reaction and the rate of the reverse reaction equal each other. At this point‚ the concentrations do not change with time. These reactions are said to be in equilibrium. Equilibrium is depended on a particular temperature‚ and the concentrations of reactants and products have to follow a rule demonstrated by the equilibrium constant Kc. The equilibrium concentrations that will be studied is the reaction between iron (III) ion and thiocyanate ion: The mixture of Fe3+ and SCN- react to form a compound
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However‚ since the boiling point of 1-bromobutane is 101°C and the boiling point of water is 100°C it would be expected that there would be a large amount of water that will distill out of the flask along with the 1-bromobutane. Other remaining reactants such as a small amount of alcohol and/or acid may also be distilled out along with the water or 1-bromobutane. Since there is such a high probability of other components in the distillate‚ separation processes will need to be carried out. Sulfuric
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team. This change occurred because the concentration of the acid and base increased. The observed temperature change in experiment 4 was 3.30 °C‚ which was half of the one that was given to the team. This change occurred because the amount of the limiting reagent in this experiment is half of the one that was given to the team. The observed change in experiment 5 was 7.05 °C‚ which was slightly higher than the one that was given to the team because a different acid was used with different
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Analysis of a Chemical Mixture Using the Ideal Gas Law The objective of this experiment was to determine the composition of the NaNO2 mixture in the net ionic reaction of NO2-(aq) + HSO3NH2(aq) → HSO4-(aq) + H2O(l) + N2(g) in unknown mixture number nine. It was known that NO2-(aq) and HSO3NH2(aq) were in a stoichiometric 1:1 molar ratio. In trial one the percent mass of NaNO2 in the unknown mixture was 59.30%. In trial two‚ the percent mass of NaNO2 was 63.47%. Lastly in trial three
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The limiting reagent it CuCl2 because it is the one that will run out first compared to the .009 moles of Na2Cl3‚ which it the excess reagent because it is a higher amount of moles compared to the .007 moles of the CuCl2. The amount of excess reagent in grams
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experiment. To do this‚ the balanced equation will be looked at and then the theoretical yield will be calculated. In order to calculate the theoretical yield‚ two equations will be used: Will be used for both reactants to determine which reactant is the limiting reagent. After the limiting reagent is used‚ then the theoretical yield will be calculated using: This will give the mass of the Acetaminophen. The actual yield will be available in the experimental data‚ and using this knowledge‚ this equation
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equilibrium‚ __________. A) all chemical reactions have ceased B) the rate constants of the forward and reverse reactions are equal C) the rates of the forward and reverse reactions are equal D) the value of the equilibrium constant is 1 E) the limiting reagent has been consumed 2) Which of the following expressions is the correct equilibrium-constant expression for the reaction below? HF (s) + H2O (l) ⇌ H3O+ (aq) + F- (aq) A) [HF][H2O] / [H3O+][F-] B) 1 /[HF] C) [H3O+][F-] /
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reaction has high synthetic utility for making unsaturated 6-membered rings (Kahn‚ 2011). The more electron-withdrawing elements there are in the reactants‚ the faster the reaction will move forward. In the case of cyclopentadiene and maleic anhydride‚ the reaction takes place quite quickly due to the many electronegative oxygen present in both reactants. Mechanism: Side Reaction: Experimental: Table of Chemicals: Cyclopentadiene Maleic Anhydride Ethyl Acetate
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valency of magnesium Objective: To study the quantitative relationship between the amount of reactant and products of a reaction. 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: In Chemistry‚ stoichiometry is the study of the quantitative relationship between amounts of reactants and products of a reaction (that is‚ how many moles of A react with a given number of moles
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The Rate of a Reaction Chemical Kinetics is the area of Chemistry that is concerned with the speed‚ rate or mechanism at which a chemical reaction occurs. Reaction Rate is the change in the concentration of a reactant or product with time (i.e. M/s). It measures how fast a reactant is consumed and how fast a product is formed. 1.2 WRITING RATE EXPRESSIONS Consider the following hypothetical reaction. A + 2B ( 3C + D Rate = - rate of consumption of A = -[pic]rate
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