A chemist decomposes several samples of water into hydrogen and oxygen and weighs or more correctly measures the mass of the hydrogen and the oxygen obtained. The results are as follows sample 1 has 1.5grams of hydrogen and 12grams of oxygen sample 2 has 2grams of hydrogen and 16 grams of oxygen sample 3 has 2.5grams and 20 grams of oxygen a. Can you summarize these observations in a short statement? Next, the chemist decomposes several samples of carbon dioxide into carbon and oxygen. The results are as follows: sample 1 has 0.5grams of carbon and 1.3grams of oxygen sample 2 has 1.0grams of carbon and 2.7grams of oxygen sample 3 has 1.5grams of carbon and 4.0grams of oxygen
b. Summarize these observations in a short statement?
c. Formulate a law from the observations in (a) and (b)?
d. Formulate a theory that might explain your law in (c)?

A. Hydrogen and oxygen combines in a constant mole ratio in all the three water samples

B. Carbon and oxygen are combined in a constant mole ratio in all the three samples of carbon dioxide

C. All pure samples of a compound contain the same elements combined in the same proportion by mass

D. Since the same elements are always combining to form a certain compound, and the atoms of each element has its own mass, the atoms of each element combining to form the compound do so in a fixed proportion by mass.

Explanation:

A. molar mass of hydrogen = 1.0 g/mol; molar mass of oxygen = 16 g/mol

The molar ratio of elements in a compound gives the proportion each element is combined with the other by mass.

molar ratio of hydrogen to oxygen in the samples:

Sample 1: Hydrogen; 1.5/1 = 1.5: Oxygen; 12/16 = 0.75

molar ratio = 1.5/0.75 = 2 : 0.75./0.75 = 1

molar ratio = 2:1

Sample 2: Hydrogen; 2/1 = 2: Oxygen; 16/16 = 1

molar ratio = 2/1 = 2 : 1/1 = 1

molar ratio = 2:1

Sample 3: Hydrogen; 2.5/1 = 2.5: Oxygen; 20/16 = 1.25

molar ratio = 2.5/1.25 = 2 : 1.25/1.25 = 1

molar ratio = 2:1

Hydrogen and oxygen combines in a constant mole ratio in all the three water samples

B. molar mass of carbon = 12 g/mol; molar mass of oxygen = 16 g/mol

molar ratio of carbon to oxygen in the samples:

Sample 1: Carbon; 0.5/12 = 0.04 : Oxygen; 1.3/16 = 0.08

molar ratio = 0.04/0.04 = 1 : 0.08/0.04 = 2

molar ratio = 1:2

Sample 2: Carbon; 1.0/12 = 0.083 : Oxygen; 2.7/16 = 0.168

molar ratio = 0.083/0.083 = 1 : 0.168/0.083 = 2

molar ratio = 1:2

Sample 3: Carbon; 1.5/12 = 0.125 : Oxygen; 4.0/16 = 0.250

molar ratio = 0.125/0.125 = 1: 0.250/0.125 = 2

molar ratio = 1:2

Carbon and oxygen are combined in a constant mole ratio in all the three samples of carbon dioxide

C. All pure samples of a compound contain the same elements combined in the same proportion by mass

D. Since the same elements are always combining to form a certain compound, and the atoms of each element has its own mass, the atoms of each element combining to form the compound do so in a fixed proportion by mass.

a

explanation:

the ideal gas law equation is as follows

pv = nrt

where p - pressure

v - volume

n - number of moles

r - universal gas constant

t - temperature

so if the pressure, volume and temperature are already known

we are left with n and r

since r is the universal gas constant that has a known fixed value then r too is known

so we are left with 'n'

once we know temperature volume and pressure

we can find the number of moles of gas present using the ideal gas law equation

this is not my own answer, this is an answer for the same question by the user blahblahmali. i do not claim ownership of this account.