The empirical formula for Brilliant Blie dye is C37 H34 N2 O9 S3 Na2, and the formula weight is 792.86 g/mol. How would you prepare a 4.73 X 10^-6 M solution of Brilliant Blue dye? How many grams of the

11,379 results
  1. Chemistry

    A compound with the empirical formula CH2O has a molar mass of approximately 90 g/mol. What is its molecular formula?

  2. Chemistry

    the formula H2O2 is an example of 1.molecular formula 2. an empirical formula 3.an ionic formula 4.an organic formula

  3. Chemistry

    What is the molecular formula of a molecule that has an empirical formula of CH2O and a molar mass of 120.12g/mol?

  4. Chemistry

    A compound with an empirical formula of C 2H 4Br has a molar mass of 215.90 g/mol. What is the molecular formula?

  5. Chemistry re-post URGENT

    Chemical analysis reveals capsaicin to contain 71.0% of carbon, 8.60% hydrogen, 15.8% oxygen and 4.60% nitrogen. a) Determine the empirical formula of capsaicin b) Each molecule contains one atom of nitrogen. What is the molecular formula of capsaicin? I

  6. 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

  7. Chemistry

    Is this done right? White phosphorous, P4, spontaneously bursts into flame in Oxygen gas. if 6.5 g of white phosphorous reacts completely with oxygen to form 11.54g of a phosphorous oxide, what is the empirical formula of this oxide? this is what i did:

  8. 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

  9. 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

  10. Chemistry

    Prior to their phaseout in the 1980s, chemicals containing lead were commonly added to gasoline as anti-knocking agents. A 3.279 g sample of one such additive containing only lead, carbon, and hydrogen was burned in an oxygen rich environment. The products

  11. chemistry

    f a compound has an empirical formula of C2HCl what is the molecular formula if the molar mass is 179 g/mol?

  12. 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

  13. 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

  14. AP Chemistry

    The structural formula for acetic acid is CH3CO2H. What is its empirical formula; what is its molecular formula?

  15. chemistry

    Water is added to 4.267 grams of UF6. The only products are 3.730 grams of a solid containing only uranium, oxygen and fluorine and 0.970 gram of gas. The gas is 95.0% flourine, and the remainder is hydrogen. From data determine the empirical formula of

  16. 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

  17. Math

    To determine whether a pancreas is functioning normally, a tracer dye is injected. A normally functioning pancrease secretes 4% of the dye each minute. A doctor injects 0.5g of the dye, and checks twenty minutes later. He finds that 0.35g of the dye

  18. Chemistry

    A student calculates the empirical formula of a compound to be C1.5H3.5. Express this as a correct empirical formula.

  19. chemistry

    In the course of research, a chemist isolates a new compound with an empirical formula C3H3O2. 4.97 g of the compound when dissolved in 100. g of water produces a solution with a freezing point of −0.325°C. What is the molecular formula of the compound?

  20. 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

  21. 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

  22. Chemistry

    If the empirical formula of a compound is CH2 and its molar mass is 70.0, then what is its molecular formula?

  23. 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.

  24. 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

  25. Chemistry

    Chemical analysis reveals capsaicin to contain 71.0% of carbon, 8.60% hydrogen, 15.8% oxygen and 4.60% nitrogen. a) Determine the empirical formula of capsaicin b) Each molecule contains one atom of nitrogen. What is the molecular formula of capsaicin? I

  26. Chemistry

    Carminic acid,a naturally occuring red pigment extracted from the cochineal insect, contains only C,H,and O. It was commonly used as a dye in the first half of the nineteenth century. It is 53.66% C and 4.09% H by mass. A titration of the 0.3602 g sample

  27. 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

  28. chemistry

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

  29. chemistry

    "empirical formulas" combustion of a 0.255g compound conatining only C,H and O, yields 0.561g CO2 and 0.306g H2O. what is the empirical formula of the compound?

  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. 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

  32. 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

  33. 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

  34. 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.

  35. 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.

  36. College Chemistry Lab

    Suppose that a 2.50x10^-6M solution of red dye No. 2 had an absorbance of 0.585 at its wavelength of maximum absorbance. A second solution of red dye No. 2 is too concentrated to read its absorbance so 5.00 mL of the concentrated dye solution was diluted

  37. Chemistry

    Water is added to 4.267 grams of UF6. The only products are 3.730 grams of a solid containing only uranium, oxygen and fluorine and 0.970 gram of gas. The gas is 95.0% flourine, and the remainder is hydrogen. From data determine the empirical formula of

  38. chemistry

    why is the formula written for an ionic compound such as NaCl the empirical formula,rather than a molecular formula?

