What is the empirical formula of a hydrocarbon that contains 89.94% C by mass?

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  1. chemistry- empirical formulas

    Calculate the empirical formula of a molecule with the following percent compositions: 55.0% gallium (Ga) and 45.0% fluorine (F). mass of 100g #of Moles in 100g of the compound Ga55.0% _____ ______ F45.0% ______ _______ c. Determine the molecular formula

  2. Chemistry

    1) A compound has the following percentages by mass: barium, 58.84%; sulfur, 13.74%; oxygen, 27.43%. Determine the empirical formula of the compound. 2) If a 1.271-g sample of aluminum metal is heated on a chlorine gas atmosphere, the mass of aluminum

  3. Chemistry

    what is the molecular formula of a compound that is 54.5% C, 9.09% H, and 36.4% O. with a molecular weight of 176g/mol. A)C8H16O4 B)C4H8O2 C)C7H12O5 D)C9H18O3 Assume you have 100 g of the substance, then you have 54.5g of C, etc. Moles C= 54.5/12=4.54 mol

  4. AP Chemistry

    An organic compound was synthesized and found to contain only C, H, N, O, and Cl. It was observed that when .150g sample of the compound was burned, it produced .138g of CO2 and .0566g of H2O. All the Nitrogen in a different .200g sample of the compound

  5. IGCSE Chemistry

    Hydrocarbons A and B both contain 85.7 % carbon. Their molar masses are 42 and 84 respectively. a) Which elements does a hydrocarbon contain? b) Calculate the empirical formula of A and of B. c) Calculate the molecular formula of A and B. I solved a) and

  6. chemistry

    Complete combustion of 4.80 g of a hydrocarbon produced 15.6 g of CO2 and 4.80 g of H2O. What is the empirical formula for the hydrocarbon?

  7. chemistry--help

    a compound contains 63.15% Carbon, 5.30% hydrogen, 31.55% oxygen. Its molar mass is 152.14 g/mol. determine the empirical and molecular formula. I get the empirical formula to be C8H803 is it right because it is not fitting the molecular formula because

  8. Chemistry

    Please check my answers for the following questions. THANK YOU. 1) The empirical formula of a compound that is 25.9% nitrogen and 74.1% oxygen is.... ANSWER: N2O 2) empirical formula of a compound that consists of 4.80 grams of carbon, 1.20 grams of

  9. Chemistry

    2) What is the empirical formula of a compound containing C, H, O if combustion of 1.23g of the compound yields 1.8g CO2 and .74g of H2O 3) What are the empirical and molecular formulas of a hydrocarbon if combustion of 2.10g of the compound yields 6.59g

  10. Chemistry

    A certain compound containing only carbon and hydrogen was found to have a vapor density of 2.550 g/L at 100 degrees C and 760 mm Hg. If the empirical formula of this compound is CH, what is the molecular formula of this compound? I had some ideas as to

  11. chemistry

    1.to calculate the percent by massof an element in a known compound, divide the mass of the element in one mole by the _______and multiply by 100%. A(n) _______formula represents the lowest________ratio of the elements in a compound. It can be calculated

  12. Chemistry

    I am completing my lab and cannot figure this out. I need someone to go over it and make sure I am right because I can't figure out why my empirical formula does not match the molecular formula. #7 is the one I am really having a problem with, but here is

  13. Chemistry HELP

    Complete combustion of 3.30 g of a hydrocarbon produced 10.2 g of CO2 and 4.68 g of H2O. What is the empirical formula for the hydrocarbon? I did the calculation and the ratio comes out to C: 1 H: 2.24 So I thought the answer is CH2 but apparently its

  14. AP Chemistry

    a 5.15g sample of a hydrocarbon is burned in oxygen, producing 15.6g of carbon dioxide and 8.45g of water. Assuming an excess of oxygen, what is the empirical formula of the hydrocarbon?

