of lithium plus the watch glass *37.41 g of Watch glass *122 cm3 of hydrogen gas collected Calculations from method 1 Moles of hydrogen produced: Assuming that 1 mole of gas occupies 24000 cm3 at pressure and room temperature! I will now calculate the number of moles of the hydrogen gas produced. I will do that by dividing the volume of gas produced by 24000cm3 : Moles (n) = Volume (cm") 24000 cm" So: n = 122 cm" = 0.005083 mol of H2 24000 cm" Equation: 2 Li(s) + 2 H2O (L)2LiOH(Ag) +
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11 g Questions 1. Calculate the value of “n”. Show your work. Include an example of ALL calculations involving solving for “n”. 3.02 g of hydrated copper sulfate is heated to drive off water. The dry sample has a mass of 2.11 g. What is the mole ratio between copper (II) sulfate‚ CuSO4‚ and water‚ H2O? Mass of Hydrate 3.02 g Mass of Dry Sample - 2.11g Mass of Water 0.91 g MM CuSO4= 63.55 + 32.07 + 4(16.00)= 159.62 g/mol 2.11 g CuSO4 (1 mol CuSO4
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Test 2 Name___________________________________ MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Find the combination that will give a gas as a product A. AgNO3(aq) + NaI(aq) B. HCl(aq) + Na2CO3 (aq) C. MgCl2(aq) + K2CO 3 (aq) D. CaSO4 (aq) + (NH4)3 PO4(aq) 1) A) A B) C C) B D) D 2) 2) The balanced molecular equation for complete neutralization of H2 SO4 by KOH in aqueous solution is __________. A) 2H+ (aq) + 2OH- (aq)
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Solution Moles from mass weighed Moles = Mass Mr = 2.42 97.1 = 0.0249mol Molarity of solution Concentration = Moles Volume = 0.0249 (250 ÷ 1000) = 0.0996dm3 Titration Moles of NH2SO3H Moles = Volume x Concentration = 12.90 x 0.0996 1000 = 1.28484 X10-3 moles From equation 1 mole NH2SO3H = 1 mole KOH Molarity of KOH Concentration = Moles
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{ 1 } = 0.41g 6. Mass of chlorine in Magnesium Chloride: { 5 } – { 3 } = 0.32g 7. Moles of Magnesium: 0.09g x 1mol = 0.004mol 24.31g 8. Moles of Chlorine: 0.32g x 1mol = 0.009mol 35.45g 9. Moles of Magnesium divided by the smaller number of moles: Mg = 0.004g =1
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ratio Urea to C.Acid 97.7-125.5 C 98.9-118.8 Calculations Molar mass of urea (CO(NH2)2) = 60.05526 g/mol and 1g of urea was used so converting it to moles take 1g / 60.05526g/mol = 0.0166513 moles of urea. Molar mass of cinnimic acid (C9H8O2) is 148.16g/mol and 1g was used so converting it to moles take 1g/ 148.16g/mol = 0.00674946 moles of cinnimic acid. Procedure A. Calibrate Thermometer a. Use Table 3.2 of known melting point temperatures for a series of standard substances. b. Note
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Chemistry Laboratory 6A – Stoichiometric Analysis of an Iron-Copper Single Replacement Reaction Martin Sun Purpose The purposes of this experiment were to: determine the number of moles of iron reacted; determine the number of moles of copper produced; and calculate the ratio of moles of copper to moles of iron. Materials and Methods Materials and methods for this laboratory followed those laid out in Experiment 6A on pages 56-59 of Essential Experiments for Chemistry by Morrison and Scodellaro
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CHAPTER 5 GASES AND THE KINETICMOLECULAR THEORY 5.1 Plan: Review the behavior of the gas phase vs. the liquid phase. Solution: a) The volume of the liquid remains constant‚ but the volume of the gas increases to the volume of the larger container. b) The volume of the container holding the gas sample increases when heated‚ but the volume of the container holding the liquid sample remains essentially constant when heated. c) The volume of the liquid remains essentially constant‚ but the volume of
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Abstract Molar volume is the volume that one mole of gas occupies when temperature and pressure are kept constant. The molar volume of a gas can be determined through evaluating how much gas is given off when the number of moles of the substance is known. To find the volume of gas that will be used to calculate the molar volume‚ the process of water displacement can be used. Reference Citation Cesa‚ J. (2002). ChemTopic labs: Experiments and demonstrations in chemistry (vol. 9). Batavia
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For example‚ a manufacturer might want to know‚ How much ammonia will I produce from 20 tonnes of nitrogen in the Haber Process? To do these calculations you will need to be familiar with the term Ar (relative atomic mass)‚ Mr‚ Molar mass and Mole. Relative Atomic Mass – Ar • The Ar tells us the average mass of an individual atom (average because of isotopes). • The Ar for an atom has no units as it is relative • You will always be given the Ar for an atom in any example set. Relative
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