3. SEP Analyze Data Calculate the ratio of the moles of product produced to the moles of each of the reactants used. (Write two separate ratios.)
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- Please find the CO2 amount and show the calculation: Air composition (apprx) = 80% N2 and 20% O2 (mol basis only)Average molecular weight of Air = (0.8 x 28 + 0.2 x 32) = 29 g/mol (apprx) Math Sample:2kg pure charcoal (12C) is to be burnt completely with air. Find the air, CO2 andN2 amount in kg’s.Solution:C + O2 = CO2 (you must use a balanced equation)Therefore from the mole ratio of the reaction we write,C : O2 : CO2 = 1:1:1and from air composition we gotO2 : N2 : Air = 1:4:5 Given, 2 kg C = 2000 g/ (12 g/mol) = 166.67 mole CTherefore, similar mole of O2 required. So equivalent Air supposed to be 5times than the mole amount of O2 and released N2 will be 4 times than therequired O2. Therefore, Air amount = 5 x 166.67 moles= 833.34 moles= (833.33x29/1000) kg= 24.17 kg air Similarly N2 released amount will be = (166.67 x 4 x 28/1000) kg = 18.67 kgFind CO2 amount by yourself! (Isn’t it 7.34 kg?)Pure CO2 may be prepared by treating limestone with sulfuric acid. The limestone used in the process contains CaCO3, MgCO3 and inert. The acid used contains 12% H2SO4 by weight The residue from the process had the following composition. CaSO4 – 8.56%; MgSO4 – 5.23%; H2SO4 – 1.05%; Inert – 0.53%; CO2 – 0.12%; H2O – 84.51%; During the process, the mass was warmed where CO2 and H2O were removed. Calculate the following.a) The analysis of lime stone and b) The % excess acid used.I need help finding the therotical yield and the percent yield with the data provided: mass of filter paper crude= 0.184 g mass of filter paper+ crude product=1.211 g mass of filter paper pure=0.182 g mass of filter paper + pure product= 0.809 g melting point of pure product= 105-110
- Mass of Na2CO3.H2O (g) = 2.12g (g) Mass of the CaCl2.2H2O (g) = 1.98g Mass of the top funnel + filter paper (g) = 15.85g Mass of top funnel + filter paper + CaCO3 collected (g) = 17.81g CaCl2 + Na2CO3 ==== CaCo3 + 2NaCl Theoretical yield in moles and grams? Moles of reagent in excess left unreacted? Mass of precipitate? Experimental yield? Percent yield?Sample: Saline 0.900% (m/v), in sodium chloride (NaCl). Data: M.A. (g/mol): Na = 22.9898; K = 39.0983; Cr=51.9961; Ag = 107.8682; Cl = 35.453; N=14.0067; O = 15.9994. Material available in the laboratory's warehouse: Reagents: distilled water; standardized solution of silver nitrate (AgNO₃), at a concentration of 0.09980 mols/L; Potassium chromate solution (K₂CrO₄) 1%; ammoniacal ferric alum solution [Fe(NH₄)(SO₄)₂] and; nitrobenzene (or cooking oil, alternatively); 0.1000 mols/L potassium thiocyanate (KSCN) standard solution. Glassware: beakers of all sizes available on the market; 50, 100, 150, 200 and 250 ml Erlenmeyers; 10.00 and 25.00 mL volumetric pipettes; 15.00 mL burette; 30.00, 50.00 and 100.00 mL volumetric flasks Calculate the molarity of saline, in terms of the NaCl concentration (concentration in mols/L). (a) 0.900 mols/L (b) 5.84 mols/L (c) 0.154 mols/L (d) 0.0154 mols/LWatch the following video, and identify the reaction type. Note: At the end of the video, they test of hydrogen gas, a flammable gas, which makes a popping sound when exposed to flame. There are two products formed. https://www.youtube.com/watch?v=A4XITC225uk&feature=emb_title (1 min 8 sec video)
- Hi! I'm a college student and i need your help in answering my chemistry subject. Please do help me and I promise to rate it helpful. Please put an understandable or clearer solutions and if possible you can put a brief explanation. Thank you so much and God bless! Nitrogen oxide is oxidized ina air to give brown nitrogen dioxide. If you have 2.2 moles of NO, 2NO(g) + O2(g) → 2NO2(g), therefore, you need _____ moles of O2 for complete reaction and produce _____ moles of NO2The catalytic decomposition of hydrogen peroxide can be expressed as: H2O2(aq) → H2O(l) + O2(g) What are the stoichiometric coefficients for the reaction above? (enter the coefficients without commas or spaces in between, e.g. 557) Calculate the number of moles of oxygen gas produced from the completely catalyzed decomposition of 6.00 mL sample of a 3.5% solution of H2O2. The density of the 3.5% solution of H2O2 is 1.01 g/mL. A trial of this decomposition experiment, using different quantities of reactants than those listed in the question above produced the following data: Volume of O2 produced at room conditions 280 mL Barometric pressure 740 torr Temperature of water 24°C Termperature of O2 25°C Vapor Pressure due to water at 25°C 22.4 torr For the conditions listed above, calculate the volume of O2(g) produced at standard conditions of temperature and pressure. (enter your answer in liters)In the common process for the manufacture of nitric acid, sodium nitrate is treated with aq. sulphuric acid containing 95% H2SO4. In order that the resulting "niter cake" may be fluid; it is desirable to use sufficient acid so that there will be 34% H2SO4 by wt in the final cake. This excess H2SO4 will actually be in combination with the Na2SO4 in the cake, forming NaHSO4, although for purposes of computation it may be assumed to be free acid. The cake will contain 1.5% water and the reaction will go to completion, but 2% of the HNO3 formed will remain in the cake. Assume that the NaNO3 used is dry and pure. Calculate per 100 kg of NaNO3 charged: (a) wt and % composition of the niter cake (b) wt of aqueous acid to be used (c) wt of water vapor and nitric acid distilled from the niter cake.
- John and Eli do a reaction with the goal to prove the law os conservation of mass. In the reaction, they place 50.00 g of acetic acid (CH3COOH) in a clean, dry ziploc bag and then add 5.00 g of baking soda (NaHCO3). The products of the reaction include sodium acetate, carbon dioxide, and water. In trial 1, Eli immediately seals the bag upon addition of the baking soda and waits until the bubbling comes to a halt. John weighs the closed bag with all contents and records mass in the table. For trial 2, John and Eli repeat the procedure but forgot to seal the bag. Their results are shown in the table below. 1. Calculate the theoretical mass of the open bag. 2. Are atoms/mass conserved in each of the reactions? 3. Provide mathematical evidence to explain your reasoning that atoms/mass are/are not conserved.Please view the video* below and answer the following questions.https://www.youtube.com/watch?v=1ocQhkHw_MM1. Two reactions were demonstrated in the video above. Write the balanced equations for both reactions below.a.b.2. What catalyst was used in the decomposition of hydrogen peroxide?3. Which safety rule is broken during the demonstrations shown in this video?4. View the video and complete the table below.https://www.youtube.com/watch?v=_G7sNq7R29w Observations Balanced Reaction Equation 5. View the video and complete the table below.https://www.youtube.com/watch?v=yLsjsy_Dqd0 Observations Balanced Reaction EquationToluene, C7H8 , is burned with 30% excess air. A bad burner causes 15% of the carbon to form soot (pure C) deposited on the walls of the furnace. What is the Orsat analysis of the gases leaving the furnace