The simple addition of water to FeSO4 will not lead to the formation of FeSO4•7H2O. Determination of the number of molecules of water in a hydrate. If you do not know how many molecules of water are in one molecule of hydrate and want to find this out, it can be done by measuring the masses of the hydrate and anhydrous compound formed after the heating. For example, let’s assume that we do not know how many water molecules are attached to BaCl2. Let’s call this number X.
Chemistry: Molarity and Stoichiometry Directions: Using the definition of molarity, the given balanced equations, and stoichiometry, solve the following problems. Please submit your work via the link provided. 1. Calcium hydroxide (“slaked lime”) and sulfuric acid react to produce calcium sulfate and water according to the following balanced equation: Ca(OH)2(aq) + H2SO4(aq) ⋄ CaSO4(s) + 2 H2O(l) a. How many liters of 0.2 M calcium hydroxide do you need in order to have 6.0 moles of calcium hydroxide?
Write a hypothesis on what you think will happen when mixed. 3. Combine the substances; record observations. Hydrochloric Acid and Magnesium 1. Add hydrochloric acid to a test tube.
Contents Abstract – Page 2 Summary of Results – Page 3 Focus Question – Page 5,6 What if… - Page 6 Confidence Report – Page 7,8 Abstract Summary of Results Observations of Reactions – Trials 1 , 2 & 3 | Dissolving Barium Iodide and Zinc Sulfate in deionized water | As the substances dissolve the water becomes cloudy and acquired a white tint. | Centrifuging up the solution obtained in previous reaction | The precipitate and the liquid seperated, and there was more precipitate in one of the test tubes. The precipitate was a thick white color, not transparent. | Heating the Precipitate in a boiling tube containing 2 boiling chips | The mixture began producing a large amount of bubbles, as we continued heating it only white powder remained. | Observations of Chemicals | Zinc Sulfate | Powder of a white solid | Barium Iodide | Powder of a white solid.
The change in enthalpy relies on the concentration of the salt solution, because different concentrations will produce different enthalpies. There is an equation to determine how much of this heat energy is lost or gained when a reaction is performed. Q = c m (T1-T2) Where: q is the energy in Joules C is the heat capacity, measured in joules per gram per degree Celsius M is the mass of the solution, measured in grams J is the joules G is the grams of water T is the temperature ΔH=ΔE + PΔV = (q p +w) – w = q p Procedure: 1. Follow instructions 1-9 in Appendix A-1 to initialize the MeasureNet workstation. a.
The following data were obtained when a sample of barium chloride hydrate was analyzed as described in the Procedure section. Calculate (a) the mass of the hydrate, (b) the mass of water lost during heating, and (c) the percent water in the hydrate. Mass of empty test tube 18.42 g Mass of test tube and hydrate (before heating) 20.75 g Mass of test tube and anhydrous salt (after heating) 20.41 g. Mass of the Hydrate is 2.33g. Loss (H2O) is 0.34g. Percent H2O in Hydrate is equal 0.34/2.33=14.6% 3.
Use a calorimeter to measure the temperature change in each of three reactions. Calculate the heat of reaction, ∆H, for the three reactions. Use the results to confirm Hess’s law. Ev al Figure 1 ua tio Na+(aq) + OH–(aq) + H+(aq) ) + Cl–(aq) → H2O(l) + Na+(aq) + Cl–(aq) ∆H3 = ? n (3) Solutions of aqueous sodium hydroxide and hydrochloric acid react to form water and aqueous sodium chloride.
Which of the following statments is not true of balancing a chemical equation? A) Subscripts in the reactants must be conserved in the products. B) Coefficients are used to balance the atoms on both sides. C) The law of conservation of matter must be followed. D) Phases are often shown for each compound but are not critical to balancing an equation.
Reaction Order and Rate Laws Abstract The purpose of the experiment is to determine the rate law for a reaction between hydrochloric acid (HCl) and sodium thiosulfate (Na2S2O3) and once found to calculate the k or specific rate constant of the reaction. To determine the reaction order and rate constant; two experiments with several trials of each will be conducted. First, the concentration of HCl will be changed while the concentration of Na2S2O3 is held constant. Next, the concentration of Na2S2O3 will be varied while the concentration of HCl is held constant. From this experimental data it is found that HCl is zero order in the reaction and Na2S2O3 is first order.
The formula for the hydrate is written as BaI2 • 2H2O And it is named barium iodide dihydrate. Mole conversions (DRAW) Nomenclature Help: B: -3 C: -2 N: -1 Cl: -1 Br: -1 I: -2 S, Se, Te: -2 P, As: -3 Si: -4 PER adds one