  15. chem

    Citric acid, the compound responsible for the sour taste of lemons, has the following elemental composition: C, 37.51%; H, 4.20%; O, 58.29%. Calculate the empirical formula of citric acid. so i did that and got C6H8O7 but now i need to find the molecular

  16. chemistry

    If a compound's empirical formula is CH2O and its' formula mass is 120.12 amu, what is its' molecular formula

  17. AP Chemistry

    a 5.15g sample of a hydrocarbon is burned in oxygen, producing 15.6g of carbon dioxide and 8.45g of water. Assuming an excess of oxygen, what is the empirical formula of the hydrocarbon? how do i set this problem up and how do i solve it?

  18. chemistry

    A 8.408 gram sample of an organic compound containing C, H and O is analyzed by combustion analysis and 12.53 grams of CO2 and 3.849 grams of H2O are produced. In a separate experiment, the molar mass is found to be 118.1 g/mol. Determine the empirical

  19. Chemistry

    An unknown gaseous hydrocarbon contains 85.63 % carbon. If its density is 0.488 g/L at 0.355 atm and 100°C, what is the molecular formula of the gas? I can't figure this out. By assuming the total mass to be 100g, I get 85.63g C and 14.37g H which I then

  20. Chemistry

    a hydrocarbon is burnt completely in excess oxygen. it is found that 1.00g of the hydrocarbon gives 2.93g carbon dioxide and 1.80g water. find the empirical formula of the hydrocarbon (H=1,C=12,O=16)

  21. Chemistry

    What is the empirical formula of a hydrocarbon that contains 89.94% C by mass?

  22. chemistry

    combustion analysis of a hydrocarbon produced: 33.01 g CO2 and 13.51 g H2O Calculate the empirical formula of the Hydrocarbon. I got CH5 but that doesn't seem right? how do i do this problem?

  23. Chemistry

    A hydrocarbon Y on combustion gives 0.352g of carbon(iv)oxide and 0.18g of water. Calculate the empirical formula of the compound and If the relative molecular mass of Y is 58g, determine the molecular formula of Y.?

  24. chemistry

    A compound is found to be 51.39% carbon, 8.64% hydrogen, and 39.97% nitrogen. It has a molecular molar mass of 140.22 g/mol. (This question requires one to find the empirical formula to end up with the final answer in molecular formula) A. C10H14N2 B.

  25. Chemistry

    9. Complete combustion of a 0.20 mole sample of a hydrocarbon, CxHy, yields 0.80 mol of CO2 and 1.0 mol of H2O. What is the empirical formula for the hydrocarbon? A. C2H5 B. C4H5 C. C4H8 D. C4H10 E. C3H8 I have C4H8 Correct?

  26. Chemistry

    A .7178 g sample of a hydrocarbon occupies a volume of 390.7 mL at 65C and 99.2kpa. When the sample is burned in excess oxygen, 2.4267 g CO2 and .4967g H2O are obtained. What is the molecular formula of the hydrocarbon? Write a plausible structural formula

  27. chemistry - empirical formula

    write the empirical formula for each of the following molecular formulae" a)P4O10 b)C2H6 Confused as to what the diff.is b/w empirical and formula...have no idea how to answer these b/c they look like empirical formulas to me

  28. Chemistry (Check)

    True or False The empirical formula of a compound is always the same as the molecular compound. My Answear: True The empirical formula for acetylene is CH. The molecular formula is C2H2. Another example: The empirical formula for glucose is CH2O. The

  29. chemistry

    Combustion analysis of a hydrocarbon produced 33.01 g {\rm CO}_2 and 27.04 g {\rm H}_2{\rm O}. Calculate the empirical formula of the hydrocarbon. Express your answer as a chemical formula.

  30. Chemistry

    If you divide the molar mass of a compound by the empirical formula mass, what is the result? That division should be VERY close to a whole number. Usually, 0.9 to 1.1 or 1.9 to 2.1 (all depending upon the accuracy and precision of experimental data). That

  31. Chem

    Complete combustion of 8.30 g of a hydrocarbon produced 26.7 g of CO2 and 9.10 g of H2O. What is the empirical formula for the hydrocarbon? My Work: First I tried to find the Amount of C and H in the product... Which I got 1 Mole of Carbon and 2 moles of

  32. chemistry.

    What is the empirical formula of a hydrocarbon that contains 89,94 by mass?

