▾ Part ACombustion analysis of toluene, a common organic solvent, gives 3.52 mg of CO2 and 0.822 mg of H₂O. If the compound contains only carbonand hydrogen, what is its empirical formula?Express your answer as a chemical formula.ΑΣΦA chemical reaction does not occur for this question.Submit Request AnswerPart B?Menthol, the substance we can smell in mentholated cough drops, is composed of C, H, and O. A 5.025x10-2-mg sample of menthol is combusted,producing 0.1415 mg of CO2 and 5.795×10-2 mg of H₂O. What is the empirical formula for menthol?Express your answer as a chemical formula.ΑΣΦΑ?A ▾ Part CIf the compound has a molar mass of 156 g/mol, what is its molecular formula?Express your answer as a chemical formula.ΑΣΦftO?A chemical reaction does not occur for this question.Submit Request Answer

Part A :Given question related to calculation of empirical formula from combustion data. “Since you…

Part A Combustion analysis of toluene, a common organic solvent, gives 3.52 mg of CO₂ and 0.822 mg of H₂O. If the compound contains only carbon and hydrogen, what is its empirical formula? Express your answer as a chemical formula. ΑΣΦ ? A chemical reaction does not occur for this question.

Part A Combustion analysis of toluene, a common organic solvent, gives 3.52 mg of CO₂ and 0.822 mg of H₂O. If the compound contains only carbon and hydrogen, what is its empirical formula? Express your answer as a chemical formula. ΑΣΦ ? A chemical reaction does not occur for this question.

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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4.33 g sample of a compound consisting of carbon, hydrogen, oxygen, nitrogen, and sulfur was combusted in excess oxygen. This produced 6.38 g CO2 and 2.88 g H2O. A second sample of this compound with a mass of 5.05 g produced 2.70 g SO3. The third sample of this compound with a mass of 6.95 g produced 2.94 g of HNO3. What is the empirical formula of the compound?
A 6.40 g sample of a compound is burned to produce 8.37 g CO, 2.75 g HO, 1.06 g N, and 1.23 g SO. What is the empirical formula of the compound? Give your answer in the form C#H#N#O#S# where the number following the element’s symbol corresponds to the subscript in the formula. (Don’t include a 1 subscript explicitly).
Compound Z is a chemical naturally found in peppermint and other mint plants and has mild anesthetic properties. In a combustion analysis experiment, 95.6 mg of Compound Z (molar mass = 156 g/mol) are burned in oxygen gas to give 269 mg CO2 and 110 mg H20. What is Compound Z's empirical formula? Write the numbers that you would write in the subscript of the formula in the boxes next to the symbol of the element. If the subscript is 1, type 1 although you normally would not write 1 in the formula. H.
Part a) When FeS3 • 2H2O is heated, it gives off water, SO2 and Fe2O3. Is this a chemical or physical change? When CuSO4 • 5H2O is heated, it gives off water and CuSO4. Is this a chemical or physical change? Which of these changes can be easily reversed? Part b) Is the molar ratio of the products is different from the molar ratio in the hydrate formula, has a chemical or physical change taken place?
A 3.000 g sample of a gaseous compound was found to contain 2.560 g of carbon and 0.440 g of hydrogen. A) What is the simplest formula of the compound (Write C first and then H)? You won't be able to make the numbers a subscript. For instance, for MgCl2 enter MgCl2. B) The molar mass of the compound was found to be 42.08 g/mol. What is the molecular formula of the compound? You won't be able to make the numbers a subscript. For instance, for MgCl2 enter MgCl2.
When 7.003 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 20.50 grams of CO2 and 12.59 grams of H2O were produced.In a separate experiment, the molar mass of the compound was found to be 30.07 g/mol. Determine the empirical formula and the molecular formula of the hydrocarbon. Enter the elements in the order presented in the question.
Combustion analysis of 1.200 g of an unknown compound containing carbon, hydrogen, and oxygen produced 2.086 g of CO2 and 1.134 g of H2O. What is the empirical formula of the compound?Combustion analysis of 1.200 g of an unknown compound containing carbon, hydrogen, and oxygen produced 2.086 g of CO2 and 1.134 g of H2O. What is the empirical formula of the compound?C2H5OC3H8O2C2H5O2C2H10O3
Combustion of a hydrocarbon in a limited supply of air produces CO in addition to CO2 and H2O. When 1.80 g of a particular hydrocarbon was burned in air, 1.74 g CO, 2.73 g CO2, and 2.80 g H2O were produced. What is the empirical formula of the hydrocarbon? Calculate the mass of oxygen used in the reaction. Calculate the total mass of oxygen that would have been required for complete combustion.
Click in the answer box to activate the palette. Menthol is a flavoring agent extracted from peppermint oil. It contains C, H, and O. In one combustion analysis, 10.00 mg of the substance yields 11.53 mg H,0 and 28.16 mg CO2. What is the empirical formula of menthol? Add subscripts to complete the empirical formula. CHO
A student performed a similar experiment to the one you performed: They took a crucible and lid, cleaned them, heated them over a flame, and after cooling found their combined mass to be 22.538 g. The student then added a sample of zinc(II) sulfate hydrate (ZnSO4·“n”H2O) to the crucible so the combined mass of the sample, crucible, and lid was 25.896 g. They heated this sample for 10 minutes with the lid ajar, let it cool, and measured the mass of the crucible, sample, and lid to be 25.054 g. a. Based on this experiment, what is the formula for they hydrated zinc(II) sulfate compound? b. The student later looked on the reagent bottle for zinc(II) sulfate hydrate and found the actual formula was ZnSO4·7H2O. If everything had been done correctly, what value should the student have expected for the final mass of their sample, crucible, and lid after heating?
43. One of the ingredients in the Native American stomachache remedy derived from common chokecherry is caffeic acid which is comprised of carbon, hydrogen, and oxygen only. Combustion of 1.00  102 mg of caffeic acid yielded 220 mg of CO2 and 40.3 mg of H2O. Determine the empirical formula of caffeic acid. You may check your answer by looking up the answer, but do not use the formula to solve the problem.
In a combustion analysis experiment, an unknown hydrocarbon produced 69.97749 g of carbon dioxide and 38.19392 g of water. Assume all of the carbon present in the initial sample ends up in the carbon dioxide produced and that all of the hydrogen present in the original sample ends up in the water produced. What is the empirical formula of the hydrocarbon?