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?
1
views
3. Chemical Reactions
Empirical Formula
Multiple Choice
A 200.0 g sample of a compound contains 175.4 g of carbon and 24.54 g of hydrogen. What is the empirical formula of the compound?
A
C3H8
B
CH2
C
CH
D
C2H5
Verified step by step guidance1
Calculate the number of moles of carbon in the sample by dividing the mass of carbon by its molar mass: \( \text{moles of C} = \frac{175.4 \text{ g}}{12.01 \text{ g/mol}} \).
Calculate the number of moles of hydrogen in the sample by dividing the mass of hydrogen by its molar mass: \( \text{moles of H} = \frac{24.54 \text{ g}}{1.008 \text{ g/mol}} \).
Determine the simplest whole number ratio of moles of carbon to moles of hydrogen by dividing each by the smallest number of moles calculated in the previous steps.
If necessary, multiply the ratio by a whole number to obtain whole numbers for the subscripts in the empirical formula.
Write the empirical formula using the whole number ratio of moles of carbon to moles of hydrogen obtained in the previous step.
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