  33. Chemistry

    Complete combustion of 7.00 g of a hydrocarbon produced 21.4 g of CO2 and 10.2 g of H2O. What is the empirical formula for the hydrocarbon?

  34. Chemistry

    Complete combustion of 8.00 g of hydrocarbon produced 26.0g of CO2 and 7.99g of H2O. What is the empirical formula for the hydrocarbon?

  35. Chemistry

    Complete combustion of 7.70 g of a hydrocarbon produced 23.7 g of CO2 and 10.9 of H2O. What is the empirical formula of the hydrocarbon? I first calculated the moles of both the carbon dioxide and the water, but I have no idea where to go from there. Any

  36. Chemistry

    In a gravimetric analysis, 0.1595g of a hydrocarbon upon combustion produces 0.5008g CO2 and 0.2041g H2O. Its molar mass is found in another experiment to be 70.13g/mol. Determine the empirical formula and it's molecular formula.

  37. chem

    a hydrocarbon has an empirical formula CH and a vapour density of 39. Determine its molecular formula. solution.................................................... CH=12+1 n=13 13n=39 =3

  38. chemistry

    How do I find the empirical formula for aluminium selenide? You have to have some data, such as masses, or percent: Empirical means it was measured. The empirical formula for aluminium selenide is the same as it's molecular formula; Al2Se3. The empirical

  39. Finding the Molecular Formula

    A certain compound containing only carbon and hydrogen was found to have a vapor density of 2.550 g/L at 100 degrees C and 760 mm Hg. If the empirical formula of this compound is CH, what is the molecular formula of this compound? I had some ideas as to

  40. Chemistry

    I need some help with some of these questions: The action of bacteria on meat and fish produces a poisonous compound called cadaverine. As its name implies, it stinks! It is 58.77 percent carbon, 13.81 percent hydrogen, and 27.40 percent nitrogen. Its

  41. Chemistry

    I'm confused on how to set up the problem for each question.. 1.) Calculate the empirical formula of a compound if a 6.21 g sample contains 1.67g of cerium and the remainder iodine 2.) An unknown compound contains 85.64% carbon with the remainder hydrogen.

  42. Chemistry Really Confused!!

    'm confused on how to set up the problem for each question.. 1.) Calculate the empirical formula of a compound if a 6.21 g sample contains 1.67g of cerium and the remainder iodine 2.) An unknown compound contains 85.64% carbon with the remainder hydrogen.

  43. Molecular formula

    I have to find the molecular formula for As2O3, to do so I have to divide its molecular mass by its empirical mass. I have worked ou that its molecular mass is 197.9 g/mol. How would I find its empirical mass, is it not the same as its molecular mass? Many

  44. general chemistry

    A 1.24g sample of a hydrocarbon, when completely burned in excess of O2(g), yields 4.04g CO2 and 1.24g H20. Determine the empirical formula.

  45. Organic Chemistry

    "Cabbage leaves are coated with a hydrocarbon of molecular formula C29H60. What purpose might this hydrocarbon coating serve?" This is a question from a textbook. Anything helps!!

  46. Chemistry

    A compound of B and H is found to have a mass percent composition of 81.1% Boron. Its empirical formula is B2H5. A mass spectrometry experiment tells us that the molecular mass is 53.3 g/mol. What is its molecular formula? So I feel like this is a trick

  47. chem

    When 3.517 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 11.59 grams of CO2 and 3.164 grams of H2O were produced. In a separate experiment, the molar mass of the compound was found to be 40.06 g/mol. Determine the empirical

  48. chemistry

    complete combustion of a 0.0100mol sample of hydrocarbon, CxHy, gives 1.344 L of CO2 at STP and 0.720 g of H2O. a. what is the molecular formula of hydrocarbon? b. what is the empirical formula of hydrocarbon?..

