Q: How many moles of NaHCO3 are there in 98 g of NAHCO3(SHOW WORK)
A: Given Mass of NaHCO3 = 98 gMolar Mass of NaHCO3=Molar mass of Na + Molarv Mass of H + Molar Mass of…
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A: Percent yield is the ratio of actual yield to the theoritical yield
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A: The electronic Configuration of Aluminum is 1s2 2s2 2p6 3s2 3p1.
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Q: athandler&extension_handler=extension_open_button&file=httpss dent Upgrade 0 9O Moodle…
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Q: How many grams of CaF2 would be needed to produce 1.18 moles of F2? CaF2(s) + H2SO4(L) ---->…
A: Stoichiometry is mainly based on the calculation of moles and volumes. These two values are used to…
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A: Following are the no. Of moles of 1st product as follows.
Q: D
A: Given :- 3H2SO4(aq) + 2Fe(s) -----> Fe2(SO4)3(aq) + 3H2(g) number of moles of H2SO4 = 0.500…
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Q: What I Have Learned (PORTFOLIO OUTPUT #19) Directions: Balance the chemical equation below and…
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Q: can you solve these 2 and just provide the answer I solved most of the work I just wanna make sure…
A: Hey, since there are multiple questions posted, we will answer first question. If you want any…
Q: Balance 1. the eq uaticn C7 Hu02 C3 Hio N2 C7 HIa N02 C17 Hia N202 2. wnat would the pruuuct be…
A: Hi! Thank you for the question, As per the honor code, we are allowed to answer one question at a…
Q: HELP me please
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Q: Average No. of moles of KMNO4 - No. of moles of H20 = 1.07 x 10 mol %3D = 2.675 x 10mol =D0.0535 M…
A: Question given, Concentration of H2O2 = 0.0535 (M), we have molecular weight of H2O2 = 34 gmol-1…
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Q: How many moles of H2 can be produced from z grams of Mg in magnesium-aluminum alloy? The molar mass…
A: Given: Alloy of magnesium and aluminium. Mass of magnesium = x And mass of aluminium = y
Q: Reaction: Cu(H2O)4]SO4•H2O(aq)+ 4 NH3(aq)®[Cu(NH3)4]SO4•H2O + +4 H2O(l) Mass of copper(II) sulfate…
A: The reaction taking place is given as, => [Cu(H2O)4]SO4•H2O (aq) + 4 NH3 (aq) ------->…
Q: sider the following reaction: Mg + F2 MgF2 eaction starts with 31.58 g of Mg and 51.54 g of F2? g…
A: Limiting reagent is mg
Q: Please answer part D PART A) What is the maximum number of moles of P2O5P2O5 that can…
A: The reaction for the formation of P2O5 from phosphorous and oxygen is shown as follows, It is given…
Q: :. 2 in Au ● Na₂ Coz + 2 Call₂ -> ? Cal 03 (s) + ? mass 0.0008 g mass of of Сасоз 2.1547 Volume of…
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Q: VISUALIZATION Determining an Empirical Formula Carbon-Hydrogen Analysis Unit Furnace HOabsorber Co,…
A: Concept is based on empirical formula and combustion.
Q: Give the percent yield when 28.16 g of CO2 are formed from the reaction of 4.000moles of C8H18?
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Q: DATA: weight of the crucible + lid (werucible-lid) =30.4265 weight of the crucible + lid + magnesium…
A: Given that: Weight of crucible and lid (W1) = 30.4265 g…
Q: No. of moles of Na2Co3 required to produce 100gof NaNO3 Na2Co3+2HNO3->2NaNO3+CO2+H2O 1.…
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Q: Current Attempt in Progress What is the coefficient of H2O when the following equation is properly…
A: Balanced equation is the equation in which equal number of atoms of every element is present on both…
Q: theoretical yield
A: Number of moles = mass/molar mass Mass /theoritical yield = moles x molar mass
Q: Active Dosage Form Raw Materials Actual Yield Formulation Packaging Ingredient Calcium carbonate…
A: Preparation of calcium carbonate from calcium oxide, carbon dioxide and water.
