When a mixture of 10.0 g of acetylene (C 2 H 2 ) and 10.0 g of oxygen (O 2 ) is ignited, the resulting combustion reaction produces CO 2 and H 2 O. (c) How many grams of CO 2 and H 2 O are present after the reaction is complete?

Welcome back everyone in this example, we're told that ethanol is a fuel made from renewable sources and produces less carbon dioxide than traditional fossil fuels. We need to calculate what massive carbon dioxide gas is produced when 13.5 g of ethanol undergoes complete combustion with 45 g of oxygen. So we want to recall that in a combustion reaction, we have our re agent which in this case is ethanol, which we recall is the formula C two H five oh H. It's reacting with oxygen and in combustion reactions, our products are always carbon dioxide and water. And as far as our labels are, ethanol is going to be a liquid and the rest of our re agents are going to have the gaseous label. Our next step is to ensure that this equation is balanced. And when we look at the molds of each of our Atoms on both sides of our equation, we're going to have to place a coefficient of three in front of our 02, a coefficient of two in front of our CO2 and a coefficient of three in front of our water so that we can ensure we have a balanced equation. Now, the prompt is asking us to figure out the mass of carbon dioxide that is produced is essentially asking us for our theoretical yield of our carbon dioxide. So we're going to need to find the theoretical yield of carbon dioxide based on both of our reactant. So, first we're going to find the theoretical yields for the mass of carbon dioxide that is produced. And sorry, that's CO2. So for the massive carbon dioxide that is produced from ethanol. So we want to make note of our molar ratio between our ethanol And our carbon dioxide. And we would get that from our balanced equation where we see we have a coefficient of one in front of ethanol and then we have a coefficient of two in front of our carbon dioxide. So we have a 1-2 molar ratio. So we're going to begin our calculation with our massive ethanol from the prompt given us 13.5 g of ethanol and we want to cancel out our units of grams of ethanol to get two moles. And so we're going to recall our molar mass of ethanol from the periodic table which we see as equal to 46.7 g of ethanol For one mole of ethanol. So now we're able to cancel out our units of grams of ethanol. And now we want to focus on going from moles of ethanol to moles of our product carbon dioxide. And we would get that from our molar ratio, which we noted to the left where we said we have one mole of ethanol for one mole of carbon dioxide. So now we're able to cancel out our moles of ethanol. And now we want to get two g of carbon dioxide. So we would recall our molar mass of carbon dioxide from the periodic table, which we understand for one mole of carbon dioxide is 43.99 g of CO2. So now we can cancel out our units of moles of carbon dioxide And we're left with our final unit being grams of carbon dioxide. And this is going to produce a mass from our ethanol of our carbon dioxide being 25.8 g of CO2. So now we want to compare this to the theoretical yields for our mass of carbon dioxide from our second reactant being oxygen. So making note of our molar ratio between oxygen and carbon dioxide, we see from our balanced equation that that ratio is a two 23 Molar ratio. And so beginning with our mass of oxygen from the prompt, we have a mass of 45.0 g of oxygen. We're going to multiply to get two moles of oxygen by recalling our molar mass from the product table, which we understand is 32 g of oxygen for one mole of oxygen. So now we can cancel out our grams of oxygen. And now we want to get from moles of oxygen. Two moles of C. 02. So, using our ratio that we took note of, we said, we have two moles of oxygen for three moles of C. 02. So now we can cancel out moles of 02 and focus on going from moles of C 022 g of C 02. So we're calling from the periodic table, our molar mass of C. 02. We see that we have one mole of C. 02 for 43.99 grams of C. 02. And now we can cancel our moles of C. 02. We're left with grams of C. 02. And this gives us a mass equal to 41.2 g of C. 02 produced from our re agent oxygen. And because we can see that we have only 25.8 g of C. 02, which is less than 41.2 g of C. 02. We would say that therefore our ethanol which makes that lower amount of carbon dioxide. So our ethanol is our limiting reactant and the reaction the reaction produces the mass of carbon dioxide being 25.8 g of C. 02. And so for our final answer, we have that highlighted in yellow here that our mass of carbon dioxide is 25.8 g produced from our ethanol. So actually we should just highlight the mass of C. 02 produced. So what's highlighted in yellow is our final answer. I hope that everything I explained was clear. If you have any questions, leave them down below and I'll see everyone in the next practice video

