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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supposedly a scientific study of the phenomena of young children remembering their most recent past lives. Adrian made a note to try to find this book‚ but before he left the A.R.E.‚ he purchased copies of Many Mansions and Many Mansions ll. He would spend the weekend reading these books before becoming further involved with Becky Williams and the Society for Paranormal Analysis. On his way home Adrian reconsidered his own beliefs.
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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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Laboratory Report 1 Title : Accurate Measurement of Mass and Volume Part A: The Formula of Hydrated Copper (II) Sulfate Aim: The objective of this experiment is to find out the accurate mass of a solid and to calculate the moles of an unknown. Materials: The materials used in this experiment are Hydrated Copper (II) Sulfate‚ weighing bottle‚ analytical balance‚ laboratory balance‚ casserole‚ spatula‚ and hotplate. Methods: First‚ approximate 1.0g of hydrated copper (II) sulfate was
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slapped‚ as if freezing water had been poured all over her. She even shivered as she remembered‚ of course she knew‚ husband-this was her husband‚ Adrian. They had been married for two years. Relief washed through her as she suddenly remembered everything. She sighed with relief and smiled at Adrian‚ who smiled back‚ still looking worried. "I’m fine Adrian‚ I just had a nightmare and woke up not knowing who I was." She said simply‚ laughing at how scared she had been‚ how on earth could she have forgotten
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each part were conducted and a temperature vs. time graph was plotted for each trial. From the experiment‚ the neutralization reactions involving strong and weak electrolytes for Part A produced q=-51.359kJ of heat per mole of H+ and Part B produced q= -52.097 kJ of heat per mole of H+. Theses
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