  39. Chemistry

    calculate the empirical formula. A chemist heats 50.00g of sulfur under controlled conditions to produce a sulfer-oxygen compund.The mass of the sulfur-oxygen compound is 100.00g. What is the empirical formula of the sulfur-oxygen?

  40. st.joseph science

    Calculate the molecular formula of a compound whose empirical formula is CH2O AND vapour density is 30

  41. chemestry

    What is the molecular formula for the folowwing compound? Empirical Formula: C3H6O2 (M=74.08 g/mol)

  42. 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

  43. Chemistry

    The empirical formula for Brilliant Blie dye is C37 H34 N2 O9 S3 Na2, and the formula weight is 792.86 g/mol. How would you prepare a 4.73 X 10^-6 M solution of Brilliant Blue dye? How many grams of the dye do you need to add to a 1.00 L of water to make

  44. Chemistry

    The empirical formula for the Brilliant Blue dye is: C37H34N2O9S3Na2 and the formula weight are 792.86g/mol. How would you prepare a 5.25 x 10-6 M solution of Brilliant Blue dye. How many grams of the dye you need to add to a 1.00 L of water to make this

  45. math problem

    To make an orange dye, 4 parts of red dye are mixed with 3 parts of yellow dye. To make a green dye, 2 parts of blue dye are mixed with 1 part of yellow dye. If equal amounts of green dye and orange dye are mixed,___________ of this mixture is composed of

  46. 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.

  47. 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?

  48. 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?

  49. 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.

  50. 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

  51. 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

  52. 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

  53. 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

  54. 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

  55. 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

  56. 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

  57. Math

    Max creates a lavender dye by mixing 3 parts of red dye. Will a mixture of 14 parts of blue dye with 23 parts of red dye create the same shade of lavender?

  58. Chemistry

    a)Would you expect the empirical formula you determine for magnesium oxide to be the same as the one determined by another student? b) Would you expectan empirical formulato be the same even though different masses of Mg were used? Briefly explain. c) If

  59. chemistry

    for our lab, we are given the molarity of ClO-. We are then supposed to use beer's law to determine the molarity of the dye that was used to make the solution with. For the dye, use the first absorbance value, Ao, and calculate the initial concentration of

  60. chemistry

    can a compound's empirical and molecular formulas be the same?Explain who cares? Yes, they can. CH4 is methane. That is the empirical formula as well as the molecular formula.

  61. Algebra

    You go to the doctor and he gives you 13 milligrams of radioactive dye. After 20 minutes, 4.5 milligrams of dye remain in your system. To leave the doctor's office, you must pass through a radiation detector without sounding the alarm. If the detector will

  62. 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

  63. 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

  64. 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:

  65. Chemistry

    I found the empirical but i don't know how to get the empirical formula for NH2. can anyone help?

  66. 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

  67. rate laws and concentrations :: Chemistry.

    A student studied the kinetics of the reaction of sodium hypochlorite and a vegetable dye by the method of pseudo order. He mixed 5 mL of a 0.67 M solution of NaOCl with 15 mL of a vegetable dye, he took a portion of the mixture and absorbance was measured

  68. Chemistry

    The question says: when .422 g of phosphorus is burned, .967 g of a white oxide is obtained. Determine the empirical formula of the oxide. I did the calculations and got that there would be 1 mole Phosphorus and 4.29 mol Oxygen. To get the empirical

  69. 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

  70. astronomy

    You find a piece of cloth painted with organic dye. By analyzing the dye, you find that only 83 % of the carbon-14 originally in the dye remains. When was the cloth painted?

  71. Chemistry

    A student measures k for a certain blue dye to be 19.4 M^-1 at 560 nm. What is the molarity of the dye in a solution with an absorbance of 0.118 at this wavelength?

  72. chemistry

    You need to make a 300 ml of a .37M Na2 SO4 solution. How much Na2 So4 should you weigh out?

  73. Chemistry :(

    hello, i would be glad if someone answer to my question fast please as i am having a class test tomorrow. So here's the question: Q:An Alkaline with 16 carbons has a molecular formula of: (a)C16 H16 (b)C16 H34 (c)C16 H8 (d)C16 H32 (e)C16 H48 please tell me

  74. Chemistry

    This problem involves a molecular compound so both empirical and molecular formulas are required. A compound composed of Carbon, Hydrogen, and Bromine is analyzed. It is found to contain 0.3194 g of C, 0.05361 g of H and 2.125 g Br. What is the empirical

  75. Stoichiometry Test

    3.Empirical formula is C4H5N2O.Its molecular weight is 194.19g/mole.The "empirical formula weight is about 97.1g/mole.What is the molecular formula ?

