Analysis of a compound shows carbon hydrogen and nitrogen present. Each molecule contains one nitrogen atom. A 150. Mg sample of the compound produces 27.4 mg of NH3 in which all the nitrogen comes from the sample. Which of the following is the formula for the compound? A. CH3N B. C2H2n C. C4h11n D. C3h13n C. C6h2n
Convert 27.4 mg NH3 to mg N, then to percent N in the 150 mg sample.
Then calculate the percent N in each of the answers. The one that matches %N in the analysis is the one to pick (although I don't think the answer is an exact match).
To find the formula for the compound, we need to analyze the given information.
From the question, we know that the compound contains carbon (C), hydrogen (H), and nitrogen (N). Each molecule of the compound contains one nitrogen atom.
We are also given that a 150 mg sample of the compound produces 27.4 mg of NH3 (ammonia) where all the nitrogen comes from the sample.
Now, let's analyze the weights of carbon, hydrogen, and nitrogen in the compound.
1. Nitrogen: Since all the nitrogen in the compound comes from the sample and is converted into NH3, we can use the molecular weight of NH3 to calculate the amount of nitrogen present in the sample. The molecular weight of NH3 is 17.03 g/mol (approximately).
The weight of nitrogen in the 27.4 mg of NH3 can be calculated as:
weight of nitrogen = (27.4 mg / 17.03 g/mol) * (14.01 g/mol) = 22.27 mg
2. Carbon and hydrogen: To find the weights of carbon and hydrogen, we need to subtract the weight of nitrogen (22.27 mg) from the total weight of the sample (150 mg).
weight of carbon = 150 mg - 22.27 mg = 127.73 mg
weight of hydrogen = 150 mg - 22.27 mg = 127.73 mg
Now that we have the weights of carbon, hydrogen, and nitrogen, let's determine the empirical formula of the compound.
1. Divide each weight by the respective atomic weight to find the number of atoms:
Number of carbon atoms = 127.73 mg / (12.01 g/mol) = 10.63
Number of hydrogen atoms = 127.73 mg / (1.01 g/mol) = 126.46
Number of nitrogen atoms = 22.27 mg / (14.01 g/mol) ≈ 1.59
2. Divide each number of atoms by the smallest number to obtain a simplified whole number ratio:
Number of carbon atoms ≈ 10.63 / 1.59 ≈ 6.68 ≈ 7
Number of hydrogen atoms ≈ 126.46 / 1.59 ≈ 79.5 ≈ 80
Number of nitrogen atoms ≈ 1.59 / 1.59 = 1
The empirical formula of the compound is therefore C7H80N.
Based on the given options, it appears that none of them match the empirical formula obtained. Please double-check the options provided or review the calculations.