Balance The Following Chemical Equation And Identify The Type Of Reaction: 2 H 2 ( G ) + O 2 ( G ) → 2 H 2 O ( L ) + 136.6 Kcal 2 \text{H}_2(g) + \text{O}_2(g) \rightarrow 2 \text{H}_2\text{O}(l) + 136.6 \text{kcal} 2 H 2 ​ ( G ) + O 2 ​ ( G ) → 2 H 2 ​ O ( L ) + 136.6 Kcal

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Introduction

Chemical equations are a fundamental concept in chemistry, representing the transformation of one or more substances into another. Balancing chemical equations is a crucial step in understanding the stoichiometry of a reaction, which is essential in predicting the amount of products formed and the amount of reactants consumed. In this article, we will balance the given chemical equation and identify the type of reaction it represents.

The Given Chemical Equation

The given chemical equation is:

2H2(g)+O2(g)→2H2O(l)+136.6kcal2 \text{H}_2(g) + \text{O}_2(g) \rightarrow 2 \text{H}_2\text{O}(l) + 136.6 \text{kcal}

Balancing the Chemical Equation

To balance the chemical equation, we need to ensure that the number of atoms of each element is the same on both the reactant and product sides. Let's start by counting the number of atoms of each element on both sides of the equation.

Reactant side:

  • Hydrogen (H): 2 x 2 = 4
  • Oxygen (O): 1

Product side:

  • Hydrogen (H): 2 x 2 = 4
  • Oxygen (O): 2

As we can see, the number of hydrogen atoms is balanced, but the number of oxygen atoms is not. To balance the oxygen atoms, we need to add a coefficient of 2 in front of O2 on the reactant side.

2H2(g)+2O2(g)→2H2O(l)+136.6kcal2 \text{H}_2(g) + 2 \text{O}_2(g) \rightarrow 2 \text{H}_2\text{O}(l) + 136.6 \text{kcal}

Now, let's count the number of atoms of each element on both sides of the equation again.

Reactant side:

  • Hydrogen (H): 2 x 2 = 4
  • Oxygen (O): 2 x 2 = 4

Product side:

  • Hydrogen (H): 2 x 2 = 4
  • Oxygen (O): 2

The number of hydrogen and oxygen atoms is now balanced on both sides of the equation.

Identifying the Type of Reaction

Now that we have balanced the chemical equation, let's identify the type of reaction it represents. The given chemical equation is:

2H2(g)+2O2(g)→2H2O(l)+136.6kcal2 \text{H}_2(g) + 2 \text{O}_2(g) \rightarrow 2 \text{H}_2\text{O}(l) + 136.6 \text{kcal}

This equation represents a combustion reaction, where hydrogen gas reacts with oxygen gas to form water. The energy released in the form of heat is 136.6 kcal.

Combustion Reactions

Combustion reactions are a type of chemical reaction where a substance reacts with oxygen to release energy in the form of heat and light. The general equation for a combustion reaction is:

Fuel+O2→Products+Heat\text{Fuel} + \text{O}_2 \rightarrow \text{Products} + \text{Heat}

In the given chemical equation, hydrogen gas is the fuel, and oxygen gas is the oxidizer. The products of the reaction are water and heat energy.

Energy Changes in Chemical Reactions

The given chemical equation also represents an energy change in a chemical reaction. The energy released in the form of heat is 136.6 kcal. This energy change can be represented by the following equation:

Energy=Heat+Work\text{Energy} = \text{Heat} + \text{Work}

In this case, the energy released in the form of heat is 136.6 kcal, and the work done is zero (since there is no external work done in the reaction).

Conclusion

In conclusion, we have balanced the given chemical equation and identified the type of reaction it represents. The balanced chemical equation is:

2H2(g)+2O2(g)→2H2O(l)+136.6kcal2 \text{H}_2(g) + 2 \text{O}_2(g) \rightarrow 2 \text{H}_2\text{O}(l) + 136.6 \text{kcal}

This equation represents a combustion reaction, where hydrogen gas reacts with oxygen gas to form water and release energy in the form of heat.

