1. Questions

chemistry

When 1.24g of an organic compound with the formula CxHyOz is burned in excess oxygen, 1.76g of carbon dioxide and 1.08g of water vapor are obtained. What is the empirical formula of the compound?



Determine the moles of CO2 in 1.76grams, that will give you the moles of C in the original compound.

Determine the moles of H2O in 1.08 grams, that will give you the moles of H2, double it, and you have the number of moles in the original compound.

Add the weight of the moles of C in the original compouond to the weight of moles of H in the orig compound, then subtract that weight from 1.24g. The remainder is the weight of O in the compound, now calculate the moles of O in that.

You have the moles of C, H, and O in the original compound.

Take the smaller of those three numbers, and divide into all three. The numbers you get will be the mole ratio.

For instance, assume you had these numbers....C .0024 moles, H .0050 moles, and O .0025 moles.

C is the lower number, dividing, we get
CH2O

  1. 👍
  2. 👎
  3. 👁
kevin

  1. Ghhhh

    1. 👍
    2. 👎
    Anonymous

Respond to this Question

First Name

Your Response

Similar Questions

  1. CHEM

    A 0.4647-g sample of a compound known to contain only carbon, hydrogen, and oxygen was burned in oxygen to yield 0.8635 g of CO2 and 0.1767 g of H2O. What is the empirical formula of the compound? i got C3H3O2 IS IT RIGHT?

  2. Chemistry

    Consider the following reaction: CH4 +2O2 -> CO2 + 2H2O. Delta H = -891 kJ Calculate the enthalpy change for each of the following cases: a. 1.00 g methane is burned in excess oxygen b. 1.00 x 10^3 L methane gas at 740. torr and

  3. Chemistry

    A- 50.0 g of H2SO4 react with 75.0 g of NaOH. Identify the limiting and excess reactants. How many grams of Na2SO4 will be formed? B- A chemist burns 160.0 g of aluminum in 200.0 g of oxygen. She produces 275.0 g of aluminum

  4. chemistry

    Fumaric acid, which occurs in many plants, contains, by mass, 41.4% carbon, 3.47% hydrogen, and 55.1% oxygen. A 0.050-mol sample of this compound weighs 5.80 g. The molecular formula of this compound is can you show me the formula

  1. Stoichiometry

    4. Vitamin C, M= 176.12 g/mol, is a compound of composed of carbon, hydrogen, and oxygen. Vitamin C is found in many natural sources especially citrus fruits. When a 1.000-g sample of vitamin C is burned in a combustion apparatus

  2. General Chemistry

    An unknown compound has a formula of CxHyOz. You burn 0.1523 g of the compound and isolate 0.3718 g of CO2, and 0.1522 g of H2O. What is the empirical formula of the compound? If the molar mass is 72.1 g/mol what is the molecular

  3. Chemistry

    A 0.100g sample of a compound containing C, H, and O is burned oxygen producing 0.1783 g of CO2 and 0.0734 g of H2O. Determine the empirical formula of the compound.

  4. Chemistry

    When 0.340 mol of butane, C4H10, are burned with excess oxygen giving CO2 and H2O, how many moles of oxygen are consumed?

  1. Cemistry

    When a 0.952 g sample of an organic compound containing C, H,and O is burned completely in oxygen, 1.35 g of CO2 and0.826 g of H2O are produced. What is the empiricalformula of the compound?

  2. Chemistry

    A 2.52g sample of a compound containing only carbon, hydrogen, nitrogen, oxygen, and sulfur was burned in excess O to yield 4.36g of CO2 and 0.892g of H20. Another sample of the same compound of mass 4.14g, yielded g of SO3. A

  3. Chemistry

    An organic compound x contains 40% carbon, 6.7% hydrogen the third compound oxygen. If the relative molecular mass of the compound is 60, calculate (i) the empirical formular of x (ii) the molecular formular of x

  4. AS ORGANIC CHEM

    An organic compound, X, will react with an excess of calcium metal to produce a salt with the empirical formula CaC4H6O4. What could be the identity of X? 1 ethanoic acid 2 butanedioic acid 3 methylpropanedioic acid With

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