We’re being asked to determine the molecular formula of a compound containing only sulfur and nitrogen is 69.6% S by mass. This means we need to do the following steps:
Step 1: Calculate the mass and moles of S and N in the compound.
Step 2: Determine the lowest whole number ratio of S and N to get the empirical formula.
Step 3: Get the ratio of the molar mass and empirical mass to determine the molecular formula.
Step 1: The compound is composed of S and N and we’re only given the mass percent of S (69.6% S). Recall that the mass percentages of a compound must add up to 100%. This means:
100% = %mass S + %mass N
100% = 69.6% + % mass N
% mass N = 100% – 69.6%
% mass N = 30.4%
Recall that mass percent is given by:
A compound containing only sulfur and nitrogen is 69.6% S by mass; the molar mass is 184 g/mol. What are the empirical and molecular formulas of the compound?
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Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition practice problems.