2 COR) + O2(2) ----> 2 CO2 (g) (OR 2 CO) + O2g) right arrow 2 CO28) Use the following conversions: 1 mol = MW in g (2 d.p.) = 22.414 L %3D %3D What is the percent yield of CO2 if 50.00 g of CO (MW = 28.01 g CO) produces 23g of CO2(MW = 44.01 g CO2)? Theoretical yield Zn'). _(Express with unit and compound, for example 'g Percent yield (Express as '%'). %3D A Theoretical Yield Percent Yield
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- For the following table fill in the missing values and calculate the theoretical yield. A + 2B à C moles 0.00242 0.00242 ?_________ MW ?_________ 98.06 164.16 g ?_________ ?__0.00002467_______ ?_________ mL 0.20 d(g/mL) 0.80Methane is produced in the human gut during digestion. As it passes through the digestive tract, it collects at thelower end and is emitted as flatulence. About 10% of a fart is composed of methane.__CH4 + __O2 → __ CO2 + __H2Oa) The average human fart contains 0.00643g of methane gas. Ifyou were to light said fart (and you SHOULD NOT), what mass ofoxygen would combust along with it?b) People, on average, pass 0.75L of gas per day. This is about0.0536g of methane per 24 hour period (remember, only ~10% ismethane). What mass of water could be generated by one personigniting their “methane emission”? c) How many water molecules is this? (SHOW ALL WORK IN TRAIN TRACKS)The ethyl alcohol content of beers produced is reported as ABV or alcohol by volume (vol/vol) If the density of ethyl alcohol at room temperature is 0.7893 grams/mL, what is the percent of ethyl alcohol in 4.50% beer expressed as percent (wt/vol)
- The combustion of liquid ethanol (C2H5OH)(C2H5OH) produces carbon dioxide and water. After 4.63 mLmL of ethanol (density=0.789g/ml)(density=0.789g/ml) was allowed to burn in the presence of 15.50 gg of oxygen gas, 3.70 mLmL of water (density=1.00g/ml)(density=1.00g/ml) was collected. Determine the theoretical and percent yeild of h2o in the reaction.Acetaminophen, a popular drug taken as pain reliever and fever reducer, is produced together with acetic acid from the reaction of 3.05 g 4-aminophenol and 4.1 ml of acetic anhydride. Acetaminophen was extracted at 60% yield. Density of acetic anhydride at 20 C, 1.08 g/ml. Calculate the actual no. of grams of acetaminophen produced. [Determine L.R., E.R.]A chemist carries out the reaction below and obtains 3.45g of iron Fe (Fe, MW=55.845g/mol). Fill in the blanks below to determine the percent yield of the reaction when 8.30g of Fe2O3 (MW= 159.69g/mol) and 3.50g of CO (MW=28.01G/mol)were used in the reaction. Fe2O3(s) + 3CO(g) = 2Fe(s) + 3CO2(g) Note that for two of the blanks, will be the same answer. 1. What would be the mass in grams of Fe produced based on the mass of Fe2O3 used? answer: (blank) 2. What would be the mass in grams of Fe produced based on the mass of CO used? answer: (blank) 3. What is the theoretical yield of Fe in grams? answer: (blank) 4. What is the limiting reagent? Enter the formula of compound. answer: (blank) 5. What is the percent yield of this reaction? answer: (blank)
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- Soda ash (sodium carbonate) is widely used in the manufacture of glass. Prior to the environmental movement much of it was produced by the following reaction. CaCO3 + 2 NaCl → Na2CO3 + CaCl2 Unfortunately, the byproduct calcium chloride is of little use and was dumped into rivers, creating a pollution problem. As a result of the environmental movement, all of these plants closed. Assume that 125g of calcium carbonate (100.09 g/mol) and 125 g of sodium chloride (58.44 g/mol) are allowed to react. Determine how many grams of useful sodium carbonate (105.99 g/mol) will be produced. How many grams of useless calcium chloride (110.98 g/mol) will be produced? You should also determine how many grams of excess reactants are left (indicate which one is the limiting reactant)For every one molecule of NaHCO3(s) there is one molecule of CO2(g) that forms: NaHCO3(s) + CH3CO2H(aq) --> CO2(g) + H2O(l) + NaCH3CO2(aq) This means that if we know how many moles of gas we need, we need the same number of moles of sodium bicarbonate to produce it. Now, we need something to fill with gas. I'll be filling a 1-quart sealable plastic bag. 1 quart is 946 mL (0.946 L). We can use the ideal gas law to determine how much gas (in moles) is needed to fill 946 mL. Remember there are four variables for the ideal gas law. Ideal Gas Law: PV = nRT P = pressure: typically 715 mm Hg in Spokane <-- unit dictates which R to use V = volume: 1 quart bag = 0.946 L <-- must be in Liters T = room temperature: 20 °C in my lab, +273 = 293 K <-- must be Kelvin n = moles: what we are solving for I used atmospheric pressure in mm Hg, so I'll have to pick the R value with "mm Hg" in the units: R = 62.4 L × m m H g K × m o l Now, use these values to calculate how many moles of…About 200 grams of glucose was fermented with 20 grams of yeast inside a fermenting vessel for 2 weeks. Calculate the percent yield of ethyl alcohol in mL or %(v/v) if the actual yield of the fermentation set-up is at 84.50 mL alcohol. Assume the density of ethanol is at 0.789 g/mL. C6H12O6 + H2O --> 2C2H5OH + 2CO2 Molar Masses: Glucose: 180.156 g/mole; Ethanol: 46.07 g/mole Water: 18.00 g/mole Report your answers in two decimal places. Please include the unit. For example: 55.33%