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Chapter 3: Problem 164

Arrange the following substances in order of increasing mass percent of nitrogen. $\begin{array}{ll}{\text { a. } \mathrm{NO}} & {\text { c. } \mathrm{NH}_{3}} \\\ {\text { b. } \mathrm{N}_{2} \mathrm{O}} & {\text { d. SNH }}\end{array}$

Short Answer

Expert verified
The correct order of the substances in increasing mass percent of nitrogen is: SNH (29.79%), NO (46.67%), N2O (63.64%), NH3 (82.35%).

Step by step solution

01

Calculate the molar mass of each compound

To find the mass percentage of nitrogen in each compound, we must first calculate the molar mass of each compound using the atomic masses of the elements (Nitrogen, Oxygen, and Sulfur). Nitrogen (N): 14 g/mol Oxygen (O): 16 g/mol Sulfur (S): 32 g/mol For each compound: 1. NO: Molar mass = 14 (N) + 16 (O) = 30 g/mol 2. N2O: Molar mass = 14x2 (N) + 16 (O) = 44 g/mol 3. NH3: Molar mass = 14 (N) + 3x1 (H) = 17 g/mol 4. SNH: Molar mass = 32 (S) + 14 (N) + 1 (H) = 47 g/mol
02

Calculate mass percentage of nitrogen in each compound

Now we can calculate the mass percentage of nitrogen in each compound: 1. NO: Mass % of N = \(\frac{14}{30}\) x 100 = 46.67% 2. N2O: Mass % of N = \(\frac{28}{44}\) x 100 = 63.64% 3. NH3: Mass % of N = \(\frac{14}{17}\) x 100 = 82.35% 4. SNH: Mass % of N = \(\frac{14}{47}\) x 100 = 29.79%
03

Arrange the compounds in increasing order of nitrogen mass percent

Now that we have found the mass percentage of nitrogen in each compound, we can arrange them in increasing order: 1. SNH: 29.79% 2. NO: 46.67% 3. N2O: 63.64% 4. NH3: 82.35% So, the correct order of the substances in increasing mass percent of nitrogen is: SNH, NO, N2O, NH3.

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Most popular questions from this chapter

Which of the following statements about chemical equations is(are) true? a. When balancing a chemical equation, you can never change the coefficient in front of any chemical formula. b. The coefficients in a balanced chemical equation refer to the number of grams of reactants and products. c. In a chemical equation, the reactants are on the right and the products are on the left. d. When balancing a chemical equation, you can never change the subscripts of any chemical formula. e. In chemical reactions, matter is neither created nor destroyed so a chemical equation must have the same number of atoms on both sides of the equation.

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