gas i) Cu(NO3)2 crystals (freshly-squeezed) 2. Define (some of these terms are found in Chapters 2 and 3): a) c) e) g) i) k) m) o) 3. b) d) f) h) j) l) n) compound physical change law of conservation of mass extensive properties accuracy stoichiometry Avogadro’s number Convert a) b) c) d) e) f) g) h) 4. element solution chemical change intensive properties precision isotopes the mole limiting reactant 5 feet 10 inches to meters 55 miles per hour to cm per second 5.0 quarts to liters 1.00
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EXPERIMENT 4 TITLE Complex Formation and Precipitation. INTRODUCTION Precipitation is the formation of a solid in a solution as the result of either a chemical reaction‚ or supersaturating a solution with a salt resulting in solid material collecting on the bottom of the beaker (Housecroft & Constable‚ 2006). When the solution has been supersaturated by a compound and no more material can be supported by the solution‚ it considered as precipitate. Commonly‚ the solid will fall out of the
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Chem Final Exam Combination Combination reactions‚ also known as synthesis reactions‚ involve the combination of two or more substances into a single new substance: A + B ---> AB Many metal oxides‚ for example‚ absorb carbon dioxide (CO2) from the air to form carbonates: CaO(s) + CO2(g) ---> CaCO3(s) Decomposition Decomposition reactions represent the reverse of the combination process in that one substance breaks down into two or more substances: AB ---> A + B Water‚ or H2O‚ for example
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1) Chemistry Review Key Terms: empirical knowledge theoretical knowledge law of conservation of mass coefficient chemical amount mole Key Concepts: Write chemical equations when given reactants and products (1.5‚ 1.6) Write balanced chemical equations (2.2‚ 2.3) Interpret balanced chemical equations in terms of chemical amount (in moles) (2.3) Convert between chemical amount and mass (2.4) Classify chemical reactions (2.5‚ 2.6) Predict the solubility of elements and ionic and
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Question 1 (Limiting Reagent) 15.00 g aluminum sulfide & 10.00 g water react until the limiting reagent is used up. [Atomic mass: H = 1.008‚ Al = 26.98‚ S = 32.07‚ O = 16.00] Here is the balanced equation for the reaction: Al2S3 + 6 H2O ( 2 Al (OH)3 + 3 H2S (i) Which of the two reactants is the limiting reagent? (ii) What is the maximum mass of H2S which can be formed from these reagents? (iii) How much excess reagent remains after the reaction is complete
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After the calcium carbonate was filtered through‚ the mass was 2.13g‚ so the calcium carbonate weighed .36g. The stoichiometry that we performed said that the predicted mass of calcium carbonate was .51g‚ so the percent yield is 71%. For trial two‚ the mass of the empty filter was 1.84g. Along with the calcium carbonate‚ the filter weighed 2.00g‚ which tells us that there
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The original solution Copper (II) chloride is blue in color‚ and when the aluminum sulfide was placed in‚ the solution began to burn and the CuCl2 began to work at the aluminum‚ turning it into a dark brown color of porous material. The reaction was exothermic‚ which is when a reaction releases heat. The way to determine this if the test tube felt hot after the heat was released‚ since it elevates
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and a negative ion (anion) are strongly attracted to one another. In this experiment‚ a precipitation reaction will be studied. Stoichiometry will then be used to investigate the amounts of reactants and products that are involved. The word stoichiometry is derived from two Greek words: stoicheion (meaning “element”) and metron (meaning “measure”). Stoichiometry is an important field of chemistry that uses calculations to determine the quantities (masses‚ volumes) of reactants and products
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IB Chemistry 2 Prompt -Design an experiment relating to or utilizing the concepts of stoichiometry. Background Information -Stoichiometry is the study of the quantitative relationships between reactants and products. You can calculate or predict the amount of reactants needed or product will be produced from a balanced equation with some known quantitative physical properties. Stoichiometry was first introduced to chemistry by Jeremias Benjamin Richter from Germany in the late 18th century
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in distilled water and then mixed them together in a single beaker. Finally we filtered this mixture and let all the water evaporate leaving behind solely the precipitate. In order to determine the amounts needed of each reactant we had to use stoichiometry. First we had to set up a balanced equation of the precipitate reaction that yielded 2.00 grams of CaCo3‚ then we looked at the ratio of moles reactant to moles product. We then substituted the ratio of the molar mass of each reactant to molar
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