2. Atoms & Elements

Law of Multiple Proportions

Law of Multiple Proportions Chemistry Made Easy with Practice Examples

Multiple Proportions

Ch 1.5  Law of Multiple proportions, Daltons Atomic Theory

The ratio of oxygen to carbon by mass in carbon monoxide is
1.33:1.00. Find the formula of an oxide of carbon in which the
ratio by mass of oxygen to carbon is 2.00:1.00.

According to Law of Multiple Proportions, ratio of both mass ratios will give a whole number.

Who Discovered the Law of Multiple Proportions in Chemistry? : Chemistry & Physics

In a series of experiments, a chemist prepared three different 
compounds that contain only iodine and fluorine and determined 
the mass of each element in each compound: 
Compound Mass of Iodine (g) Mass of Fluorine (g) 
1 4.75 3.56 
2 7.64 3.43 
3 9.41 9.86 
(b) How do the numbers in part (a) support the 
atomic theory?

The atomic weight of carbon (12.011) is approximately 12 times that of hydrogen (1.008).
(a) Show how you can use this knowledge to calculate pos-sible formulas for benzene, ethane, and ethylene (Prob-lem 2.82).

In methane, one part hydrogen combines with three parts carbon by mass. If a sample of a compound containing only carbon and hydrogen contains 32.0 g of carbon and 8.0 g of hydrogen, could the sample be methane? If the sample is not methane, show that the law of multiple proportions is fol-lowed for methane and this other substance.

Benzene, ethane, and ethylene are just three of a large num-ber of hydrocarbons—compounds that contain only carbon and hydrogen. Show how the following data are consistent with the law of multiple proportions.

The ratio of 2.0 g of hydrogen to 16 g of oxygen simplifies to 8.

The law of multiple proportions compares two compounds.

The ratio of 2.0 g of hydrogen to 32 g of oxygen simplifies to 16.

If 4 g of hydrogen had been used to form water, 32 g of oxygen would be needed.

Correct, the ratio is a small whole number.

In this example, the law of multiple proportions is not obeyed.

The law of multiple proportions is obeyed for these two compounds.

 When two elements (call them A and B) form two different compounds, the mass of element B that combines with 1 g of element A can be expressed as a ratio of small whole numbers. 

2.0 g of hydrogen combine with 16 g of oxygen to form water and 2.0 g of hydrogen combine with 32 g of oxygen to form hydrogen peroxide.  Which of the following is an expression of the law of multiple proportions?

In a series of experiments, a chemist prepared three different
compounds that contain only iodine and fluorine and determined
the mass of each element in each compound:
Compound Mass of Iodine (g) Mass of Fluorine (g)
1 4.75 3.56
2 7.64 3.43
3 9.41 9.86
(a) Calculate the mass of fluorine per gram of iodine in Compound 3.

Sodium reacts with oxygen in air to form two compounds:
sodium oxide and sodium peroxide. In forming sodium oxide,
23.0 g of sodium combines with 8.0 g of hydrogen. In forming
sodium peroxide, 23.0 g of sodium combines with 16.0 g
of oxygen. (b) What fundamental law does this experiment
demonstrate?

Sulfur and fluorine form several different compounds including
sulfur hexafluoride and sulfur tetrafluoride. Decomposition of a
sample of sulfur hexafluoride produces 4.45 g of fluorine and
1.25 g of sulfur, while decomposition of a sample of sulfur tetrafluoride
produces 4.43 g of fluorine and 1.87 g of sulfur. Calculate
the mass of fluorine per gram of sulfur for each sample and
show that these results are consistent with the law of multiple
proportions.

Palladium forms three different compounds with sulfur. The
mass of sulfur per gram of palladium in each compound is listed
here. Show that these masses are consistent with the law of
multiple
proportions.
Compound Grams S per Gram Pd
A 0.603
B 0.301
C 0.151

Sulfur and oxygen form both sulfur dioxide and sulfur trioxide.
When samples of these are decomposed, the sulfur dioxide
produces 3.49 g oxygen and 3.50 g sulfur, while the sulfur trioxide
produces 6.75 g oxygen and 4.50 g sulfur. Calculate the mass
of oxygen per gram of sulfur for each sample and show that
these results are consistent with the law of multiple proportions.

What is the law of multiple proportions, and how does Dalton’s atomic theory account for it?

Law of: Definite Proportions vs Multiple Proportions vs Conservation of Mass

In a series of experiments, a chemist prepared three different
compounds that contain only iodine and fluorine and determined
the mass of each element in each compound:
Compound Mass of Iodine (g) Mass of Fluorine (g)
1 4.75 3.56
2 7.64 3.43
3 9.41 9.86
(a) Calculate the mass of fluorine per gram of iodine in Compound 2.

Ammonia (NH3) and hydrazine (N2H4) are both compounds of nitrogen and hydrogen. Based on the law of multiple pro-portions, how many grams of hydrogen would you expect 2.34 g of nitrogen to combine with to yield ammonia? To yield hydrazine?

The ratio of sulfur to oxygen by mass in SO2 is 1.0:1.0.
a. Find the ratio of sulfur to oxygen by mass in SO3.
b. Find the ratio of sulfur to oxygen by mass in S2O.

Two different compounds containing osmium and oxygen have
the following masses of oxygen per gram of osmium: 0.168 and
0.3369 g. Show that these amounts are consistent with the law
of multiple proportions.

A compound containing sulfur and fluorine contains 8.00 g of S and 9.50 g of F. Which combination of S and F masses represents a different compound that obeys the Law of Mul-tiple Proportions? (LO 2.8) 
(a) 32.0 g of S and 38.0 g of F 
(b) 4.00 g of S and 4.75 g of F 
(c) 8.00 g of S and 10.5 g of F 
(d) 16.0 g of S and 57.0 g of F

The ratio of the mass of a nitrogen atom to the mass of an atom
of 12C is 7:6, and the ratio of the mass of nitrogen to oxygen in
N2O is 7:4. Find the mass of 1 mol of oxygen atoms.

Chemistry 5.8b Law of Multiple Proportions

In borane, one part hydrogen combines with 3.6 parts boron by mass. A compound containing only hydrogen and boron contains 6.0 g of hydrogen and 43.2 g of boron. Could this compound be borane? If it is not borane, show that the law of multiple proportions is followed for borane and this other substance.

A 1.0-g sample of carbon dioxide (CO2) is fully decomposed
into its elements, yielding 0.273 g of carbon and 0.727 g of
oxygen. (b) If a sample of a different compound decomposes into 0.429 g of
carbon and 0.571 g of oxygen, what is its ratio of the mass of
O to C?

Two compounds containing carbon and oxygen have the following percent composition by mass. Compound 1: 42.9% carbon and 57.1% oxygen Compound 2: 27.3% carbon and 72.7% oxygen Show that the law of multiple proportions is followed. If the formula of the first compound is CO, what is the formula of the second compound?

Law of Definite Proportions - Law of multiple proportions

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Ions

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Periodic Table: Charges

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Law of Definite Proportions

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Periodic Table: Element Symbols

The Element Symbols of the Periodic Table represent the abbreviated form of an element