  49. chemistry

    in an experiment a sample of hydrocarbon was analyzed. The sample contained6 g of carbon and 1.344 g Hydrogen. a) whats the empirical formula? the density of hydrocarbon at 25 C and 1.09 atm is 1.96 g/L b.) whats the molar mass of the hydrocarbon? c) whats

  50. chemistry

    a hydrocarbon was burnt completely and the products were bubbled into excess of Ca(OH)2 solution. The resulting mixture was filtered, and the residue dried and weighed. The mass of the hydrocarbon was found to be 10.00g. In a separate experiment, the same

  51. chemistry

    Combustion analysis, Empirical and Molecular formulas, help!? When 2.686 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 9.224 grams of CO2 and 1.511 grams of H2O were produced. In a separate experiment, the molar mass of the

  52. Chemistry

    A 0.1592g sample of a hydrocarbon upon combustion analysis produces 0.5008g CO2. Its molar mass is found in another experiment to be 70g mol. Determine the empirical formula, and its molecular formula. I completely messed up this question, and I don't know

  53. Chemistry

    When 1.578 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 4.951 grams of CO2 and 2.027 grams of H2O were produced. In a separate experiment, the molar mass of the compound was found to be 56.11 g/mol. Determine the empirical

  54. Chemisty!

    a flask with a volume of 267.5 mL contains a few milliliters of a volatile hydrocarbon. after vaporizing the gas at 100 degrees C, the flask is weighed and found to contain 0.728 grams of hydrocarbon vapor at 755 mmHg. a separate combustion analysis

  55. chemistry

    a flask with a volume of 267.5 mL contains a few milliliters of a volatile hydrocarbon. after vaporizing the gas at 100 degrees C, the flask is weighed and found to contain 0.728 grams of hydrocarbon vapor at 755 mmHg. a separate combustion analysis

  56. Chemistry

    A 1.24-g sample of a hydrocarbon, when completely burned in an excess of O2(g), yields 4.04 g CO2 and 1.24 g H2O Draw a plausible structural formula for the hydrocarbon molecule. I think I understand how to get it to an empirical formula but I don't know

  57. Chemistry

    What is the empirical formula of a hydrocarbon that contains 89.94% C by mass?

  58. chemistry

    Complete combustion of 8.80 g of a hydrocarbon produced 27.1 g of CO2 and 12.5 g of H2O. What is the empirical formula for the hydrocarbon?

  59. chemistry

    Complete combustion of 4.20 g of a hydrocarbon produced 13.4 g of CO2 and 4.81 g of H2O. What is the empirical formula for the hydrocarbon?

  60. Chemistry

    Hydrocarbon burn in excess oxygen yields 4.4g of carbon(iv)oxide and 2 of 7g of water. Find the empirical formula of hydrocarbon

  61. chem 1411

    A combustion analysis of a 0.00134g sample (CxHy) of a hydrocarbon yields 0.00375g of CO2 and 0.00164g of H2O. What is the empirical formula of the hydrocarbon?

  62. Chemistry

    When 1.5g of a hydrocarbon was completely burnt in excess oxygen gas,4.395g of carbon dioxide and 2.70g of water was produced. Determine the empirical formula of the hydrocarbon.(C=12,H=1,O=16)

  63. Chemistry

    A liquid hydrocarbon (Cx Hy) is found to be 16.37% H by mass. A 1.158-g vaporized sample of the hydrocarbon has a 358 mL volume at 71.0 C and 749 mmHg. what is the molecular formula for this hydrocarbon?

  64. chemistry

    Derive the empirical formula of a hydrocarbon that on analysis gave the following percentage by mass composition: C = 85.63 % and H = 14.37 %. If the molecular mass of this compound is 56 g, derive the molecular formula.

  65. Chemistry

    0.717 g of a compound containing carbon, hydrogen, and oxygen is burned and found to produce 1.02 g CO2 and 0.624 g H2O. The molar mass of the compound is 124 g/mol. (a) Write a chemical equation for the combustion of this unknown hydrocarbon. (b)

  66. Chemistry

    Compound K is a hydrocarbon. Combustion of 6.51 g of K gave 20.47 g of carbon dioxide and 8.36 g of water. The relative molecular mass of K was found to be 84. Calculate the empirical and molecular formula of K

  67. Chemistry

    0.717 g of a compound containing carbon, hydrogen, and oxygen is burned and found to produce 1.02 g CO2 and 0.624 g H2O. The molar mass of the compound is 124 g/mol. (a) Write a chemical equation for the combustion of this unknown hydrocarbon. (b)

  68. Chemistry

    I need some help with some of these questions: The action of bacteria on meat and fish produces a poisonous compound called cadaverine. As its name implies, it stinks! It is 58.77 percent carbon, 13.81 percent hydrogen, and 27.40 percent nitrogen. Its

  69. chemistry

    Determining a Molecular Formula from an Empirical Formula 1. A compund has an experimental molar mass of 78g/mol. Its empirical formula is CH. What is its molecular formula?

