Complete and balance the equation for each of the following reactions. d. C 2 H 6 ( g ) + H 2 O ( g ) → c a t a l y s t h e a t C_2H_6\left(g\right)+H_2O\left(g\right)\overset{heat}{\underset{catalyst}\rightarrow} C 2 H 6 ( g ) + H 2 O ( g ) c a t a l ys t → h e a t

Hello, everyone. Today, we have the following problem. Predict the products formed and provide the complete balanced equation for the following reaction. So here we have a hydrocarbon reacting with water with heat and a catalyst. And this is called a steam hydrocarbon reforming process. And this reaction will form a mixture of carbon monoxide gas as well as hydrogen caps. So former answer choices, we see that the products consist of carbon monoxide and hydrogen gas and then carbon dioxide and hydrogen gas. So we know that answer choices C and D can be eliminated because we are dealing with hydro carbon monoxide. So for balancing, we have to look on each side of the reaction arrow for how many of each atom we have. So we have carbons, hydrogens and oxygens. On the left of our reaction arrow, we have four carbons and on the right, we have one on the left, we have 12 hydrogens and on the right, we have two and then we have one oxygen on the left and we have one on the right. So the first thing we want to balance is our carbons. And so we simply need to add a coefficient of four to the carbon monoxide. And that multiplies our coefficient by four. And then we see we also changed the number of oxygens on the right. So now we have four there. What we need to do next is we need to balance our oxygens and our hydrogens. And so what we can do is we can essentially essentially add a four to our water. And then we do that, we change the number of hydrogens and oxygens. And now instead of 12 hydrogens, we have 16, we have 18, excuse me. And for oxygens, we have four. And so lastly, for to get from two hydrogens to 18, we just simply add a nine to our hydrogen gas. And then we get that the balanced equation is be following. And with that, we have solved the problem overall, I hope this helped. And until next time.

Ch.22 - The Main Group Elements

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McMurry 8th Edition

Ch.22 - The Main Group Elements

Problem 22.53d

Chapter 22, Problem 22.53d

Complete and balance the equation for each of the following reactions.
d. $C_2H_6\left(g\right)+H_2O\left(g\right)\overset{heat}{\underset{catalyst}\rightarrow}$

Verified step by step guidance

Identify the type of reaction: This is a hydrocarbon combustion reaction where ethane (C₂H₆) reacts with water (H₂O) in the presence of a catalyst and heat.

Write the unbalanced chemical equation: C₂H₆(g) + H₂O(g) → products.

Determine the products: In a typical reaction involving ethane and water with heat and a catalyst, the products are often carbon dioxide (CO₂) and hydrogen gas (H₂).

Write the unbalanced equation with products: C₂H₆(g) + H₂O(g) → CO₂(g) + H₂(g).

Balance the chemical equation: Ensure the number of atoms of each element is equal on both sides of the equation. Start by balancing carbon atoms, then hydrogen atoms, and finally oxygen atoms.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Balancing Chemical Equations

Balancing chemical equations is essential to ensure that the law of conservation of mass is upheld, meaning that the number of atoms of each element must be the same on both sides of the equation. This involves adjusting coefficients in front of the chemical formulas to achieve balance. For example, in the reaction of ethane (C2H6) with water (H2O), one must determine the correct stoichiometric coefficients to balance the products formed.

Catalysts in Reactions

A catalyst is a substance that increases the rate of a chemical reaction without being consumed in the process. In the given reaction, a catalyst is indicated, which suggests that the reaction may proceed more efficiently or at a lower temperature. Understanding the role of catalysts is crucial for predicting the behavior of reactions and optimizing conditions for desired outcomes.

Thermochemistry and Heat in Reactions

Thermochemistry studies the heat changes associated with chemical reactions. The notation 'heat' in the reaction indicates that the process is endothermic or exothermic, depending on whether heat is absorbed or released. Recognizing how heat influences reaction dynamics helps in understanding reaction mechanisms and the energy profiles of reactants and products.