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Q: CeGive Up? Resources ! Hint Check Answer For the reaction Na,CO, + Ca(NO,), → CaCO, + 2 NaNO, how…
A: Given, Mass of sodium carbonate = 45.3g. Moles of sodium carbonate can be calculated as follows:
Q: Close Problem Calculate percent yield. Consider the reaction of AgNO, with Cu to form Cu(NO3)2 and…
A: The reaction for the process is given below. 2AgNO3 + Cu → Cu(NO3)2 + 2AgFrom the above…
Q: can you solve these 2 and just provide the answer I solved most of the work I just wanna make sure…
A: Hey, since there are multiple questions posted, we will answer first question. If you want any…
Q: what is the percent asubstance if yield of the profected amount is 130.87 grams but only 106:2 g of…
A: Percentage yeild =( actual yeild ÷ theoretical yeild)x100
Q: Which one or more of the following equations is (are) balanced? (Select all that apply.) O C7H16 +…
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Q: Current Attempt in Progress How many moles of H2 and N2 can be formed by the decomposition of 0.227…
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Q: 4N92 Crz 07+ 3C 6HIO +16H2 304 4N92 SO4 + 4Cr2(s04)3 13C6HIO Oy t16 Hz6 28,2009 of C6HIO are reacted…
A: percent yield of reaction = 43.90%
Q: Current Attempt in Progress A sample of NaSO4 weighing 7.10 grams contains i moles. eTextbook and…
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Q: 1
A: In the given equation, one mole of Fe is present at reactant side whereas one mole of Cu is present…
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Q: Raw Materials: 500 g calcium polysulphide and 1.5 kg hydrochloric acid Actual Yield: 343.4g…
A: Given data,Mass of CaS5=500gMass of HCl=1.5Kg=1500gActual yield of S=343.4g
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A: Molar mass of H2O is 18 g/mol
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A: Limiting reagent is that which consumed first or present in less amount.
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A: According to balanced chemical reaction equation:- a.) mass of aniline=93.13g b.) No. Of mole of…
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- Souring of wine occurs when ethanol is converted to acetic acid by oxygen: C2H5OH(l) +O2(g)--->CH3COOH(g)+H2O(l). A 1.00 L bottle of wine labeled as 7.00% (%v/v) ethanol, is found to have a defective seal. Analysis of 1.00 mL showed that there were 0.0274 g acetic acid in that 1.00 mL. The density of ethanol is 0.816 g/mL. (a) What mass of oxygen must leaked into the bottle in pounds(lb) (b) What is the percent yield for the conversion of ethanol to acetic acid, if oxygen is in excessTo determine the mass of Fe2O3 from the given mass of K3Fe(CN)6, the gravimetric factor to be used is a. Fe2O3 / K3Fe(CN)6 b. Fe2O3 / 2K3Fe(CN)6 c. 2Fe2O3 / K3Fe(CN)6 d. 3Fe2O3 / 2K3Fe(CN)61.Methane was combusted at 100.0 degrees C and 1.00 atm. The following data table was used to collect and record data: Item Mass Before (g) Mass After (g) Volume (L) Methane 774 x x Oxygen XS x x Carbon dioxide x ? ? Water Vapor x ? ? CH4 + O2 ---> How many grams of water vapor is formed as a result of the reaction? How many liters of carbon dioxide is formed? ________g H2O _________L CO2 Blank 1: Blank 2:
- Would you help me whit this example (6) Thank you.A mixture of Al2O3(s) and CuO(s) weighing 18.371 mg was heated under H2(g) at 1 0008C to give 17.462 mg of Al2O3(s) 1 Cu(s). The other product is H2O(g). Find wt% Al2O3 in the original mixture.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 0.157g of a compound containing C, H, N and possibly O, yields 0.213g CO2 and 0.0310g H2O upon combustion. Another sample of the same compound weighing 0.103g yields 0.023g NH3 in a nitrogen analysis. Calculate the empirical and molecular formulae given the MW= 450 +20 (Answer: C7H5O6N3; C14H10O12N6)Show work using conversion factors Answer key: #37d 1.250 moles CO2 #37e 4.92 mole HCl #37f 7.1422 moles HCl ( fixed 10/14/2020) #37g 143 g CO2What is the concentration of a 62.0 % (w/w) concentrated nitric acid (HNO3, Mr = 63.0 g/mol) solution (density: 1.32 g/cm3) in mol/dm3 (molarity) and g/dm3 (mass concentraion) units? How many cm3 do you need to dilute into 200.0 cm3 from that concentrated nitric acid if you would like to have a solution with a concentration of 3.0 mol/dm3 ?
- Methane was combusted at 100.0 degrees C and 1.00 atm. The following data table was used to collect and record data: Item Mass Before (g) Mass After (g) Volume (L) Methane 774 x x Oxygen XS x x Carbon dioxide x ? ? Water Vapor x ? ? CH4 + O2 ---> How many grams of water vapor is formed as a result of the reaction? How many liters of carbon dioxide is formed? _________ g H2O __________ L CO2 Blank 1: Blank 2:Mass of original mixture: 0.280g Mass of naphthalene recovered: 0.160 g Mass of 3-nitroaniline recovered: 0.015 g Mass of benzoic acid recovered: 0.135 g 1. a) calculate % by mass of naphthalene, 3-nitroaniline and benzoic acid in original sample 1. b) calculate total mass of three recovered components (g) 1. c) calculate total percent recovery (%)"Nitric acid reacts with S to give H2SO4 and nitrogen monoxide. 30 ml of acid at 25% by mass and a density of 1.08 g/ml with 5 g of S. a) Adjust the reaction. b) Calculate limiting reactant and its excess. c) Calculate mass of unreacted reactant. d) Determine volume of NO at 600 mm Hg and 20°C. 20% yield"THE EQUATION THEY PROVIDE IS:2HNO3 + S → H2SO4 +2NOYOU DONT NEED TO ADD H20 IN THE EQUATION