  70. chemistry

    Determining a Molecular Formula from an Empirical Formula 1. A compund has an experimental molar mass of 78g/mol. Its empirical formula is CH. What is its molecular formula?

  71. Chemistry

    Maleic acid is an organic compound composed of 41.39% C, 3.47% H, and the rest oxygen. If 0.271 mol of maleic acid has a mass of 31.4 g, what are the empirical and molecular formulas of maleic acid? My work: C: 41.39 g x (1 mol/12.01 g) = 3.44629 = 1 H:

  72. chemistry

    a certain hydrocarbon has the analysis C=85.84% and H=14.16%. the density of its vapour is 2.50g/L at STP. find the empirical and molecular formula.

  73. chemistry

    0.60g of a gaseous hydrocarbon E when completely burnt in oxygen gave 1.76g of carbon dioxide. WHAT IS THE EMPIRICAL FORMULA OF E?

  74. science

    15g of an unknown hydrocarbon burns in oxygen to give 4,7g of carbon dioxide and 19,35g of water calculate the empirical formula

  75. chemistry

    A gas has an empirical formula of POF3. If 0.350L of the gas at STP has a mass of 1.62g, what is the molecular formula of the mass? molar mass= 1mol x 22.4L/1mol x 1.62g/0.350L = 103.7g molarmass/empirical formula mass = 103.7g/214.5g = 0.4834 ... how do I

  76. chem

    combustion analysis of a 285.7 mg sample of a hydrocarbon produces 880.8 mg of CO2 ans 405.7 mg of H2O. What is the empirical formula of the compound? a rough measurement of the molecular weight indicates it is a little over 100mg/mol. what is the

  77. Chemistry

    Styrene is a hydrocarbon. If .438 g of the compound is burned and produces 1.48 g CO2 and .303 g of H2O what is the empirical formula of the compound?

  78. Chemistry

    When 1.63 g sample of an unknown hydrocarbon is completely burned in oxygen, 4.97 g of CO2 are produced. What is the percentage by mass of hydrogen in this hydrocarbon? THANK YOUU Found out the formula: 4CH+5O2--> 4CO2+2H2O then found out the moles of CH=

  79. chemistry

    I have a chemical composition of As2O3. How do I calculate the mass of oxygen that combines with 1 mol of arsenic to form the oxide of arsenic? How do I use this to obtain the empirical formula of the oxide? That IS the empirical formula of the compound.

  80. Chemistry (Check)

    Classify each of these statements as always true, sometimes true, or never true. 7____AT____It is necessary to know the formula of a compound in order to calculate its percent composition. 8___ST_____If the percent by mass of carbon in methane, CH4, is

  81. Chemistry

    Xenon of mass 5.08 g reacts with fluorine to form 9.49 g of a xenon fluoride. What is the empirical formula of this compound? A) XeF6 B) XeF4 C) XeF2 D) XeF E) Xe2F I am not familiar with these types of empirical formula problems. If I'm given the

  82. chem

    could anyone tell me why the molecular formula of agas is not always the same as the empirical formula tnx It may be a dimer or a trimer. For example, CH is the empirical formula for acetylene but the molecular formula is HC(triple bond)CH or C2H2.

  83. Chemistry

    Sometimes, instead of percentages compostion, you will have the composition of a sample by mass. Using the actual mass of the sample, determine the empirical formula for compounds that have the following analyses. A. a .858g sample of an unkown substance

  84. chemistry

    lactic acid is the avid responsible for the sour test in spit milk. on the basis of combustion analysis, it's percentage composition by mass is 40.00% carbon, 6.71%hydrogen and x% oxygen. a. Calculate the empirical formula of lactic acid b. The molar mass

  85. chemistry

    A compound has the following composition. C 54.5%, H 9.10% and 0 36.4% its molecular weight is 88.10. Determine its empirical formula and molecular formula. Take 100 g sample. That gives you 54.5 g C, 9.10 g H and 36.4 g O. Now convert those grams to mols.

