Be sure to answer all parts.Pheromones are a special type of compound secreted by the females of many insect species to attract themales for mating. One pheromone has the molecular formula C19H350. Normally, the amount of thismolecules does this quantitypheromone secreted by a female insect is about 1.2 x 10 12g.Howmanycontain?x 10moleculesEnter your answer in scientific notation.

For this question, first calculate number of moles for pheromone and then convert that moles in…

Be sure to answer all parts. Pheromones are a special type of compound secreted by the females of many insect species to attract the males for mating. One pheromone has the molecular formula C19H35O. Normally, the amount of this pheromone secreted by a female insect is about 1.2 x 10-12 contain? g. How many molecules does this quantity x 10 molecules Enter your answer in scientific notation.

Be sure to answer all parts. Pheromones are a special type of compound secreted by the females of many insect species to attract the males for mating. One pheromone has the molecular formula C19H35O. Normally, the amount of this pheromone secreted by a female insect is about 1.2 x 10-12 contain? g. How many molecules does this quantity x 10 molecules Enter your answer in scientific notation.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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[Tutorial: Limiting reactant stoichiometry] This question will walk you through the steps of calculating the mass of products produced based on your determination of the limiting reactant. b) Step 2a: Use dimensional analysis to determine the theoretical yield of the product. Calculate the theoretical yield in grams Al₂O₃ from the complete reaction of 64.7 grams Al according to the following balanced chemical equation: 2 Al(s) + Fe₂O₃(s) → Al₂O₃(s) + 2 Fe(s) c) Calculate the theoretical yield in grams Al₂O₃ from the complete reaction of 201 grams Fe₂O₃ according to the following balanced chemical equation: 2 Al(s) + Fe₂O₃(s) → Al₂O₃(s) + 2 Fe(s) d) Which of the following substances is the limiting reactant? e) What is the mass in grams of the excess Fe₂O₃ remaining after the partial reaction of 201 g Fe₂O₃ with 64.7 g Al? Give your answer to three significant figures.
When answering this problem, report the answer with the appropriate number of significant figures. Enter your answer USING scientific notation. When entering units, use proper abbreviated units with proper capitalization. In this experiment, a series of solutions are prepared by combining multiple components into a single container. One solution prepared contains 5.00 mL of 0.010 molar KI, 10.00 mL of 0.0010 molar Na2S2O3, 15.00 mL of water, 10.00 mL of 0.040 molar KBrO3, and 10.00 mL of 0.10 molar HCl. What is the concentration of iodide ions in this solution? Answer: ____x10______units
When answering this problem, report the answer with the appropriate number of significant figures. When entering units, use proper abbreviated units with proper capitalization. A titration is performed to determine the amount of sulfuric acid, H2SO4, in a 6.5 mL sample taken from car battery. About 50 mL of water is added to the sample, and then it is titrated with 43.37 mL of a standard 0.5824 molar NaOH solution. You balanced this reaction in a previous problem.How what is the molar concentration of sulfuric acid in the original sample? Present the answer in the following form. Answer: _____ x10 ___power ___units
A chemist adds 160.0mL of a ×9.310−5/molL magnesium fluoride MgF2 solution to a reaction flask. Calculate the mass in milligrams of magnesium fluoride the chemist has added to the flask. Be sure your answer has the correct number of significant digits. mg
Solutions of sodium carbonate and silver-nitrate react to form solid silver carbonate and a solution of sodium nitrate. A solution containing 8.00 g of sodium carbonate is mixed with one containing 4.00 g of silver nitrate. After the reaction is complete, the solutions are evaporated to dryness, leaving a mixture of salts. How many grams of each of the following compounds are present after the reaction is complete? sodium carbonate 1.52 silver nitrate 0 X 9 sodium nitrate 12.84 ✓ q silver carbonate 6.48 X g X 9 D
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13. Aluminum metal (Al) reacts with sulfur (S) to produce aluminum sulfide (ALS) according to this balanced chemical equation: 2 Al(s) + 3 S(s) → AlS(s) How many atoms of aluminum will react completely with 1.33 x 10 atoms of sulfur?
A molecular formula expresses the number of each kind of atom in a molecule. For example, the molecular formula for propene, C3H6C3H6, indicates three carbon atoms and six hydrogen atoms per molecule. This also means that one mole of propene contains three moles of carbon and six moles of hydrogen.An empirical formula expresses the mole ratio of the elements. The empirical formula for propene is CH2CH2, indicating twice as much hydrogen as carbon. When analyzing unknown compounds in a lab, it is often possible to identify the mole ratios, and thus the empirical formula, but not the molecular formula.Notice that the molecular mass of propene, 3(12)+6(1)=42amu3(12)+6(1)=42amu, is a multiple of the empirical formula mass, 1(12)+2(1)=14 amu An unknown compound contains only carbon, hydrogen, and oxygen (CxHyOzCxHyOz). Combustion of 6.50 gg of this compound produced 9.53 gg of carbon dioxide and 3.90 gg of water. Part A How many moles of carbon, CC, were in the original sample?…
The formula for alum is KAl(SO4)2 x 12 H2O. All of the atoms in this formula contribute to the molar mass. When you add up all the masses in the formula, the molar mass is 474.39 grams/mole. The molar mass of aluminum is 26.98. If you started this experiment with 1.063 grams of aluminum foil, what is the theoretical yield of Alum? Give your answer to 1 decimal place. __________________________ The actual yield of alum in the lab was 17.8 grams. What percentage yield is this? Give your answer to 1 decimal place. ____________________________
A sample of bismuth weighing 0.687 g was converted to bismuth chloride by reacting it first with HNO3, and then with HCI, followed by careful evaporation to dryness. The mass of the bismuth chloride obtained was 1.032 g. What is the empirical formula of bismuth chloride? You won't be able to make the numbers a subscript. For instance, for MgCl2 enter MgCl2.
A. What is the density of an unknown liquid if 15.00 mL of the unknown has a mass of 12.257 g? B. A sample of chromium is heated in a crucible over a Bruson burner until the chromium turns into a grey powder. If the original chromium had a mass of 0.357 g and the chromium oxide has a mass of 0.522 g, what is the empirical formula of the chromium oxide?
[Tutorial: Limiting reactant stoichiometry] This question will walk you through the steps of calculating the mass of products produced based on your determination of the limiting reactant. Step 3: Determine the limiting reactant. You have determined complete reaction of 64.7 g aluminum (Al) would give a theoretical yield of 122 g aluminum oxide (Al2O3), whereas complete reaction of 201 g iron (III) oxide (Fe203) would give a theoretical yield of 128 g aluminum oxide (Al203). Which of the following substances is the limiting reactant? A) aluminum (AI) B) iron (III) oxide (Fe2O3) C) aluminum oxide (Al2O3) D) iron (Fe)