Description Fill in the template provided. 6 videos. background and procedure provided. Need reference and in-text citation. Use the data from file: Data set EP3
Description Make sure you understand the overall picture before you come to lab. In Part A you will determine the mole mole relationship between your starting material, sodium bicarbonate ("sodium hydrogen carbonate") and the product, CO2 gas. Once you know this relationship from Part A, you will use that known relationship to analyze the amount of sodium bicarbonate in an antacid. (The label claims 1.916 g NaHCO3 per tablet.) Check with me before you move onto Part B so I can make sure you have the correct reaction! Below I show a diagram of how to arrange your reactants so you can weigh the correct values: In Part B, you will use the balanced reaction you picked from your data in Part A, along with the moles of CO2 produced, to determine how many moles of sodium bicarbonate are in the antacid tablet. (This relationship will come in at lines (e) and (f) of the table in Part B.) When you add sodium bicarbonate to the acid, add slowly. If the mixture bubbles over the beaker and loses liquid, you will need to start over. Also note that if the bicarbonate spills outside of the beaker, this will also cause significant error in the results. Complete calculations from Part A and have me check your reaction (sign your notebook) before moving on. Only then may you obtain the antacid. Antacid contains some insoluble binding agents to help hold the pill shape. That means there will be some white junk in your reaction for Part B even after it has gone to completion. After you have completed the pre-lab calculation and understand how the procedure works, watch the videos for Part A. Complete the calculations during our lab period and make sure you have the correct results before moving on to Part B. Your results in Part B depend on your results from Part A so ask for help and check with me before moving on to Part B! (I normally only hand out the Alka Seltzer after you have selected and written your reactions for Part A.) Videos for this lab are located on my youtube channel, Stoichiometry Playlist: https://www.youtube.com/playlist?list=PLuuIip6svThbeLGRRsfXq_NCErDVXH1Qm [+] prelab lecture: https://www.youtube.com/watch?v=cG3wmygIAok&list=PLuuIip6svThbeLGRRsfXq_NCErDVXH1Qm&index=1&t=699s [+] Question 1:Results Part A: Reaction Stoichiometry of Sodium Bicarbonate with Acetic Acid. Enter the results for Part A, based on the masses determined in the lab video for Part A. Although your data may not be rounded, round the answers for the results below to the appropriate number of significant figures. Trial 1 Trial 2 Trial 3 mass of CO2 gas released g g g moles of CO2 gas released mol mol mol moles of CO2 gas, corrected for amount dissolved mol mol mol moles of NaHCO3 used mol mol mol Using the results above, select the reaction that best described the chemical reaction between sodium bicarbonate and acetic acid. (Note that the order may not match the lab manual, so check each reaction carefully.) NaHCO3(s) + HC2H3O2(aq) ? CO2(g) + H2O(l) + NaC2H3O2(aq) 2 NaHCO3(s) + HC2H3O2(aq) ? CO2(g) + Na2CO3(aq) + H2O(l) + 2 CH2O(aq) NaHCO3(s) + HC2H3O2(aq) ? 2 CO2(g) + CH3OH(aq) + NaH(aq) Question 2:Results Part B: Analysis of an Antacid Enter the results for Part B, based on the masses determined in the lab video for Part B. Round all answers below to 2 significant figures. (Trial 2 produced only one significant figure, but we will use 2 sig figs in this section.) Trial 1 Trial 2 mass of CO2 gas released g g moles of CO2 gas released mol mol moles of CO2 gas, corrected for amount dissolved mol mol Experimental moles of NaHCO3 mol mol Experimental mass of NaHCO3 g g Average mass of NaHCO3 for two tablets: g Question 3:Describe how your data in Part A supports your conclusion about the appropriate reaction in Part A. Question 4:In Part B, suppose some of your reaction mixture splashed out of the beaker when you dropped the tablets into the acetic acid. How would this affect your measurements? Be as specific as possible. How would the splashing error affect the amount of CO2 determined, and consequently, would your final calculated mass of sodium bicarbonate in the tablet be artificially high or artificially low? Question 5:To calculate the percent error, use the mass of sodium bicarbonate in one tablet of Alka-Seltzer recorded from the package for the true value and your average mass of NaHCO3 for the experimental value. (Show 1 significant figure) %
Description EJERCICIOS SELECCIONADOS- CAPÍTULO 6 (Referencia: Timberlake, Karen C. Chemistry: An Introduction to General Organic, and Biological Chemistry Tenth edition, Harper Collins Publishers, 2011.) 6.1 Considerando la teoría cinética molecular de los gases, justifícalas siguientes afirmaciones: a. Los gases se mueven más rápido a mayores temperaturas porque b. Los gases se pueden comprimir más que los líquidos o los sólidos. 