masses and volumes as Trial 1. Calculations: 1. Determining the volume of 6 M CH3COOH (acetic acid) required to completely react with the mass of NaHCO3 NaHCO3 (s) + CH3COOH (aq) CO2 (g) + CH3COONa (aq) + H2O (l) Given 0.8023 g of NaHCO3 (Trial 1) Mole ratio 1 mol of NaHCO3 : 1 mol of CH3COOH Molar
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the formula molality = moles solute/kg solvent to find the number of moles in 10% antifreeze solution. 3. Using the formula molar mass = grams/moles calculate the molecular mass of antifreeze in the 10% solution. 4. Using the equation ΔT = Kf m¸calculate the molality of the 20% antifreeze solution. 5. Use the formula molality = moles solute/kg solvent to find the number of moles in 20% antifreeze solution. 6. Using the formula molar mass = grams/moles calculate the molecular
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atm/k mol. Finding the molar volume at STP was done by multiplying the number of moles of the gas by the value of the gas constant found in the experiment. Introduction: The purpose of this experiment is to discover how the molar volume of a gas and the gas constant is found. The molar volume can be found by the equation: MV = V/n = RT/P where it is either dependent on a given volume (V) and a number (n) of moles or a constant temperature (T)‚ pressure (P) and the gas constant. In Avogadro’s
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Chapter 4 Fundamentals of Material Balances Material Balance-Part 1 Process Classification 3 type of chemical processes: 1. Batch process – Feed is charge to the process and product is removed when the process is completed – No mass is fed or removed from the process during the operation – Used for small scale production – Operate in unsteady state March 31‚ 2009 ChE 201/shoukat@buet.ac.bd 2 Process Classification 2. Continuous process – Input and output is continuously
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The Equilibrium Constant of an Ester Hydrolysis Reaction CHM 152LL Section 33263 March 28‚ 2014 John Weide Abstract: The purpose if this experiment is to determine the equilibrium constant of an unknown alcohol. In this experiment unknown alcohol number three and unknown ester number three were used. The equilibrium constant was found by titrating a series of reactions containing H2O‚ HCl‚ and the unknown ester with only the last solution containing the unknown alcohol
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the Job’s method-the method of continuous variation-for determine the reaction stoichiometry. In the method of continuous variations‚ the total number of moles of reactants is kept constant for a series of measurements. Each measurement is made with a different mole ratio or mole fraction of reactants. The maximum change will occur when the mole ratio of the reactants is closest to the optimum ratio which is the stoichiometric ratio in the chemical equation. A job plot itself is used to determine
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Calculate the number of atoms in 10.0 grams of Fe. 2. Give the mass number‚ #protons‚ #neutrons and #electrons for the isotope strontium-88. 3. Calculate the number of moles of carbon in 50.0 g of benzene C6H6 4. A substance is found to be 38.7 % C‚ 9.7 % H and 51.6 % O by mass. Its molar mass is 62.1 g/mole. What is its molecular formula? 5. Name the following: a) Ca(OH)2 b) KCN c) HClO4(aq) d) FeSO4 e) Na2O f) SF6 g) MgSO4 ( 2H2O h) Na2O2 6. What are the
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Conductimetric Titration and Gravimetric Determination of a Precipitate Objective: * Measure the conductivity of the reaction between sulfuric acid and barium hydroxide * use conductivity values to determine equivalence point * measure mass of a product to determine equivalence point gravimetrically * calculate molar concentration of barium hydroxide solution Procedure: * First‚ combine 10.0 mL of the Ba(OH)2 solution with 50 mL of distilled water. Then‚ measure out 60 mL
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LEARNING TASK NO. 4B Composition Stoichiometry Problems Mole Relationship from Chemical Formulas: a) Determine the number of moles of chloride ions in 2.53 mol ZnCl2. b) Calculate the number of moles of each element in 1.25 mol glucose (C6H12O6). c) How many molecules of oxygen atoms are present in 5.00 mol diphosphorus pentoxide? d) Calculate the number of moles of hydrogen atoms in 11.5 mol water. e) A sample of ethanol (C2H5OH) has a mass of 45.6 g.How many carbon atoms does the sample
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x17.99916] 100 m(O) 15.99938 1 m( H ) x[99.985 x1.007825 0.015 x 2.0141] 100 m( H ) 1.007975 m( H 2O) 18.01533 m(O) (a) # of moles of water= (b) # of 1H atoms=2.76 moles x 0.6022e24 x 2 atoms of H x 0.99985 abund. =3.32e24 atoms of 1H (c) # of 2 H atoms=2.76 moles x 0.6022e24 x 2 atoms of H x 0.015e-2 abund. =4.98e20 atoms of 2 H 50 =2.76 moles 18.01533 2.16 The fission of the nucleus of 235 U releases approximately 200MeV. How much energy (in kilowatt235 hours and megawatt-days)
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