Consider two compounds. Compound A contains 15.7 g of sulfur and 18.6 of fluorine. Compound B contains 25.4 of sulfur and 60.2 g of flurine. A. What is the mass ratio of flurine to sulfur in Compound A. B. What is the mass ratio of fluorine to sulfur in Compound B. C. Using the law of definite proportions (also called the law of constant composition), could compound A and compound B be the same compound?

The following data were collected for several compounds of iron and oxygen:   Mass of iron that combines with 1 g of oxygen Compound A 3.49 g Compound B 2.33 g Compound C 2.62 g   Which calculations should be performed to illustrate the law of multiple proportions? Group of answer choices a. determine the ratio of the mass of iron combining for one compound by that for another compound b. determine the mass of iron combining with 1 g oxygen for each compound c. determine the ratio of iron and oxygen atoms for each compound d. convert the ratio into a whole number fraction

Match the term on the left box with the most appropriate definition on the right. 1 Empirical Formula A A compound with a specific number of water molecules bonded to each formula unit. 2 Mass Percent B This shows only the relative amounts of the elements, not the actual amounts. Atoms of an element are chemically similar but Chave different numbers of neutrons and, thus, different mass numbers. This represents an element in a compound is the D mass of the element expressed as a percentage of the total mass of the compound. E The study of mass-mole-number relationships in chemical reactions and formulas. F The reactant that runs out first following a chemical reaction. G The amount of substance contains as many elementary entities as exactly 12g of carbon-12. The law states that the elements in a chemical H compound are always present in the same proportions by mass. A compound that does not have any water I molecules bonded to it; applies to compounds that can be hydrated. J This…

On another planet, the isotopes of titanium have the given natural abundances. Abundance Mass (u) 74.200% 45.95263 15.100% 47.94795 10.700% 49.94479 Isotope 46 Ti 48 Ti 50 Ti What is the average atomic mass of titanium on that planet? average atomic mass= x10 TOOLS u

A 5.93 g sample of calcium sulfide was decomposed into its constituent elements, producing 3.30 g of calcium and 2.63 g of sulfur. Which of the statements are consistent with the law of constant composition (definite proportions)? Every sample of calcium sulfide will have 3.30 g of calcium. The ratio of calcium to sulfur will vary based on how the sample was prepared. The mass percentage of calcium plus the mass percentage of sulfur in every sample of calcium sulfide equals 100%. The mass ratio of S to Ca in every sample of calcium sulfide is 0.80. Every sample of calcium sulfide will have 55.6% mass of calcium.

A 12.6712.67 g sample of NaBr contains 22.3422.34% Na by mass. Considering the law of constant composition (definite proportions), how many grams of sodium does a 6.636.63 g sample of sodium bromide contain?

Consider two compounds. Compound A contains 2.77 g of 4 phosphorus and 9.53 g of chlorine. Compound B contains 11.9 g of phosphorus and 40.9 g of chlorine. What is the mass ratio of chlorine to phosphorus in Compound A?

A sample of Co weighs 77.2 grams. Will a sample of Sn that contains the same number of atoms weigh more or less than 77.2 grams? OA sample of Sn weighs less than 77.2 grams. OA sample of Sn weighs more than 77.2 grams. Calculate the mass of a sample of Sn that contains the same number of atoms. 9 Sn Mass =

Element C has three naturally occurring isotopes. The masses (amu) and % abundances of the isotopes are given in the table below. The average atomic mass of the element is ___amu?

Determine the number of atoms in 53.0 grams of bromine, Br. (The mass of one mole of bromine is 79.90 g.) atoms 1 3 6. C 7 8. 9. +/- х 100