the color of the flame. Test it again by observing the flame through two pieces of cobalt blue glass held together. Record the flame color with the cobalt blue glass on a separate line. You will observe the solution of sodium chloride mixed with potassium chloride without the cobalt blue glass and then again with the cobalt blue glass. Record the color of the flame seen not two separate lines.
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Results and discussion: I. a. How would you compare that relative reactivity of Na and k -Sodium and potassium react somewhat similar when reacting with water however they are slightly different. Sodium moves because of the hydrogen coming off of it and has a low melting point while potassium’s reaction is faster and enough heat is produced to set light to the hydrogen coming off of it. Each leaves a pink color hue in the water. Discuss the similarities and differences in the behavior of the metals
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the unknown elements is the same as one of the known elements‚ then they are the same element. Materials * Samples of the following metallic salts * calcium chloride * copper chloride * iron chloride * lithium chloride * potassium chloride * sodium chloride * strontium chloride * unknown 1 * unknown 2 * Bunsen burner and accessories * Safety goggles * Lab apron * Splints soaked overnight in distilled water * 250 mL. beaker full of distilled
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will produce a pure‚ intense color when present in moderate concentration. Fertilizer[edit] Potassium nitrate is mainly used in fertilizers‚ as a source of nitrogen and potassium – two of the macronutrients for plants. When used by itself‚ it has an NPK rating of 13-0-44. Oxidizer[edit] Potassium nitrate is an efficient oxidizer‚ producing a lilac-colored flame upon burning due to the presence of potassium. It is one of the three components of black powder‚ along with powdered charcoal (substantially
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concentration of Potassium Hydroxide affecting the temperature of water that it is dissolved in. One person stirred in the different concentrations of Potassium Hydroxide while the other measured the temperature as it rose after the pellets dissolved. At times it was difficult to ensure that the pellets were completely dissolved within the solution. Raw Data Table: The temperature of water after dissolving different concentrations of Potassium Hydroxide in it. Concentration of Potassium Hydroxide (g/ml)
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decomposing potassium chlorate using the reaction below. If 138.6 g of KClO3 is heated and decomposes completely‚ what mass of oxygen gas is produced? KClO3 (s) --> KCl (s) + O2 (g) [unbalanced] Answer to Practice Problem #1: 1. Balance your equation first. 2KClO3 (s) --> 2KCl (s) + 3O2 (g) [balanced] 2. Convert from grams to moles using molar mass. To get moles from grams of potassium chlorate (KClO3):
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Date Performed: July 30‚ 2012 EXPERIMENT NO. 10 COMPOSITION OF POTASSIUM CHLORIDE ABSTRACT The aim of the experiment was to look for the percentage composition of the elements present in the decomposition of potassium chlorate (KClO3) and to find out what the residue after heating was. After performing the experiment the researchers found out that there were about 66.14% of potassium chloride (KCl) in KClO3‚ and they also deducted that the residue was actually KCl. _____________________
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Experiment 7: Percentage Composition of Kclo3- A Gas law Experiment Anna CunananProfessor Stewart Chemistry 400 T/TH 1:30 PM 18 March‚ 2014 Objectives: In this Experiment‚ we will be decomposing KClO3 into two different compounds‚ KCl and O2. We are given a known mixture that has MnO2 in it to act as a catalyst. When decomposing KClO3 it releases O2 gas‚ which we then collect into the Erlenmeyer flask. The gas then displaces the water into the beaker‚ which we can then calculate the water evolved
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substances to see if they formed a double replacement reaction. We also looked for precipitants that were formed from the mixing of the different substances. We used barium nitrate‚ potassium hydroxide‚ sodium sulfate‚ magnesium nitrate‚ aluminum sulfate‚ and iron (III) chloride in set one. In set two we used potassium chloride‚ sodium hydroxide‚ magnesium nitrate‚ barium chloride‚ sodium sulfate‚ and magnesium sulfate. For each set‚ we mixed two drops of one compound in five wells of a spot plate
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How does a catalyst in the form of a metal ion affect the rate of reaction in an iodide clock reaction with potassium peroxydisulphate ions? Background When peroxydisulfate ions (S2O82-) react with iodide ions (I-) in the presence of a starch indicator‚ they produce a dark blue solution. Reaction (1) S2O82- + 3I- I3- + 2 SO42- (peroxydisulfate ion) (iodide ion) (iodine ion) (sulfate ion) To determine the rate law for this reaction a series of changes
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