  76. 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?

  77. Chemistry

    If one wanted to a make a 500.0 mL of 4.5 x 10-6M solution of this red dye, how many grams would they need to weigh out? The molar mass of the dye is 492 g/mol. SHOW WORK.

  78. 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.

  79. Chemistry

    A standard of red dye was prepared in the following manner: 4.5mL of 0.100M of food dye was added to a test tube and 5.5mL of water was added. What was the final concentration of food dye in the test tube?

  80. Chemistry

    If I have 0.17g of Mg and 0.10g of O, and I am asked to find the empirical formula for magnesium oxide, is the following the right way to go about it? Convert g-> mol 0.17g=0.01mol Mg 0.10g=0.01mol O Divide by smallest mole amt. (0.01mol) 0.01mol/0.01mol=1

  81. Chemistry

    Prior to their phaseout in the 1980s, chemicals containing lead were commonly added to gasoline as anti-knocking agents. A 3.279 g sample of one such additive containing only lead, carbon, and hydrogen was burned in an oxygen rich environment. The products

  82. Chemistry

    Prior to their phaseout in the 1980s, chemicals containing lead were commonly added to gasoline as anti-knocking agents. A 3.279 g sample of one such additive containing only lead, carbon, and hydrogen was burned in an oxygen rich environment. The products

  83. chemistry

    I need to know if I have th right molecular formula for Sorbito 39.56g C 7.75g H 52.7g O Empirical Formula is CH2O 30.026 amu how I how calculate the molecular mass and how I figure out the melecular formula? please help

  84. Chemistry

    A student mixes 450 mL of water and 116 mL of 7.90 x 10-5 M greenfood dye solution. What is the concentration of this new dilute solution of green food dye?

  85. Chemistry

    A student mixes 675 mL of water and 256 mL of 3.30 x 10-5 M orangefood dye solution. What is the concentration of this new dilute solution of orange food dye?

  86. Chemistry

    In my experiment I heated some oxide of tin, in order to figure out its empirical formula. How would the empirical formula be affected if the oxide was not heated to dryness? Also If some oxide splattered out of the container, how would this affect the

  87. chemistry

    How do I determine the molecular formula of a gas? It depends on what information you have. I have the empirical formula and chemical composition of the oxide. I also have the volume of the gas. I have the empirical formula and chemical composition of the

  88. 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

  89. Chemistry

    A dye has a λmax = 460 nm (ε = 70,000 L/(mol*cm)). What is the concentration of dye in a sample whose absorbance at 460 nm is A = 0.350 in a cell with a path length of 1.00 cm (4 points) I have no idea how to do this.

  90. 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

  91. Chem.

    in the equation Ba(NO3)2(aq)+Na2SO4 (aq) →BaSO4(s) + Na2(NO3)2 .......is Na2(NO3)2 aqueous?

  92. Chemistry

    A buret (initial and final buret reading were 2.20 mL and 11.86 mL) was used to deliver a sample of 2.1E-5 M stock dye into a 25.0 mL volumetric flask. The dye was then diluted with water to exactly 25.0 mL. Calculate the molarity of the resulting

  93. chemistry

    3. Find the empirical formula for a compound that consists of aluminum and chlorine in which the aluminum is 20.2 % by mass. 4. A sample contains 71.65% CL, 24.27% C nad 4.07% H. the molecular weight is known to be 98.96 g/mol. What are the empirical and

  94. 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

  95. Biology

    A drop of two dyes, A and B were placed on the surface of gelatin in two test tubes. After 24 hours dye A and B had traveled 2.7 and 1.8 cm below the surface of the gel in their respective tubes. Calculate the diffusion rates. Why dye has a larger

  96. 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

  97. Chemistry

    the empirical formula of a given compound is C H O and its relative density is 44. determine its molecular formula.

  98. Chemistry

    How can i determine the molar mass of acetylene and its molecular formula if i only know its density at stp and its empirical formula

  99. Chemistry

    A hydrogen has an empirical formula CH and a vapour density of 39.Determine its molecular formula,show workings.

  100. chemistry

    The formula of benzine and organic solvent is C6 H6. what is the empirical formula express the mass of a mole of materials in gram

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