1. Questions

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.?

  1. 👍
  2. 👎
  3. 👁
The orange baboon

  1. ...Y + O2 ==> CO2 + H2O
    ...................0.352 g + 0.18 g
    g C in Y is 0.352 x (12/44) = 0.096
    g H in Y is 0.18 x (2/18)) = 0.02

    mols C in Y = 0.096/12 = 0.008
    mols H in Y = 0.02/1 = 0.02
    Now find the ratio. The easy way is to divide both numbers by the smallest number; i.e.,
    C = 0.008/0.008 = 1
    H = 0.02/0.008 = 2.5
    Make whole numbers which will be C = 2 and H = 5 so the empirical formula is C2H5. The empirical formula will be (C2H5)x so x is a multiple of the empirical formula. The empirical formula is 29 so 29*what number = 58.
    The molecular formula is (C2H5)2 or C4H10. Is the molar mass 59?
    4*12 = 48 and 10*1 = 10
    48+10 = 58. Bingo.

    1. 👍
    2. 👎
    👤
    DrBob222

  2. Mega Thanks

    1. 👍
    2. 👎
    Olakunle

Respond to this Question

First Name

Your Response

Similar Questions

  1. chemistry

    A 15.27 g sample of Mo2O3(s) is converted completely to another molybdenum oxide by adding oxygen. The new oxide has a mass of 18.33 g. Add subscripts below to correctly identify the empirical formula of the new oxide.

  2. Chemistry

    Can someone answer this question? The enthalpy of combustion of solid carbon to form carbon dioxide is -393.7 kJ/mol carbon, and the enthalpy of combustion of carbon monoxide to form carbon dioxide is -283.3 kj/mol CO. Use these

  3. 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

  4. 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?

  1. Chemistry

    Complete combustion of a sample of a hydrocarbon in the presence of excess oxygen produces equal molar quantities of carbon dioxide and water. Which of the following could be the molecular formula of the compound? a. C4H4 b. C2H6

  2. 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

  3. 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

  4. chemistry

    In an experiment 3.10g of carbon, hydrogen and oxygen produced 4.4g of C02 and 2.7g of water on complete combustion. Determine the empirical formula of the compound ( C= 12, 0= 16, H =1)

  1. Chemistry

    A student made a determination of the empirical formula ot tungsten oxide (WO) produced by the total ignition of air of a smaple of metallic Tungsten. From the lab: Weight of crucible 11.120g weight of tungsten 8.820 weight of

  2. C hemistry

    An unknown compound contains only carbon, hydrogen, and oxygen . Combustion of 2.50 g of this compound produced 3.67 g of carbon dioxide and 1.50 g of water. What is the empirical formula of a substance that contains 8.33×10−2

  3. chem

    Combustion reactions involve reacting a substance with oxygen. When compounds containing carbon and hydrogen are combusted, carbon dioxide and water are the products. Using the enthalpies of combustion for C4H4 (-2341 kJ/mol),

  4. chem

    A sample of carbon,3.0g, was burned to carbon dioxide in a copper calorimeter.The mass of the calorimeter was 1.5kg and the mass of water in the calorimeter was 2kg.The initial temperature was 20°c and the final temperature was

You can view more similar questions or ask a new question.