Open Question
What is the empirical formula of nitrogen chloride given that a 0.77 mg sample of nitrogen reacts with chlorine to form 6.61 mg of the chloride?
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3. Chemical Reactions
Empirical Formula
Multiple Choice
What is the empirical formula of the compound given the combustion data: 2.08 g CO₂, 1.28 g H₂O, and 4.77 g SO₃?
A
C₄H₁₀O₃NS
B
C₂H₅O₂NS
C
CH₄O₃NS
D
C₃H₈O₄NS
Verified step by step guidance1
Determine the moles of carbon in CO₂: Use the molar mass of CO₂ (44.01 g/mol) to convert the mass of CO₂ to moles. The formula is: \( \text{moles of C} = \frac{\text{mass of CO₂}}{\text{molar mass of CO₂}} \).
Determine the moles of hydrogen in H₂O: Use the molar mass of H₂O (18.02 g/mol) to convert the mass of H₂O to moles. Since each molecule of H₂O contains 2 hydrogen atoms, multiply the moles of H₂O by 2 to find the moles of hydrogen. The formula is: \( \text{moles of H} = 2 \times \frac{\text{mass of H₂O}}{\text{molar mass of H₂O}} \).
Determine the moles of sulfur in SO₃: Use the molar mass of SO₃ (80.06 g/mol) to convert the mass of SO₃ to moles. The formula is: \( \text{moles of S} = \frac{\text{mass of SO₃}}{\text{molar mass of SO₃}} \).
Assume the presence of one nitrogen atom in the compound, as nitrogen is not directly measured in the combustion analysis. Calculate the moles of oxygen by considering the total mass of the compound and subtracting the masses of C, H, S, and N (using their respective atomic masses and moles calculated).
Determine the simplest whole number ratio of moles of each element (C, H, O, N, S) by dividing each by the smallest number of moles calculated. This will give the empirical formula of the compound.
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