Conclusion: Compare Trial 1 and Trial 2. The Trial 1 change in mass are 12.5g, however Trial 2 changes in mass is 1.2g. The Trial 1 change in mass is more than Trial 2. And I think the Low of Conservation of Mass violated in the Trial 1 is can be exist. Because the Trial 1 actually the soda with vinegar have Chemical reactions occur and chemical
Copper Transformations Prelab Questions Three metals ions are Magnesium, Iron, and Nickel. Iron is used in the sea with iron rich minerals, for substances. Iron was also used in the formation of earth.
K.D.A. Saboia et al. , (2007) have been prepared the Bi4Ti3O12–CaCu3Ti4O12 {[BIT(X)–CCTO(100-X)]} composite powders through solid state reaction method and calcined in the range of 900 to 1020 ºC for 12 h. The as-prepared powders have modified in the form of thick film onto alumina ceramic substrate by utilizing screen printing. At 100 Hz, the value of dielectric constant (κ) of CCTO100 and BIT100 is 316.61 and 53.64 respectively. Conversely, the composite with X=20 % shows an unexpected dielectric constant of 409.71, which is around 20% higher in comparison with the CCTO.
- A hydrate is a salt that contains water as a part of its crystal structure. The hydrate used in this lab was Copper (ll) Sulfate Pentahydrate. To heat the hydrate in this lab a crucible is needed. A crucible is a heat resistant container used to heat things to high temperatures. In this lab a mole was used to determine the measurements of all substances.
After the reaction finishes, the amount of CO2 that was released is calculated and then using the molemap, it is possible to solve for the amount of the unknown substance. The grams of the unknown powder are then divided by the moles of the substance to get the molar mass. This molar mass is then compared to the molar mass of the known substances. Unknown substance A is lithium carbonate since the molar mass produced in the experiment is 66.68 g/mol and the molar mass of lithium carbonate is 73.89 g/mol. Unknown substance B has a molar mass of 146.70 g/mol which is inconclusive since it is too different from the other molar masses.
Even if chemical reactions occur the total mass should stay the same. When doing this experiment there will be times when the mass of a sample cannot be found directly and the formula below will need to be used to find the sample’s mass. Formula 1 : Mass of sample= mass of evaporating dish with sample – mass of evaporating dish For completing this experiment the use of percentages will be used in order to determine the percent of each component in the total mixture. Below is the formula used in order to determine the percentages of each component of a mixture.
Balanced Chemical Equation: Cu(s) + 4HNO3(aq) —> Cu(NO3)2 (aq) + 2NO2 (g) + 2H2O (l) Reaction 2: when sodium hydroxide (NaOH) is added to copper (II) nitrate (Cu(NO3)2), a double displacement reaction will occur. Copper and sodium will displace each other to create copper (II) hydroxide and sodium nitrate. Balanced Chemical Equation: Cu(NO3)2 (aq) + 2NaOH (aq) —> CuOH2 (s) + 2NaNO3 (aq) Reaction 3: When copper (II) hydroxide is heated, a decomposition reaction will occur. The reaction will decompose forming two compounds, Copper (II) oxide, and water. Balanced Chemical Equation: Cu(OH)2 (s) + Heat —> CuO (s)
The mole ratio can be used as a conversion factor between different quantities. The first step to a stoichiometry problem is to balance the equation. Next, convert the known reactant amount to moles. Then, find the moles of the reactant using the mole ratios. Lastly, convert moles to mass.
This experiment was not carried out in chronological order to maximize efficiency. First the volume (3.33mL) of needed liquid ammonium sulfate was calculated based on the assigned 25% saturation. 3.33mL of the liquid ammonium sulfate was added to 10mL of the protein extract (given by the instructor) in a centrifuge tube to precipitate the protein out. Water was then added to a second centrifuge tube to balance out the mass in the centrifuge. The mass of the mixture was weighed and the water was measured (using a scale) to weigh the same as the mixture.
For example, in the first experiment (A+B+C), the procedure is to mix a teaspoon of calcium (A), ½ teaspoon of sodium bicarbonate (B), and 100 drops of phenol red solution (C) in a sealable plastic bag. As a result, there were several visible chemical changes that occurred over the course of time: there is an energy change (increase in temperature), color change to mustard substance, gas released, and changed from a solid to liquid state. Another observation seen was how without the mixture of the phenol red solution or deoxidized water, little to no visible chemical or physical changes occurred. For example, when calcium chloride and sodium bicarbonate are mixed together, there are no occurring changes: both solids don’t dissolve, their colors stay the same, and no gas or bubbles are released. Some questions arise concerning the changes observed in the experiments are the following: Does the interaction of phenol red cause the observed color change in the overall phenomenon?; what interaction is responsible for the increase and decrease in temperature change; can there be any reaction without the presence of water-based solutions?; and if the amount of each chemical was adjusted to be added more or less of in the combinations; would there be more or less chemical changes visible to observe in the individual experiments?
Introduction: Stoichiometry is the calculation of the quantities of chemical elements or compounds involved in chemical reactions. It is the amount of substances used before the reaction and the product of the reaction. The Law of Conservation of Mass states that matter can be changed from one form into another, mixtures can be separated or made, and pure substances can be decomposed, but the total amount of mass remains constant.
The lab was performed using the thermometer, the graduated cylinder, the scale, the pipet, and many more lab equipment. There were four separate parts. The first part of the experiment consists of examining the meter stick, and using the meter stick to measure the length and width of the lab notebook. The second part of the experiment consists of observing the graduated cylinder. You had to fill it with water and estimate the closest value to the measurement on the side of the graduated cylinder.
Purpose This experiment is to determine the concentration of the solute copper sulfate pentahydrate, and the unknown solution, by passing different wavelengths of light through each solution. Procedure Weigh out approximately 5g of copper sulfate pentahydrate. Record the mass and place the solute into a 50 mL volumetric flask. Fill half of the flask with distilled water, add the stopper for the flask, and lightly shake the flask, until the copper sulfate pentahydrate fully dissolved.
Finding the empirical formula for hydrated copper sulfate using calculations to find the amount of each element present in the copper ion, sulfate ion, and water while also comparing the empirical formula to a literature value. Christian Cooper Alexis Powers CHM1210-18M/Gregory Bowers 11-5-15 Purpose: To begin, there are several different goals, techniques, and claims to note in the experiment involving hydrated copper sulfate. The overall goal of this experiment is to find the empirical formula and compare it with a literature value. Yet, in finding the empirical formula of hydrated copper sulfate, there are several process for it to get through, like finding the percentages of copper, water, and finally sulfate.
This applies the same to my example above, same number of particles, different, elements, therefor, different masses. Another concept we need to master is Balancing. Balancing chemical equations is quite tricky, that is the process wherein you put coefficients, which signifies how many element is put up in that particular equation, in front of the element/coefficient. It is pretty tricky and we need to master it. Here is an example of an unbalanced chemical equation, H2 + O2 = H2O
