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Chemical equations play a fundamental role in understanding and predicting chemical reactions. They provide a concise representation of the reactants and products involved in a reaction, allowing scientists to uncover the underlying principles and laws governing chemical changes. However, in order for chemical equations to accurately represent a chemical reaction, they must be balanced. Balancing chemical equations is a crucial skill in chemistry, where the number of atoms on the reactant side must equal the number of atoms on the product side. This ensures that the principle of conservation of mass is upheld. In this guide, we will explore the process of balancing chemical equations, providing step-by-step instructions and key tips to make the process easier and more efficient. Whether you are a student studying chemistry or just interested in understanding the basics of chemical reactions, this guide will equip you with the necessary tools to expertly balance any chemical equation.
This article was co-written by Bess Ruff, MA. Bess Ruff is a graduate student in geography at Florida. She received her Master’s degree in Environmental Science and Management from the Bren School of Environmental Science & Management, UC Santa Barbara in 2016. She has conducted survey work for marine spatial planning projects in the coastal area. Caribbean and support research as a contributor to the Sustainable Fisheries Group.
There are 7 references cited in this article that you can view at the bottom of the page.
This article has been viewed 477,141 times.
Are you looking to learn more about chemical equations? At first glance, chemical equations may seem confusing, but they are actually very simple when you know the basic steps and principles for balancing. Don’t worry – this article will help you with any problem, no matter how many atoms and molecules are in the equation. What about complex equations? Scroll down to the second section for a guide to help you deal with difficult equations through algebraic balance.
Steps
Balancing equations the traditional way
- C _{3} H _{8} + O _{2} –> H _{2} O + CO _{2}
- This reaction occurs when propane (C3H8) is burned in oxygen to produce water and carbon dioxide.
- For example, you have 3 oxygens on the right, but that’s because you add up the total.
- Left: 3 carbon (C3), 8 hydrogen (H8) and 2 oxygen (O2).
- Right: 1 carbon (C), 2 hydrogen (H2) and 3 oxygen (O + O2).
- You need to count the atoms again before balancing the hydrogen and oxygen, because you need to use the correlation coefficient to balance the other atoms in the equation.
- C _{3} H _{8} + O _{2} –> H _{2} O + 3 CO _{2}
- A coefficient of 3 before carbon on the right indicates 3 carbons, similarly, a subscript 3 on the left indicates 3 carbons.
- In a chemical equation, you can change the correlation coefficient, but you cannot change the subscript.
- C _{3} H _{8} + O _{2} –> 4 H _{2} O + 3CO _{2}
- On the right hand side, you have now added a factor of 4 because the lower number indicates you already have 2 hydrogen atoms.
- When you multiply the factor 4 by the subscript 2, you get 8.
- Add a factor of 5 to the oxygen molecule on the left side of the equation. You now have 10 oxygen atoms on each side.
- C _{3} H _{8} + 5 O _{2} –> 4H _{2} O + 3CO _{2} .
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- The carbon, hydrogen and oxygen atoms are balanced. You are done balancing the equation.
- You have 6 other oxygen atoms from 3CO _{2} .(3×2=6 oxygen atoms + 4 other atoms = 10).
Balancing Equations Algebraically
This method is also known as the Bottomley method, and is useful for complex reactions, but will take more time.
- PCl _{5} + H _{2} O –> H _{3} PO _{4} + HCl
- a PCl _{5} + b H _{2} O –> c H _{3} PO _{4} + d HCl
- a PCl _{5} + b H _{2} O –> c H _{3} PO _{4} + d HCl
- The left side has 2 b hydrogen atoms (2 for each H _{2} O molecule), and the right side has 3 c + d hydrogen atoms (3 for each H 3 PO _{4} molecule and 1 for each H _{3} PO 4 molecule). HCl molecule). Since the number of hydrogen atoms on both sides must be equal, 2 b must be equal to 3 c + d .
- Do this for each element.
- P: a = c
- Cl: 5 a = d
- H: 2 b = 3 c + d
- To solve equations quickly, you will set a value to a variable. For example a = 1. The next thing is to solve the equation to get the following values:
- Since P: a = c, then c = 1.
- Since Cl: 5a = d, d = 5
- Since H: 2b = 3c + d, b is calculated as:
- 2b = 3(1) + 5
- 2b = 3 + 5
- 2b = 8
- b=4
- You will have the following values:
- a = 1
- b = 4
- c = 1
- d = 5
- If the value you specify becomes a fraction, you simply multiply the entire correlation coefficient (including the factor 1) by the least common multiple of the denominator to make the value an integer. If there is only one fraction, you multiply the entire correlation coefficient by the numerator of the fraction.
- If the value you specified becomes the greatest common divisor, you will simplify the chemical equation by dividing each correlation coefficient (including the factor 1) by the greatest common divisor.
Advice
- If you’re having trouble, you can balance the equation with an online balancer. However, keep in mind that you can’t use an online equation balancer when taking the test, so don’t rely on it.
- Remember to simplify the equation! If the whole correlation coefficient is divisible by the same number, do this for the most minimalist result.
- To drop a fraction, you simply multiply the entire coefficient in the equation (left and right sides) by the fraction’s denominator.
Warning
- While balancing the equation, you will probably need the help of fractions, but the equation remains unbalanced as long as the coefficients are in the form of fractions. You cannot use half a molecule or half an atom in a chemical reaction.
This article was co-written by Bess Ruff, MA. Bess Ruff is a graduate student in geography at Florida. She received her Master’s degree in Environmental Science and Management from the Bren School of Environmental Science & Management, UC Santa Barbara in 2016. She has conducted survey work for marine spatial planning projects in the coastal area. Caribbean and support research as a contributor to the Sustainable Fisheries Group.
There are 7 references cited in this article that you can see at the bottom of the page.
This article has been viewed 477,141 times.
Are you looking to learn more about chemical equations? At first glance, chemical equations may seem confusing, but they are actually very simple when you know the basic steps and principles for balancing. Don’t worry – this article will help you with any problem, no matter how many atoms and molecules are in the equation. What about complex equations? Scroll down to the second section for a guide to help you deal with difficult equations through algebraic balance.
In conclusion, balancing chemical equations is an important skill in chemistry as it allows scientists to accurately represent the reactions that occur in a chemical system. By following the steps mentioned in this guide, one can successfully balance chemical equations by adjusting the coefficients of the reactants and products. This ensures that the law of conservation of mass is upheld, as the number of atoms on both sides of the equation remains equal. Additionally, understanding the concept of balancing chemical equations enables chemists to predict the products of a reaction, determine the quantities of reactants needed, and analyze the efficiency of chemical processes. With practice and familiarity, balancing chemical equations becomes easier and serves as a foundation for further exploration in the field of chemistry.
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