References

  • Atkins, P. W., & de Paula, J. (2010). Physical chemistry (9th ed.). Oxford University Press.
  • Chang, R. (2010). Chemistry: The central science (11th ed.). McGraw-Hill.
  • Petrucci, R. H., Harwood, W. S., & Herring, F. G. (2011). General chemistry: Principles and modern applications (10th ed.). Pearson Education.

Keywords

  • Balancing chemical equations
  • Combustion reactions
  • Energy changes in chemical reactions
  • Stoichiometry
  • Chemical equations
  • Reaction types
  • Energy released in chemical reactions
    Balancing Chemical Equations and Identifying Reaction Types: Q&A ================================================================

Introduction

In our previous article, we balanced the given chemical equation and identified the type of reaction it represents. In this article, we will answer some frequently asked questions related to balancing chemical equations and identifying reaction types.

Q: What is the purpose of balancing chemical equations?

A: The purpose of balancing chemical equations is to ensure that the number of atoms of each element is the same on both the reactant and product sides. This is essential in predicting the amount of products formed and the amount of reactants consumed.

Q: How do I balance a chemical equation?

A: To balance a chemical equation, follow these steps:

  1. Write down the unbalanced equation.
  2. Count the number of atoms of each element on both the reactant and product sides.
  3. Add coefficients in front of the formulas of reactants or products to balance the number of atoms of each element.
  4. Check if the equation is balanced by counting the number of atoms of each element on both sides.

Q: What is the difference between a balanced and unbalanced chemical equation?

A: A balanced chemical equation has the same number of atoms of each element on both the reactant and product sides. An unbalanced chemical equation has a different number of atoms of each element on both sides.

Q: Can a chemical equation be balanced in more than one way?

A: Yes, a chemical equation can be balanced in more than one way. However, the balanced equation that is most commonly used is the one that has the smallest possible coefficients.

Q: How do I identify the type of reaction represented by a chemical equation?

A: To identify the type of reaction represented by a chemical equation, follow these steps:

  1. Look at the reactants and products.
  2. Determine if the reaction involves the combination of two or more substances to form a new substance.
  3. Determine if the reaction involves the decomposition of a substance into two or more substances.
  4. Determine if the reaction involves the replacement of one element with another element.
  5. Determine if the reaction involves the release or absorption of energy.

Q: What are some common types of chemical reactions?

A: Some common types of chemical reactions include:

  • Combination reactions: These reactions involve the combination of two or more substances to form a new substance.
  • Decomposition reactions: These reactions involve the decomposition of a substance into two or more substances.
  • Replacement reactions: These reactions involve the replacement of one element with another element.
  • Combustion reactions: These reactions involve the reaction of a substance with oxygen to release energy in the form of heat and light.
  • Neutralization reactions: These reactions involve the reaction of an acid with a base to form a salt and water.

Q: How do I determine the energy change in a chemical reaction?

A: To determine the energy change in a chemical reaction, follow these steps:

  1. Write down the balanced chemical equation.
  2. Determine the energy change using the following equation:

ΔE = ΔH + ΔU

where ΔE is the energy change, ΔH is the enthalpy change, and ΔU is the internal energy change.

Q: What is the difference between enthalpy and internal energy?

A: Enthalpy (H) is a measure of the total energy of a system, including the energy of the system itself and the energy of the surroundings. Internal energy (U) is a measure of the energy of a system itself.

Conclusion

In conclusion, balancing chemical equations and identifying reaction types are essential skills in chemistry. By following the steps outlined in this article, you can balance chemical equations and identify the type of reaction represented by a chemical equation.

References

  • Atkins, P. W., & de Paula, J. (2010). Physical chemistry (9th ed.). Oxford University Press.
  • Chang, R. (2010). Chemistry: The central science (11th ed.). McGraw-Hill.
  • Petrucci, R. H., Harwood, W. S., & Herring, F. G. (2011). General chemistry: Principles and modern applications (10th ed.). Pearson Education.

Keywords

  • Balancing chemical equations
  • Identifying reaction types
  • Energy changes in chemical reactions
  • Stoichiometry
  • Chemical equations
  • Reaction types
  • Energy released in chemical reactions
  • Enthalpy
  • Internal energy