than the normal saline. Results: 1. Determine the molar mass of NaCl. Show the workup. Na= 23g/mole Cl= 35g/mole Molar mass of NaCl 23g/mole+35g/mole= 58g/mole 2. Determine the molarity of the two solutions you prepared in terms of NaCl. Show the workup. Normal Saline M=Mole/L of NaCl Mass= .9g NaCl .9g=1mole/58g= .015 moles/L Nasal Irrigation Saline M=Mole/L 1.23g=1mole NaCl/58g= 71.34 moles/L 3. The University of Wisconsin recommends that if stinging or burning occurs‚ than individuals
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Data collection Quantitative Data Raw Data Table 1: Table showing the mass of the amount of unknown acid X measured in grams (±0.001g) Table 2: Table of reading of the burette initially filled with 25mL of 0.201moldm-3 sodium hydroxide (NaOH) to titrate 25mL (±0.03mL) of unknown acid X in mL (±0.05mL) after each titre. Reading on the burette initially filled with 25mL of 0.201moldm-3 NaOH (±0.05mL) First titre 21.3 Second titre 18.2 Third titre 15.2 Fourth titre 12.0 Qualitative
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reaction: 2HCl(g) ⇄ H2(g) + Cl2(g) is 0.0213 at 400 oC. If 20.0 moles of HCl(g) are heated at 400 oC‚ what amounts of HCl(g)‚ H2(g) and Cl2(g) would be present in the equilibrium mixture? (H2 = Cl2 = 2.26 moles; HCl = 15.48 moles) 3. The equilibrium constant Kc for the reaction: 2CO(g) + O2(g) ⇄ 2CO2(g) is 2.24 x 1022 at 1273oC. Calculate the Kp for the reaction at the same temperature. (1.76 x 1020) 4. A 2.50 mole sample of NOCl was placed in a 1.50-L container at 400oC. When equilibrium
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We will have one species conservation equation (IC.6.15) for each of CH4‚ O2‚ N2‚ CO2 and H2O concentrations and one equation for temperature. All of these equations use fuel consumption rate which is in the following form (from table 5.1): ⎛ mole ⎞ & {ω F }n = { .3E8 × exp(−24358 / T ) × [CH 4]−0.3 [O 2]1.3 }n ⎜ 1 ⎟ ⎝ cc. sec ⎠ Where “n” indicates the time‐step number. Assuming zero heat transfer to the reactor‚ the temperature equation is: & ⎧ − ∑ (h f ‚i + c p ‚i (T − Tref
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property which could be monitored in order to measure the rate of reaction. ("a" is done as an example.) a) 3H2(g) + N2(g) 2NH3(g) Pressure will decrease as reaction proceeds because you are going from 4 moles of reactants to 2 moles of products. Assuming you have a constant volume‚ less moles exert less pressure. b) CaCO3(s) CaO(s) + CO2(g) Two things could be monitored here. Look at the states of everything carefully. c) 2NO2(g) N2O4(g) brown colourless Two things could be monitored
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GRAVIMETRIC ANALYSIS OF A CHLORIDE SALT Report Submitted by: Ronald Milner Laboratory partner: Kiesha Mantik Lab Performed: February 16th‚ 2012 Group: Thursday Afternoon‚ Group F Date submitted: March 14th‚ 2012 Purpose: To determine the chloride content of an unknown soluble salt while illustrating the techniques involved in gravimetric analysis. Theory: In order to find the chloride content of an unknown soluble salt‚ that chloride can first be extracted from the
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methylene blue. The average diameter of potassium permanganate (11.64 mm) was bigger than potassium dichromate (9.18 mm) and methylene blue (7.91 mm). Note that the molecular weight of potassium permanganate is 158g/mole‚ potassium dichromate is 294 g/mole and methylene blue is 374 g/mole. Thus‚ the lighter the molecular weight‚ the faster the rate of diffusion. INTRODUCTION Diffusion is the process in which the molecules merge as an outcome of their spontaneous movement or randomized motion of kinetic
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react together: They must collide with each other The collisions must have enough energy The independent variable in this particular reaction is the concentration of the hydrochloric acid. Each time the concentration will be increased by 0.25 moles. This will ensure that our readings are close and help when working out the rate of reaction. So that it will be easier to make comparisons. The dependent variable will be the volume of hydrogen gas produced and this will be measured using the inverted
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hydrate CaSO4·XH2O (trial 1): (mass of hydrated salt – mass of anhydrous salt) (1.99 – 1.595) = 0.395 g Mass percent of water in unknown hydrate CaSO4·XH2O (trial 1): (mass of water / mass of hydrated salt) x 100 (0.395 / 1.99) x 100 = 19.85 % Initial mole calculation for CaSO4 (trial 1): (mass anhydrous salt / molecular weight of salt)
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TOPIC 2 Metals The History of Metals * Uses of metals through history: * Copper Age (3200-2300 BCE) – copper and tin were most common metals‚ and were used for ornaments‚ weapons and tools. * Bronze Age (2300-700 BCE) – copper‚ tin and bronze were used for tools‚ weapons and transport. They produced bronze by heating copper and tin with charcoal. * Iron Age (1000 BCE – 1 CE) – iron steel and lead was used for tools‚ weapons and pipes. Iron is much harder than bronze.
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