6.7 En una escalada al Monte Whitney, la presión atmosférica es de 467 mmHg. ¿Cuál es la presión en las siguientes unidades? a. atm b. mmHg 6.13 Un gas con un volumen de 4.0 L se almacena en el interior de un contenedor cerrado. Indica los cambios de presión que se producirán si el volumen experimenta los siguientes cambios a una temperatura constante: a El volumen se comprime a 2.0 L. b. El volumen se expande a 12 L. c. El volumen se comprime a 400 mL. 6.17 Una muestra de nitrógeno (N2) ocupa un volumen de 50.0L a una presión de 760 mmHg. ¿Cuál es el volumen del gas a cada una de las siguientes presiones, si no se producen cambios de temperatura? a. 1500 mmHg b. 2.0 atm c. 0.500 atm 6.19 El ciclopropano (C3H6) es un anestésico general. Una muestra de 5.0L tiene una presión de 5.0 atm, ¿cuál es el volumen del anestésico que se administra a un paciente a una presión de 1.0 atm? 6.26 Un gas tiene un volumen de 4.00L a 0 ° C ¿Qué temperatura final, en grados Celsius, es necesaria para que el volumen del gas cambie a los siguientes volúmenes, considerando que P y n se mantienen constantes? a. 100L b. 1200 mL c. 250 mL d. 50.0 mL 6.28 Una burbuja de aire tiene un volumen de 0.500L a 18 °C. Si la presión no cambia, ¿cuál es el volumen en litros a cada una de las siguientes temperaturas? a. 0 °C b. 425 K c.- 12 ° C d. 575K 6.37 Una burbuja de 100.0 mL con gases calientes que escapan de un volcán a 225 °C tiene una presión de 1.80 atm. ¿Cuál es el nuevo volumen de la burbuja fuera del volcán, cuando la temperatura es de -25 °C y la presión de 0.80 atm? 6.41. Una muestra contiene 1.50 moles de gas neón en un volumen de 8.00L. Calcula el nuevo volumen del gas en litros cuando, manteniendo constantes temperatura y presión, se dan los siguientes cambios en la cantidad del gas: a. Se produce la pérdida de la mitad del gas. b. Se añade una muestra de 25.0 g de neón al gas que ya está en el recipiente c. Se añade una muestra de 3.50 moles de 02 al gas neón que ya está en el recipiente. 6.49 En una mezcla gaseosa, las presiones parciales son: nitrógeno, 425 torr; oxígeno, 115 torr y helio, 255 torr. ¿Cuál es la presión total (torr) ejercida por la mezcla de gases?
Description Hello Femma, This is my last lab assignment of the quarter. I am unable to send you the link to the simulation because I cannot open it. It's a jar.file. I downloaded the new Java but I still cannot get it to work. I have attached the assignment. I can give you my course log on information to see if you can access the lab. Please let me know if that is possible, Thank you!
Description Requirements Submit your assignment using the following steps: Take pictures of each page of your worksheet using a digital device after you have solved it. Paste all pictures in a Word or PowerPoint file. Save this file as a Word, PowerPoint, or pdf file. Upload this file. Please be aware that submitting individual pictures is not permitted and will not be graded. Submission should be one file only containing all your work. Please ensure your work is legible.
Description There are two sections to this assignment. BOTH must be completed Section 1 Discussion questions Each answer must be 100 words Each answer must be in your own words. What are atoms? What is an Electrical Charge? Define elements and compounds. Give an example of elements and compounds and describe some of the properties of your examples. What are metals, nonmetals, and metalloids? Definition of the Periodic Table. List the different types of chemical reactions listed in your textbook. (Synthesis, Decomposition reactions, Single displacement reaction) Give an example. Describe a real world use of the chemical reaction that you provided. Definition of Chemical Reactios What is Stoichiometry? Section 2 Week 2 Exercises Prepare written answers to the following exercises: Determine the number of electrons, protons and neutrons in each isotope of titanium based on the table below. Determine its atomic mass. For each compound listed below write down the correct formula and calculate the formula mass. Isotope Mass (Da) Natural Abundance (%) Electrons Protons Neutrons Atomic Mass 46Ti 45.9526294 8.25 47Ti 46.9517640 7.44 48Ti 47.9479473 73.72 49Ti 48.9478711 5.41 50Ti 49.9447921 5.18 Iron(III) sulfide Aluminum nitrate Carbon tetrachloride Perchloric acid Ammonium hydroxide Aluminum is refined from the mineral bauxite, which is mostly aluminum hydroxide (Al(OH)3). Presuming that an ore sample is approximately 54% bauxite, how much Al could be extracted from 1 kg of ore? Calcium carbonate (a weak base) reacts with nitric acid (a strong acid) quantitatively in the following reaction to form calcium nitrate, water and carbon dioxide: Metallic sodium reacts vigorously with liquid bromine in the following reaction: The combustion of gasoline (C8H18) with excess oxygen produces carbon dioxide and water. How many kg of carbon dioxide (CO2) are formed per kg of CaCO3 reacted? Presume that there is an excess of HNO3 available. 1 kg of Na is brought into contact with 3 kg of liquid bromine. Presuming that the reaction is quantitative and proceeds to completion, determine the limiting reagent and the quantity of NaBr formed. Determine the amount of excess reagent remaining after the reaction is complete. Write a balanced chemical reaction for the combustion of gasoline to yield carbon dioxide and water. Presuming that a tank of gasoline contains 80 liters and that its density is 0.77 kg/liter, determine how many kg of CO2 are produced for each tank of gasoline burned.
Description Here is a redox reaction between Mg metal and chlorine gas: 2Cr(s) + 3Cl2(g) --> 2CrCl3 (s) (a) What is getting oxidized? (b) What is getting reduced? (c) How many electrons are being transferred?
