A student believes that a sample of RbCl may be contaminated with CsCl(s). Knowing that pure RbCl(s) contains 29% chlorine by mass, the student performs and experiment to determine the mass percent of chlorine in the sample of RbCl(s).
Which of the following results for the mass percent would best support the student's claim that the sample of RbCl(s) is contaminated with CsCl(s)?
Answer choices:
A: 37% chlorine by mass
B: 29% chlorine by mass
C: 23% chlorine by mass
D: 52% chlorine by mass
Answers
Answered by
2
Answer:
23/ chlorine by mass
option c
Answered by
0
Answer:
23% chlorine by mass
Explanation:
Based on the chemical formulas and molar masses of the two compounds, we know that CsCl contains less chlorine by mass than RbCl
This means that if the student’s sample of RbCl were contaminated with CsCl, the mass percent of chlorine in the sample would be lower than the mass percent of chlorine in pure RbCl, which is 29%.
So, the result that would best support the student’s claim is 23% chlorine by mass.
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