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How does Dalton’s atomic theory account for the fact that when 1.000 g of water is decomposed into its elements, 0.111 g of hydrogen and 0.889 g of oxygen are obtained regardless of the source of the water?

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Patrina Schowalter
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24 May 2020

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Related questions

Hydrogen sulfide is composed of two elements: hydrogen and sulfur. In an experiment, 6.500 g of hydrogen sulfide is fully decomposed into its elements. (a) If 0.384 g of hydrogen is obtained in this experiment, how many grams of sulfur must be obtained? (b) What fundamental law does this experiment demonstrate? (c) How is this law explained by Dalton’s atomic theory?

Section 1-5 describes the postulates of Dalton’s atomic theory. With some modifications, these postulates hold up very well regarding how we view elements, compounds, and chemical reactions today. Answer the following questions concerning Dalton's atomic theory and the modifications made today.
 
a. The atom can be broken down into smaller parts. What are the smaller parts?
 
b. How are atoms of hydrogen identical to each other and how can they be different from each other?
 
c. How are atoms of hydrogen different from atoms of helium? How can H atoms be similar to He atoms?
 
d. How is water different from hydrogen peroxide (H2O2) even though both compounds are composed of only hydrogen and oxygen?
 
e. What happens in a chemical reaction and why is mass conserved in a chemical reaction?

Complete combustion of 12.34 g of a compound of carbon, hydrogen, and oxygen yielded 21.99 g CO2 and 9.005 g H2O. When 11.40 g of the compound was dissolved in 323 g of water, the freezing point of the solution was found to be -0.889 °C. For water, Kfp = 1.86 °C/m. What is the molecular formula of the compound?

  • Enter the elements in the order C, H, O
    molecular formula =

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