When $CH_4(g)$ Is Burned In $O_2(g)$, The Reaction Represented By The Equation Occurs:${ CH_4(g) + 2 O_2(g) \rightarrow CO_2(g) + 2 H_2O(g) }$If 32 G Of $CH_4$ Is Burned Completely, How Many Moles Of

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When Methane is Burned: Understanding the Chemical Reaction and Stoichiometry

Chemical reactions are the foundation of chemistry, and understanding the stoichiometry of these reactions is crucial in various fields, including chemistry, physics, and engineering. In this article, we will explore the chemical reaction that occurs when methane ($CH_4(g)$) is burned in oxygen ($O_2(g)$), and we will calculate the number of moles of carbon dioxide ($CO_2(g)$) and water ($H_2O(g)$) produced when 32 g of methane is burned completely.

The chemical reaction that occurs when methane is burned in oxygen is represented by the equation:

CH4(g)+2O2(g)→CO2(g)+2H2O(g){ CH_4(g) + 2 O_2(g) \rightarrow CO_2(g) + 2 H_2O(g) }

In this reaction, one molecule of methane reacts with two molecules of oxygen to produce one molecule of carbon dioxide and two molecules of water.

Stoichiometry is the branch of chemistry that deals with the quantitative relationships between reactants and products in chemical reactions. In this case, we are interested in calculating the number of moles of carbon dioxide and water produced when 32 g of methane is burned completely.

To do this, we need to know the molar mass of methane, which is 16 g/mol. We can use this information to calculate the number of moles of methane that are present in 32 g of the substance.

Calculating the Number of Moles of Methane

The number of moles of methane can be calculated using the following formula:

n=mM{ n = \frac{m}{M} }

where $n$ is the number of moles, $m$ is the mass of the substance, and $M$ is the molar mass.

Plugging in the values, we get:

n=32 g16 g/mol=2 mol{ n = \frac{32 \text{ g}}{16 \text{ g/mol}} = 2 \text{ mol} }

So, there are 2 moles of methane present in 32 g of the substance.

Calculating the Number of Moles of Carbon Dioxide and Water

Now that we know the number of moles of methane, we can use the stoichiometry of the reaction to calculate the number of moles of carbon dioxide and water produced.

From the balanced equation, we can see that 1 mole of methane produces 1 mole of carbon dioxide and 2 moles of water. Therefore, we can calculate the number of moles of carbon dioxide and water produced as follows:

moles of CO2=moles of CH4=2 mol{ \text{moles of CO}_2 = \text{moles of CH}_4 = 2 \text{ mol} }

moles of H2O=2×moles of CH4=2×2 mol=4 mol{ \text{moles of H}_2\text{O} = 2 \times \text{moles of CH}_4 = 2 \times 2 \text{ mol} = 4 \text{ mol} }

So, there are 2 moles of carbon dioxide and 4 moles of water produced when 32 g of methane is burned completely.

In conclusion, we have explored the chemical reaction that occurs when methane is burned in oxygen, and we have calculated the number of moles of carbon dioxide and water produced when 32 g of methane is burned completely. We have used the stoichiometry of the reaction to calculate the number of moles of products produced, and we have found that there are 2 moles of carbon dioxide and 4 moles of water produced.

In our previous article, we explored the chemical reaction that occurs when methane ($CH_4(g)$) is burned in oxygen ($O_2(g)$), and we calculated the number of moles of carbon dioxide ($CO_2(g)$) and water ($H_2O(g)$) produced when 32 g of methane is burned completely. In this article, we will answer some frequently asked questions related to this topic.

Q: What is the chemical equation for the reaction between methane and oxygen?

A: The chemical equation for the reaction between methane and oxygen is:

CH4(g)+2O2(g)→CO2(g)+2H2O(g){ CH_4(g) + 2 O_2(g) \rightarrow CO_2(g) + 2 H_2O(g) }

Q: What is the molar mass of methane?

A: The molar mass of methane is 16 g/mol.

Q: How many moles of methane are present in 32 g of the substance?

A: To calculate the number of moles of methane, we can use the following formula:

n=mM{ n = \frac{m}{M} }

where $n$ is the number of moles, $m$ is the mass of the substance, and $M$ is the molar mass.

Plugging in the values, we get:

n=32 g16 g/mol=2 mol{ n = \frac{32 \text{ g}}{16 \text{ g/mol}} = 2 \text{ mol} }

So, there are 2 moles of methane present in 32 g of the substance.

Q: How many moles of carbon dioxide and water are produced when 32 g of methane is burned completely?

A: From the balanced equation, we can see that 1 mole of methane produces 1 mole of carbon dioxide and 2 moles of water. Therefore, we can calculate the number of moles of carbon dioxide and water produced as follows:

moles of CO2=moles of CH4=2 mol{ \text{moles of CO}_2 = \text{moles of CH}_4 = 2 \text{ mol} }

moles of H2O=2×moles of CH4=2×2 mol=4 mol{ \text{moles of H}_2\text{O} = 2 \times \text{moles of CH}_4 = 2 \times 2 \text{ mol} = 4 \text{ mol} }

So, there are 2 moles of carbon dioxide and 4 moles of water produced when 32 g of methane is burned completely.

Q: What is the relationship between the number of moles of methane and the number of moles of carbon dioxide and water produced?

A: From the balanced equation, we can see that 1 mole of methane produces 1 mole of carbon dioxide and 2 moles of water. Therefore, the number of moles of carbon dioxide and water produced is directly proportional to the number of moles of methane.

Q: What are the products of the reaction between methane and oxygen?

A: The products of the reaction between methane and oxygen are carbon dioxide ($CO_2(g)$) and water ($H_2O(g)$).

Q: What is the role of oxygen in the reaction between methane and oxygen?

A: Oxygen is the reactant that is necessary for the reaction between methane and oxygen to occur. It is the oxidizing agent that helps to break down the methane molecule and produce the products of the reaction.

In conclusion, we have answered some frequently asked questions related to the reaction between methane and oxygen. We have provided information on the chemical equation, molar mass, number of moles of methane, number of moles of carbon dioxide and water produced, relationship between the number of moles of methane and the number of moles of carbon dioxide and water produced, products of the reaction, and the role of oxygen in the reaction.