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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E-85 is an alternative fuel for automobiles and light trucks that consists of 85.0% (by volume) ethanol (C2H5OH), and 15.0% gasoline. When ethanol burns completely it produces CO2 and H2O. The balanced equation for the burning of ethanol isC2H5OH+3O2-->2CO2+3H2OThe density of ethanol is 0.790 g/mL. How many moles of carbon dioxide are produced by the complete combustion of the quantity of ethanol in 8.00 gallons of E-85 fuel? _mol CO2
The theoretical yield of CCl4 is 50 g. If the actual yield from the reaction is 38 g of CCl4, what is the percent yield of CCl4? PY= (Actual/Theoretical)x 100
A chemist needs to add 3.5 moles NaClNaClto a reaction. How much NaCl should she measure out in grams (g)? Round to two decimal places if necessary. 140.21g NaCl 204.54g NaCl 58.44g NaCl 0.60g NaCl
bctions: Show your solution in the space provided. Follow the GFFSA (Given, Find, ymula, Solution, Answer) format if possible. Write your answers in the space provided. 1. Combustion of hydrocarbons like methane (CH4) produces two products, water (H2O) and carbon dioxide (CO2). Consider the chemical equation of this combustion: CHA + 2 02 - CO2 + 2 H2O, when 4 mol of CH4 reacts with 4 mol of O2, how many moles of CO2 are formed? What is the limiting reactant? 2. How many grams of lead II chloride are produced from the reaction of 16.2 g of NaCl and 62.0 g of Pb(NO3)27 What is the limiting reactant? How much excess is left over?
Consider the following chemical reaction HCl (aq) + HgNO3 (aq) à Hg2Cl2 (s) + HNO3 (aq) If 20.0 grams of HCl is mixed with 30.0 grams of HgNO3 Determine the excess reactant The amount of the solid precipitate that was recovered equals to .................. grams , if the percentage yield from this reaction was determined to be 78.4%. Write the net ionic equation for the chemical reaction Determine the type of this chemical reaction
For the reaction shown, calculate how many moles of each product form when the given amount of each reactant completely reacts. Assume that there is more than enough of the other reactant. C3H8(g)+5O2(g)→3CO2(g)+4H2O(g) 1. 0.0558 molO2, v=?molCO2 2. 0.0558 molO2, v= ?molH2O
83. The combustion of gasoline produces carbon dioxide and water. Assume gasoline to be pure octane (C8H18) and cal- culate how many kilograms of carbon dioxide are added to the atmosphere per 1.0 kg of octane burned. (Hint: Begin by writing a balanced equation for the combustion reaction.)
8.50 g of a certain Compound X, known to be made of carbon, hydrogen and perhaps oxygen, and to have a molecular molar mass of 128. g/mol, is burned completely in excess oxygen, and the mass of the products carefully measured. Use this information to find the molecular formula of X
13. Suppose 90.0 g of Iron (III) chloride reacts with 17g of water? What is the limiting reagent? How much (in grams) will the products produce and how much of the excess reactant will remain after the reaction is complete?( Write the complete balanced reaction along with it states)
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
In the picture shown, the limited reactant is ____. The excesss reactant is ____. The product of the reaction is ___.
If 52.4 g of O2 is mixed with 52.4 g of H2 and the mixture is ignited, what is the maximum mass of water that may be produced?

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