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Balance the following equation: Н2 + N2. NH3

Balance the following equation: Н2 + N2. NH3

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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### Balancing Chemical Equations #### Balance the following equation: \[ \boxed{} H_2 + \boxed{} N_2 \rightarrow \boxed{} NH_3 \] **COUNT HOW MANY YOU HAVE ON EACH SIDE!!** To balance this chemical equation, adjust the coefficients (the numbers in the boxes) so that the number of each type of atom on the left-hand side of the equation is equal to the number on the right-hand side. This ensures the law of conservation of mass is upheld. In this equation: - H stands for Hydrogen. - N stands for Nitrogen. Start by counting the number of atoms of each element on both sides of the equation and then adjust the numbers in the boxes accordingly. 1. **Identify the number of each atom** in the reactants and products. For example, initially: - Hydrogen (H) atoms on the left: \(2 \times \) number in first box. - Hydrogen (H) atoms on the right: \(3 \times \) number in third box. - Nitrogen (N) atoms on the left: \(2 \times \) number in second box. - Nitrogen (N) atoms on the right: \(1 \times \) number in third box. 2. **Balance the equation** by ensuring the number of atoms of each element is the same on both sides. Adjust the coefficients in the boxes as needed. Remember, balancing equations often requires trial and error. It is sometimes easier to start with the most complex molecule. ### Example: If we start with the simplest coefficients: \[ 3 H_2 + 1 N_2 \rightarrow 2 NH_3 \] Results in: - Left side: 6 Hydrogens (3 \(\times\) 2) and 2 Nitrogens. - Right side: 6 Hydrogens (2 \(\times\) 3) and 2 Nitrogens. The equation is now balanced! Keep counting and adjusting until both sides have equal numbers of each type of atom.
Transcribed Image Text:### Balancing Chemical Equations #### Balance the following equation: \[ \boxed{} H_2 + \boxed{} N_2 \rightarrow \boxed{} NH_3 \] **COUNT HOW MANY YOU HAVE ON EACH SIDE!!** To balance this chemical equation, adjust the coefficients (the numbers in the boxes) so that the number of each type of atom on the left-hand side of the equation is equal to the number on the right-hand side. This ensures the law of conservation of mass is upheld. In this equation: - H stands for Hydrogen. - N stands for Nitrogen. Start by counting the number of atoms of each element on both sides of the equation and then adjust the numbers in the boxes accordingly. 1. **Identify the number of each atom** in the reactants and products. For example, initially: - Hydrogen (H) atoms on the left: \(2 \times \) number in first box. - Hydrogen (H) atoms on the right: \(3 \times \) number in third box. - Nitrogen (N) atoms on the left: \(2 \times \) number in second box. - Nitrogen (N) atoms on the right: \(1 \times \) number in third box. 2. **Balance the equation** by ensuring the number of atoms of each element is the same on both sides. Adjust the coefficients in the boxes as needed. Remember, balancing equations often requires trial and error. It is sometimes easier to start with the most complex molecule. ### Example: If we start with the simplest coefficients: \[ 3 H_2 + 1 N_2 \rightarrow 2 NH_3 \] Results in: - Left side: 6 Hydrogens (3 \(\times\) 2) and 2 Nitrogens. - Right side: 6 Hydrogens (2 \(\times\) 3) and 2 Nitrogens. The equation is now balanced! Keep counting and adjusting until both sides have equal numbers of each type of atom.
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