NaOH(aq) Equation: C6H4COOH.COOK + NAOH → C6H4COOK.COONa Ratio of Reactants: 1 : 1 1 mole of Potassium Hydrogen Phthalate (C6H4COOH.COOK) reacts with 1 mole of Sodium Hydroxide (NAOH). Concentration of NaOH = Weight of Potassium Hydrogen Phthalate Volume of NaOH (dm3) × Molar Mass of Potassium
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this experiment is to determine the atomic mass of each metal and the percent composition of a known mass aluminum-zinc alloy by determining the moles of H2 gas formed. Zn(s) + 2HCl(aq) → ZnCl2(aq) + H2(g) 1 mole of H2(g) is produced for every 1 mole of Zn(s) 2. 2Al(s) + 6HCl(aq) → 2AlCl3(aq) + 3H2(g) 3 moles of H2(g) is produced for every 2 moles of Al(s) Both the aluminum and the zinc contained in the alloy react to produce hydrogen gas. The reaction occurs in a test tube and generates
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Name:_________________________ MASS AND MOLE RELATIONSHIPS IN A CHEMICAL REACTION PRE-LAB QUESTIONS 1. Balance the equation for the reaction of barium chloride with silver nitrate. 2. Predict the mole ratio of BaCl2 to AgCl for the equation. 3. If an experiment with 10.2 g barium chloride produced 14.5 g silver chloride‚ calculate the experimental mole ratio of silver chloride to barium chloride. Name:_______________________
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the amount of moles of each. To find the amount of moles we must solve for them: Zinc = (2.4375g / 1) X (1 / 65.38g) = 3.73 X 10-2 moles Copper = (0.0625g / 1) X (1 / 63.546g) = 9.835 X 10-4 moles The balanced equation for zinc and HCl is Zn + 2HCl = 1H2 + 1 ZnCl2 H=1‚ Zn = 65.38‚ Cl=35.45 Molar Mass of HCl = 101.83 (3.73 X 10-2 moles Zn) (2HCl/1Zn) = 7.46 X 10-2 moles HCl The amount of HCl that should be used is: 50mL of HCl = .05 L of HCl 7.46 X 10-2 moles of HCl X 2 = .1492 moles of HCl used
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the needed amount of Na2CO3 Convert 1.0g of CaCl2-.2H2O to moles of CaCl2-.2H2O 1.0g x 1 mole CaCl2-.2H2O 147.0 g CaCl2-.2H2O = 0.00680 moles CaCl2-.2H2O The mole ratio is 1:1 Hence if we have 0.00680 moles of CaCl2-.2H2O we will as well need 0.00680 moles of Na-2CO3 Convert moles of Na-2CO3 to grams of Na2CO3 = 0.00680 moles Na-2CO3 x 105.99g Na-2CO3 1 mole Na-2CO3 = 0.72g This means that we need 0.72g of Na-2CO3
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chloride solution. Then‚ stoichiometry was used to determine how much Na2CO3 was needed for a full reaction: First‚ 1 g of CaCl22H2O was converted to moles: 0.00680 moles. The mole ratios of CaCl22H2O and Na2CO3 was seen to be 1:1. Then‚ moles of Na2CO3 were converted to grams: 0 .72 g. The measure of CaCo3 was predicted to be 0.00680 moles. 0.00680 moles converted to grams is 0.68 grams. Then‚ 0 .72 grams of Na2CO3 was measured into a paper cup because that was the measure calculated for Na2CO3 using
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of new moles‚ changes in the color of existing mole‚ a painful or itchy sore on the skin‚ a shiny lump on the skin‚ a scaly spot on the skin‚ and a sore that does not heal‚ among
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Hence‚ from calibration curve of refractive index versus mole % of ethanol‚ Mole % of ethanol = 37.0% Table 01: Observed Data for Vapor Liquid Equilibrium of Ethanol Water system Observation No. | Refractive Index | | Liquid | Vapor | 01 | 1.351 | 1.362 | 02 | 1.3515 | 1.3615 | 03 | 1.351 | 1.3615 | 04 | 1.352 | 1.3615 | 05 | 1.352 | 1.3615 | Calculated Data Table 02: Calculated data for equilibrium composition (% mole) of vapor and liquid Observation No. | Refractive Index
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Student:………………… Date:………….. What is the volume of 1 mole of hydrogen gas? One mole of any gas occupies the same volume when measured under the same conditions of temperature and pressure. In this experiment you will calculate the volume of 1 mole of hydrogen at room temperature and pressure. Intended lesson outcomes By the end of this practical you should be able to: • further develop skills in manipulating apparatus and accurate measurement; • use the mole concept; • calculate the molar volume at
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ratios‚ and rarely occur in simple whole numbers. When a chemical reaction occurs‚ how do the masses of reactants and products compare? In this experiment we will be making a comparison between the masses of reactants and products and the number of moles of reactants and products. PROCEDURE Polish the zinc strip using steel wool and then determine its mass. Allow the strip to sit in lead acetate for approximately an hour and observe the changes in the zinc strip. The zinc starts to accumulate
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