrolyte is a compound that when dissolved in water, it forms a solution that can conduct electricity.
I also conclude that neutralization between acid and base, which can be indicated by the use of different indicators like cabbage and nitromine, reacts to form water and salt.
Tyndall Effect is the scattering of light by a colloidal dispersion. Brownian Movement is a movement which the particles changes speed and direction erratically. Which, colloidal systems can be stable or unstable depending on the tendency of the colloidal system to remaun a true solution.
Matter occupies space and has mass and can be classified as pure substance or a mixture where colloid is a type of mixture and pure substance can either be a element of a compound. Electrolyte is a compound that when dissolved in water, it forms a solution that can conduct electricity.
SEPARATION TECHNIQUES
EXPERIMENT NO. 2
SEPARATION TECHNIQUES
OBJECTIVES
To demonstrate how to separate the components of a mixture by decantation, filtration evaporation, distillation, adsorption, and sublimation
CONCLUSION
Throughout the experiment, I conclude that mixtures of different substances have different ways in separating them. It depends on what kind of substances ore being mixed together, what state the substance is and which is the solute or the solvent. Decantation, filtration evaporation, distillation, adsorption, and sublimation are the different ways to separate two or more different substances.
SEPARATION TECHNIQUES
OBJECTIVES
To demonstrate how to separate the components of a mixture by decantation, filtration evaporation, distillation, adsorption, and sublimation
CONCLUSION
Throughout the experiment, I conclude that mixtures of different substances have different ways in separating them. It depends on what kind of substances ore being mixed together, what state the substance is and which is the solute or the solvent. Decantation, filtration evaporation, distillation, adsorption, and sublimation are the different ways to separate two or more different substances.
BASIC LABORATORY TECHNIQUES
EXPERIMENT NO. 1
BASIC LABORATORY TECHNIQUES
OBJECTIVES
1. To use common laboratory apparatus in measuring mass, length, volume, temperature, and density
2. To compute the accuracy and the precision of a set of scientific measurements
3. To apply the concept of significant figures in reporting correctly scientific measurements
CONCLUSION
This experiment helped us how to use basic laboratory apparatus in measuring mass, length, volume, temperature and density. By the use of this measurements, we learned how to compute the accuracy and precision of the results and proper way in reporting in significant figures.
In performing this experiment number 1, Basic Laboratory Techniques, I conclude that in doing laboratory experiment, you are required to have a careful and keen observation plus proper and right laboratory techniques and operations to obtain correct results. Furthermore, using the correct formulas in computing accuracy and precision and reporting it on a right way by using the rules on scientific notation.
BASIC LABORATORY TECHNIQUES
OBJECTIVES
1. To use common laboratory apparatus in measuring mass, length, volume, temperature, and density
2. To compute the accuracy and the precision of a set of scientific measurements
3. To apply the concept of significant figures in reporting correctly scientific measurements
CONCLUSION
This experiment helped us how to use basic laboratory apparatus in measuring mass, length, volume, temperature and density. By the use of this measurements, we learned how to compute the accuracy and precision of the results and proper way in reporting in significant figures.
In performing this experiment number 1, Basic Laboratory Techniques, I conclude that in doing laboratory experiment, you are required to have a careful and keen observation plus proper and right laboratory techniques and operations to obtain correct results. Furthermore, using the correct formulas in computing accuracy and precision and reporting it on a right way by using the rules on scientific notation.
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