05.09 Module Five Review and DBA 05.01 Four Phases of Matter * Matter exists in different phases‚ also called states‚ which include solid‚liquid‚ gas‚ and plasma. These phases can be distinguished at the molecular level by how the particles are held together. * Solids * In the solid phase‚ the intermolecular attraction between particles of matter is strong enough to hold all the particles together in a fixed three-dimensional arrangement. Because of the rigid arrangement of particles
Free Gas Temperature Ideal gas law
reacted‚ The concentration of sodium thiosulphate. Then we can know the mass of vitamin C = No. of moles of vitamin C × Molar mass of vitamin C = No. of moles of I2 reacted with vitamin C ×10 × Molar mass of vitamin C = ( No. of moles of I2 produced - No. of moles of I2 reacted with Na2S2O3 ) ×10 × Molar mass of vitamin C = ( No. of moles of KIO3 used ×3 - No. of moles Na2S2O3 ÷2) ×10 × Molar mass of vitamin C Results: Part A: Standardization of sodium thiosulphate solution
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0.87 % Using mole ratio‚ HCl : NaOH 1 : 1 Number of moles of HCl in 25.00 〖cm〗^3 of solution = 0.00575 mol % ∆ of moles = 0.87 % Number of moles of excess HCl in 250.0 〖cm〗^3 volumetric flask 0.00575 × 250.0/25.00=0.0575 mols % ∆ of pipette 0.03/(25.00 ) × 100 % = 0.12 % % ∆ of volumetric flask 0.3/250.0 × 100 %= 0.12 % % ∆ of moles of HCl 0.12% + 0.12% + 0.87% = 1.11% Initial mole of HCl added to eggshell 2.00 × 50/1000 = 0.100 mols % ∆ of moles of HCl 0.50/50
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Cup o’ Noodles: Through the Eyes of a Chemist Background: Before completing this experiment‚ one must know about chemical formulas‚ ionic bonding‚ solutions and moles to understand the results of this experiment. A chemical formula is the symbol for compounds and elements. It tells chemists how many atoms are in a chemical compound‚ formula unit or molecular compound. In a chemical formula a subscript indicates how many atoms there are of an element before it. The coefficient in a chemical formula
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all percentages to a mass in grams‚ eg‚ 21% = 21g‚ 9% = 9g c. Find the relative atomic mass (r.a.m) of each element present using the Periodic Table d. Calculate the moles of each element present: n = mass ÷ r.a.m e. Divide the moles of each element by the smallest of these to get a mole ratio f. If the numbers in the mole ratio are all
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Unit 3 – Virtual Labs Letizia Schianodicola Lab #1 – Atomic Weight of Magnesium 1. Moles of hydrogen evolved‚ from chemical property dialog for beaker: a. 0.000411 mol H2 2. Calculate the atomic weight of Magnesium. Atomic weight of Mg = weight of Magnesium/moles of H2. b. 59‚136.253 g/mol Mg (24.305 - weight of Mg / 0.000411 mol H2) 3. Calculate the # of molecules of H2 that were produced in the reaction – use Avagadro’s number –
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salt over icy roads in winter in the North? Explain. This actually is interesting and since I lived up North I know that the truck don’t actually melt the ice but rather bring the temp of the ice melting point. 7. Will 1 L of 1 M NaCl contain mole chloride ions than 0.5 L of 1 M MgCl2? Explain. Support your answer by calculations. They will contain the same number of chloride ions. .5L( 1 mol MgCl2/L) ( 2 mol Cl-/1 mol MgCl2) = 1 mol Cl- 8. Describe step by step how you would
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Exercise 1 Binary Solid-Liquid Diagram CHEM 112.1 – 2L Group 2 I. Data and Results Table 1.1 Break and arrest temperature of diphenylamine-naphthalene mixture. Table 1.1. Mole fraction of naphthalene‚ χB‚ and corresponding arrest and break temperature at each run. Run number | Mole Fraction‚XB | Ave. break temperature‚ ˚C | Ave. arrest temperature‚ ˚C | 1 | 1 | 72 | 35.4375 | 2 | 0.868388 | 72 | 35.4375 | 3 | 0.725218 | 62 | 35.4375 | 4 | 0.568895 | 49 | 35.4375 |
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partial pressures: |[pic] |[pic] |[pic] | The partial pressures in the bottom row were found by multiplying the mole fraction of each gas by the total pressure: Pi = XiPt. The term in the denominator of each mole fraction is the total number of moles of gas present at equilibrium: (0.200 – x) + (3.00 + x) + x = 3.20 + x. Substituting the equilibrium partial pressures into the equilibrium expression‚ we have [pic] whose polynomial
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2012 INRODUCTION In the method of continuous variations the total number of moles of reactants is kept constant for the series of measurements. Each measurement is made with a different mole ratio of reactants. A mole ratio is ratio between the amounts in moles of any two compounds involved in a chemical reaction. Mole ratios are used as conversion factors between products and reactants in many chemistry problems. The optimum ratio‚ which is the
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