What are the possible sources of error when reacting sodium bicarbonate and hydrochloric acid within an evaporating dish over wire gauze over a bunsen burner? Procedure of the lab down below.
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What are the possible sources of error when reacting sodium bicarbonate and hydrochloric acid within an evaporating dish over wire gauze over a bunsen burner? Procedure of the lab down below.
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- Suppose that you are closing a cabin in the north woods for the winter and you do not want the water in the toilet tank to freeze. You know that the temperature might get as low as 30. C, and you want to protect about 4.0 L water in the toilet tank from freezing. Calculate the volume of ethylene glycol (density = 1.113 g/mL; molar mass = 62.1 g/mol) you should add to the 4.0 L water.3. Carefully put an egg in a glass half filled with vinegar. Replace the vinegar on the second day. Place the covered glass with the vinegar and egg in a safe place for one week without disturbing it. After one week, pass a light through the egg using a flashlight. N.B. DO NOT BOIL AND EAT THE EGG. A. Results and observation. Equation: HC2H3O2 + CaCO3 calcium acetate + H20 + carbon dioxide B. Calculation: If 9.02 x 1024 particles of vinegar (HC2H3O2)HC2H3O2) is added to 16.5 moles of eggshell (CaCO3) and 6.35 moles g of calcium acetate is formed. What are the (a) theoretical yield, (b) actual yield and (c) percent yieldB. Density of Liquid 1. Obtain a sample of distilled water (any quantity of your choice) anddetermine its mass and volume. Record your data on table 3 in theexperimental report 2. Calculate the density of the water sample using equation 1 Substance Density (g/mL) Substance Density (g/mL)Aluminum 2.7 Lead 11.3Brass 8.4 Zinc 7.1 Copper 8.9 Cork 0.26Tin 7.3 Silver 10.5Bone 1.80 Rhodium 12.4Iron 7.9 Platinum 21.45 Density of Liquid Density can be determined in the laboratory by measuring the mass and volume ofa substance. To measure the density of a liquid, first measure the mass of a clean,dry beaker. Then add…
- Part D: Food Calories Naked Juice Serving size 240 mL D1. Name of food product D2. Mass of food nutrients in one serving Fat Carbohydrate 33 g, Protein g, D3. Calculations for Calories (Cal) or kilocalories (kcal) per serving kcal (Cal) Carbohydrate Protein kcal (Cal) Fat kcal (Cal) D4. Total Calories (Cal or kcal) per serving kcal (Cal) D5. Calories (for one serving) listed on the label cal (Cal) D6. Percentage of total Calories from carbohydrate % (show calculations) D7. Percentage of total Calories from protein (show calculations) % D8. Percentage of total Calories from fat (show calculations) % Q 4. How does your calculated number of Calories in one serving compare to the Calories listed on the food product nutrition label? Comment on it.1. Iron metal rusts in an atmosphere of moist air. a. Physical Propertyb. Chemical Property 2. Mercury metal is a liquid at room temperature.a. Physical Propertyb. Chemical Property3. Silver salts discolor the skin by reacting with skin protein.a. Physical Propertyb. Chemical Property4. Nickel metal dissolves in acid to produce a light green solutiona. Physical Propertyb. Chemical Property 5. Potassium metal has a melting point of 63°C.a. Physical Propertyb. Chemical Property6. Titanium metal can be drawn into thin wires.a. Physical Propertyb. Chemical Property7. Silver metal shows no sign of reaction when placed in hydrochloric acid.a. Physical Propertyb. Chemical Property8. Copper metal possesses a reddish-brown color.a. Physical Propertyb. Chemical Property9. Beryllium metal, when inhaled in a finely divided form, can produce serious lung disease.a. Physical Propertyb. Chemical PropertyPrepare a solution of NaCl by accurately weighing approximately 1.45g of NaCl into a 100 mL beaker / conical flask. Record the mass of the sample. Add 25 mL distilled water. Mix until all crystals dissolve. Prepare a solution of magnesium chloride by accurately weighing approximately 3.61 g of MgCl2٠6H20 into a 100 mL beaker / conical flask. Record the mass of the sample. Add 25 mLdistilled water. Mix until all the crystals dissolve. 1. Calculate the molality of the NaCℓ and MgCℓ2.6H2O solutions. 2. Calculate the total mass of water (solvent) in kg: a) Mass of crystal water added (kg): b) Mass of water added (kg): c) Total mass of water added (kg): 3. Calculate the molality of MgCℓ2. All questions follow on from each other. Thanks very much.
- Vodka is typically 80 proof, or 40% ethanol. The density of ethanol is 0.789 g/ml, and the standard shot is 1.5 fl oz (US) or 44.36 ml. in one shot of vodka, what is the mass of ethanol? Assume the alcohol percentage is (volume of alcohol) per (volume of solution). Select one: a. 14.00 g ethanol b. 13.90 g ethanol c. 14.10 g ethanol Od. 12.05 g ethanolA student wishes to prepare 2.00 L of 0.100 M KIO3, which has a molecular weight of 214g/mol. The proper procedure is to weigh out… 42.8 g of KIO3 and add 2.00 kg of H2O 42.8 g of KIO3 and add H2O until the final homogeneous solution has a volume of 2.00 L. 21.4 g of KIO3 and add H2O until the final homogeneous solution has a volume of 2.00 liters 42.8 grams of KIO3 and add 2.00 liters of H2O 21.4 grams fo KIO3 and add 2.00 liters of H2Oa. Convert 52.6 mM (millimolar) to μM (micromolar) and to M (molar). b. Convert 200.0 μM to mM (millimolar) and to M (molar). c. The new U.S. Public Health Service optimal fluoride concentration in water is 0.700 mg/L. Convert this value to M (molar) and to ppm. Upload your responses here.
- Part F In volcano vents, sulfur is converted directly from the emitted hot gases to form mounds of solid sulfur. This is an example of Deposition. Boiling. Sublimation. freezing.A 25.0 ml aliquot of a well-shaken and filtered sample of river water is pipetted into an evaporating dish. The sample was heated to dryness. Determine the concentration of Total Dissolved Solids (TDS) in mg/L given the following data: Mass of evaporating dish = 25.5 g Mass of dried sample plus evaporating dish = 25.9729 g Note: Round off your answer to the nearest whole number.earson.com/?courseld=1 ← 2 S MISSED THIS? Read Section 4.2 (Page); Watch KCV 4.2, IWE 4.2. W Write a balanced chemical equation for each reaction. म X → #3 E D C C $ 4 R F V % 5 T G B ^ ▾ 6 Part A G Search or type URL Y Aqueous hydrogen chloride reacts with oxygen gas to form chlorine gas and liquid water. Express your answer as a chemical equation. Identify all of the phases in your answer. ² ΑΣΦ H Submit Part B A chemical reaction does not occur for this question. Part C Request Answer Solid iron(III) oxide reacts with hydrogen gas to form solid iron and liquid water. Express your answer as a chemical equation. Identify all of the phases in your answer. Submit Request Answer MacBook Pro ΑΣΦ 4 A chemical reaction does not occur for this question. & 7 N Nitrogen monoxide gas reacts with hydrogen gas to form ammonia gas and water vapor. Express your answer as a chemical equation. Identify all of the phases in your answer. U J ☆ * 00 B 8 M C w ? I ? K ( 9. < O ) - O L P A I' Review I…