Chemistry · Laws of chemical combination, Atomic and molecular masses
Compound and are two oxides of sulfur. Compound A is 50\% sulfur by mass, while
Compound \( A \) and \( B \) are two oxides of sulfur. Compound A is 50\% sulfur by mass, while Compound B is \( 40 \% \) sulfur by mass. Given the atomic masses of sulfur and oxygen are 32 amu and 16 am \( u \) respectively, which of the following statements is NOT a valid interpretation of these data? This question has multiple correct options
- A. Compound A could have the formula, \( S O_{2} \)
- B. Compound B could have the formula, \( S O_{2} \)
- C. Compound A and B illustrate Dalton's law of multiple proportions.
- D. Compound A could have the formula, \( S O \).
Step-by-step solution
Compound B is 40% sulfur by mass. For SO2, the sulfur mass percent is (32)/(32+32)=50%, not 40%. Therefore, B cannot be SO2.
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