2. Nipa vinegar or sukang puti is produced by the fermentation of nipa sap by veasts andacetic acid bacteria. Based on the overall reaction given below, complete the followingtable, assuming complete reaction takes place.C,H120, + 20,2C,H,0, + 2C0, + 2H,0C,H1203.60 g0.125 mol5.25 x 10 23 moleculesC,H,O2molCO2H,0molbymolmoleculesmoleculesby

The balanced reaction taking place is given as, => C6H12O6 + 2 O2 →2 C2H4O2 + 2 CO2 + 2 H2O And…

Answered: 2. Nipa vinegar or sukang puti is…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Use the References to access important values if needed for this question. An element X has a tribromide with the empirical formula XBr3 and a trichloride with the empirical formula XCl3. The tribromide is converted to the trichloride according to the equation XBr3+ Cl₂ → XCl3 + Br₂ If the complete conversion of 1.329 g of XBr3 results in the formation of 0.719 g of XCl3, what is the atomic mass of the element X? Atomic mass X = g/mol
Metallic aluminum reacts with MnO2 at elevated temperatures to form manganese metal and aluminum oxide. A mixture of the two reactants is 67.2% mole percent Al. Find the theoretical yield (in grams) of manganese from the reaction of 300 g of this mixture. Express your answer using two significant figures.
Question 105 of 109 Submit Methanol can be formed by the following UNBALANCED equation below. What is the mass in grams of methanol that can be formed from 105 molecules of CO? H2(g) + CO(g) → CH;OH(1). 1 6. C 7 8. +/- x 10 0 Tap here or pull up for additional resources 3. LO
Imagine you mix 16.05 g of methane (CH4) gas and 96.00 g of oxygen (O2) gas and then ignite the mixture. After a bright flash and a loud bang, some water droplets form on the inside of the reaction vessel. how many moles of water
Mass NaHCO3 = 6.9341 g 5. Calculate the moles of NaHCO3 in the sample and record the data below. 0.0825 mol 6. Drag the 25 mL empty graduated cylinder under the sink tap and hold it there till it fills with water. (When the graduated cylinder is full, it will automatically snap back into place.) Pour that water into the beaker with the NaHCO3. Then pour the beaker with the solution into the 50 mL graduated cylinder (the largest one). Hold the 50 mL cylinder under the tap until it fills with water to make an aqueous solution of NaHCO3. Note that the solid is added and dissolved before the volume is measured when making a molar solution. Chemists normally use a volumetric flask for making molar solutions, but this is not available in the simulation. Record the volume of the solution, in L, below. Volume NaHCO3 = 0.05 7. The molarity is calculated using the formula: L Calculate the molarity of the NaHCO3 solution in units of mol/L. M 8. If the density of the solution is 1.047 g/mL,…
Aspirin (C9H8O4) is synthesized by reacting salicyclic acid (C7H6O3) with acetic anhydride (C4H6O3). The chemical equation is:C7H6O3 + C4H6O3  C9H8O4 + HC2H3O2a. If we react 100. g of acetic anhydride with 100. g of salicyclic acid, what mass of aspirin do we expect to produce? (theoretical yield)b. If the percent yield comes out to 84%, what mass of aspirin did the reaction actually produce? (what is the actual yield?)
Epsom salts, a strong laxative used in veterinary medicine, is a hydrate, which means that a certain number of water molecules are included in the solid structure. The formula for Epsom salts can be written as MgSO4⋅xH2OMgSO4⋅xH2O, where xx indicates the number of moles of H2OH2O per mole of MgSO4MgSO4. When 7.592 gg of this hydrate is heated to 250 ∘C∘C, all the water of hydration is lost, leaving 3.708 gg of MgSO4MgSO4. What is the value of x?
22.0 g of CO2 gas and 9.01 g of H2O gas are formed from combustion of an unknown hydrocarbon (containing only hydrogen and carbon) in the presence of O2 gas. The molar mass of the gas is 84.2 g/mol. What is its molecular formula?
61. Consider the reaction between calcium oxide and carbon dioxide: CaO(s) + CO2(g) →→ CaCO3(s) A chemist allows 14.4 g of CaO and 13.8 g of CO₂ to react. When the reaction is finished, the chemist collects 19.4 g of CaCO3. Determine the limiting reactant, theoretical yield, and percent yield for the reaction.
given the chemical equation Zn+2HCl->ZnCl2+H2 how many molecules of H2 will be produced if 19 Atoms of ZN are consumed in the reaction
A sample of 48.7 g of tetraphosphorous decoxide (P₂O₁0) reacts with 84.6 g of water to produce phosphoric acid (H₂PO4) according to the following balanced equation. PAO10 + 6H₂O4 H₂PO4 Determine the limiting reactant for the reaction. OH₂O O H₂PO4 OP40 10 Calculate the mass of H₂PO4 produced in the reaction. mass of H₂PO4:
When ammonia is mixed with hydrogen chloride (HCl), the white solid ammonium chloride (NH4Cl) is produced. Suppose 10.0 g ammonia is mixed with the same mass of hydrogen chloride. What substances will be present after the reaction has gone to completion, and what will theirmasses be?

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