amount of reactants and products of a reaction ( that is how many moles of A react with a given mol of B). A known starting mass of magnesium and the measured collection of hydrogen gas will be used to determine the reaction stoichiometry and the valency of magnesium Introduction Stoichiometry is the study of the quantitative relationship between amounts of reactants and products of a reaction. Stoichiometry can be used to calculate the amount of a product formed when given the reactants and a percentage
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Objectives: 1. To make careful measurements of the amounts of each reactant. 2. To calculate the number of moles of each reactant. 3. To predict which reactant is in excess. 4. To use drawings to relate microscopic events‚ to write a chemical equation that represent those microscopic events. 5. To learn how to measure the volume of a liquid using a buret. Prelab Questions: 1. Calculate the number of moles in 2.65g of zinc. 2. Calculate the number of moles of hydrochloric acid
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sodium carbonate. The resulting products were solid calcium carbonate and aqueous sodium nitrate (equation 1). To calculate the theoretical yield‚ the moles of sodium carbonate and calcium nitrate were calculated to find the limiting reagent. Then the moles of the limiting reagent (calcium nitrate) were used in ratio with the precipitate ( 1:1)‚ calcium carbonate‚ to find how many moles of the solid were produced‚ then to conclude the mass of the precipitate (equation 2). The percent yield was
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3 5.4300 kJ The products and reactants in reactions 1 and 2 were manipulated. In reaction 2‚ the equation was flipped so NH4+ was a product and NH3 was a reactant used later in reaction 3. Since the second reaction was flipped‚ the sign must also change from a negative to a positive. The spectator ions were canceled out to yield only the final equations for the reactions‚ specifically reaction 3. The ΔHrxn was calculated by first determining the limiting reactant. The volume was multiplied by
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equations indicate the molar ratio of the reactants and products taking part in the reaction. There are three major categories of stoichiometry problems such as mass-mass‚ mass-volume‚ and volume-volume. Convert to desired limit Molar Ratio Convert to moles Along with the three major categories‚ after finding the quantity that you need‚ stoichiometry will let you find the limiting reactants and the excess reactants. The limiting reactant is the reactant that limits the amount of product formed
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138.6 g KClO3 X ( 1 mol / 122.55 g ) = 1.131 mol KClO3 3. Determine the limiting reagent [if necessary] (Use mole ratios to figure out.) * Not necessary to determine because there is only 1 reactant in this decomposition reaction. 4. Use ratios to find the moles of the reactant or product you need to find. Since KClO3 is the only reactant‚ it is the limiting reagent. You use the moles of KClO3 if you have to calculate how many moles of oxygen
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acid‚ CH3CHOHCOOH‚ in an excess of O2? 3. 31.5 g of Na2S2O3 was made to react with 18.6 g of Cl2 according to the balanced chemical reaction below: Na2S2O3(aq) + 4Cl2(g) + 5H2O(aq) → 2NaHSO4(aq) + 8HCl(aq) a. Which is the limiting reactant? b. What mass (in g) of the excess reactant remains after the reaction? c. What is the theoretical yield (in g) of NaHSO4? IV. FINAL BOSS! A 25.00 g sample of deep-sea sediment was collected and it was found that 12.56% of it was equivalent to the weight (in g)
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false. _______true___________ 1. The study of the quantitative relationships between the amounts of reactants used and the amounts of products formed by a chemical reaction is called stoichiometry. ________true__________ 2. Stoichiometry is based on the law of conservation of mass. _________false_________ 3. In any chemical reaction‚ the mass of the products is less than the mass of the reactants. ________true__________ 4. The coefficients in a chemical equation represent not only the number of
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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 ft2 to cm2 32.06 amu to g 25 g of carbon to moles of carbon 1.00 g of gold to number of atoms of gold 25 °F to Kelvins How many significant figures are
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the marble chips and gently stir until all the CaCO3 is dissolved 6. Weigh the beaker again and record the mass. VI. Results and Calculations 7. Find the limiting reagent 8. Find the theoretical yield by multiplying the amount of moles of the limiting reactant to the molar ration of limiting reactant : ratio and by the molecular weight of the product. 9. Find the percentage yield --> Pecentage
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