  86. chemistry

    A 2.000g sample of magnesium was burned in air to form an oxide. After the product was purified it was found to have a mass of 3.317g. What is the empirical formula for the product? I know how to find a empirical formula, I just don't understand what

  87. Science/ Chemistry

    When 0.422 g of phosphorus is burned, 0.967 g of a white oxide (a compound of phosphorus and oxygen) is obtained. a. Determine the empirical formula of the oxide. So for the empirical Formula I got P_2O_5 now it wants me to Write a balanced equation for

  88. Chemistry

    For Peroxyacyl nitrate (PAN) A compound of C,H,N,O Determine the empirical formula from the percent composition by mass: 19.8% C, 2.50% H, 11.6% N What is its molecular formula given that its molar mass is about 120g?

  89. Chimstery

    (white Powder) : 42.2% carbon, 6.4% Hydrogen, and 51.4% Oxygen Formula Mass = 342.2965 amu Molecular Formula: Empirical Formula: Identity?what does the drug do?

  90. Treacher girls scholl

    A hydrocarbon is burnt completely in air to form 13.2g of carbon dioxide gas and 7.2g of water. What is the molecular formula of the hydrocarbon?

  91. Chemistry

    What is the empirical formula of benzene, C6H6? I know how to find empirical formula; as long as you know the moles, you can find the ratio and thus the empirical formula. But the question provides nothing and I can only find the Mr? The answer from the

  92. Chemistry

    A 10.0000 g block of aluminum is heated and placed in a stream of oxygen gas, resulting in the formation of aluminum oxide on the surface of the block. The block is cooled and weighed and found to have a mass of 11.6471 g. The block is then placed in a

  93. Chemistry

    A 10.0000 g block of aluminum is heated and placed in a stream of oxygen gas, resulting in the formation of aluminum oxide on the surface of the block. The block is cooled and weighed and found to have a mass of 11.6471 g. The block is then placed in a

  94. Chemistry

    4.12 grams of Zinc are placed in a crucible with 3.00 grams (excess) of Sulfur. when reaction is complete the product mass is 6.10 grams. What mass of Sulfur should be used in the simplest formula calculation? Find the empirical formula of Zinc Sulfide. My

  95. chemistry

    why is the molecular formula of oide of arsenic in its gaseous state is not neccessarialy the same as its empirical formula what does this mean and how do i do it Molecules are known to dimerize or trimerize. We actually don't know what the molecular

  96. Science Chemistry

    The elementary analysis of 22 g hydrocarbon sample results in 18 g C and 4 g H. a) Choose the correct chemical formula of the hydrocarbon: i) CH4 ii) C2H4 iii) C3H8 b) What is the amount of CO2 in grams formed by the total combustion of hydrocarbon? Assume

  97. Chemistry

    10cm^3 of aa hydrocarbon was completely combusted in 200cm^3 of O2. It was found that there was 20cm^3 of O2 remaining and the volume of CO2 produced was 120cm^3. Determine the formula of the hydrocarbon.

  98. Chemistry

    10cm^3 of aa hydrocarbon was completely combusted in 200cm^3 of O2. It was found that there was 20cm^3 of O2 remaining and the volume of CO2 produced was 120cm^3. Determine the formula of the hydrocarbon.

  99. Science

    10. ALTERNATIVE B The elementary analysis of 22 g hydrocarbon sample results in 18 g C and 4 g H. a) Choose the correct chemical formula of the hydrocarbon: i) CH4 ii) C2H4 iii) C3H8 b) What is the amount of CO2 in grams formed by the total combustion of

  100. AP Chemistry

    Could you please review my work and see what i'm doing incorrectly? Thank you Given this information: CxHyOz (s) + O2 (g) ----> CO2 + H20 given: 2.165 g of the unknown hydrocarbon v = 1.868 L P = 130.2 kPa T = 65.0 degrees C g of H2O = 1.818 a)find g H in

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