Ch.3 - Chemical Reactions and Reaction Stoichiometry

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Brown 15th Edition

Ch.3 - Chemical Reactions and Reaction Stoichiometry

Problem 103c3

Chapter 3, Problem 103c3

When a mixture of 10.0 g of acetylene (C₂H₂) and 10.0 g of oxygen (O₂) is ignited, the resulting combustion reaction produces CO₂ and H₂O. (c) How many grams of CO₂ and H₂O are present after the reaction is complete?

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Determine the molar mass of acetylene (C2H2) and oxygen (O2).

Calculate the moles of acetylene and oxygen initially present using their respective molar masses.

Write the balanced chemical equation for the combustion of acetylene: 2 C2H2 + 5 O2 ightarrow 4 CO2 + 2 H2O.

Using stoichiometry, determine the limiting reactant by comparing the mole ratio from the balanced equation with the moles of each reactant calculated.

Calculate the moles of CO2 produced based on the moles of the limiting reactant, then convert these moles of CO2 to grams using the molar mass of CO2.

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Key Concepts

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

Stoichiometry

Stoichiometry is the branch of chemistry that deals with the quantitative relationships between the reactants and products in a chemical reaction. It allows us to calculate the amounts of substances consumed and produced in a reaction based on balanced chemical equations. In this case, understanding the stoichiometric ratios of acetylene and oxygen will help determine how much carbon dioxide is produced.

Combustion Reactions

Combustion reactions are exothermic reactions that occur when a substance reacts with oxygen, producing heat and light. In the case of acetylene (C2H2), it combusts in the presence of oxygen to form carbon dioxide (CO2) and water (H2O). Recognizing the products of the combustion of acetylene is essential for calculating the mass of CO2 produced.

Molar Mass

Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). It is crucial for converting between grams of a substance and moles, which are used in stoichiometric calculations. For this problem, knowing the molar masses of acetylene, oxygen, carbon dioxide, and water will facilitate the conversion of the initial masses into moles, allowing for the determination of the final mass of CO2 produced.

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Molar Mass Concept

Related Practice

Textbook Question

A mixture of N21g2 and H21g2 reacts in a closed container to form ammonia, NH31g2. The reaction ceases before either reactant has been totally consumed. At this stage 3.0 mol N2, 3.0 mol H2, and 3.0 mol NH3 are present. How many moles of N2 and H2 were present originally?

Textbook Question

A mixture containing KClO3, K2CO3, KHCO3, and KCl was heated, producing CO2, O2, and H2O gases according to the following equations: 2 KClO31s2¡2 KCl1s2 + 3 O21g2 2 KHCO31s2¡K2O1s2 + H2O1g2 + 2 CO21g2 K2CO31s2¡K2O1s2 + CO21g2 The KCl does not react under the conditions of the reaction. If 100.0 g of the mixture produces 1.80 g of H2O, 13.20 g of CO2, and 4.00 g of O2, what was the composition of the original mixture? (Assume complete decomposition of the mixture.) How many grams of K2CO3 were in the original mixture?

Textbook Question

When a mixture of 10.0 g of acetylene (C₂H₂) and 10.0 g of oxygen (O₂) is ignited, the resulting combustion reaction produces CO₂ and H₂O. (c) How many grams of C₂H₂are present after the reaction is complete?

Textbook Question

The source of oxygen that drives the internal combustion engine in an automobile is air. Air is a mixture of gases, principally N₂(79%) and O₂(20%). In the cylinder of an automobile engine, nitrogen can react with oxygen to produce nitric oxide gas, NO. As NO is emitted from the tailpipe of the car, it can react with more oxygen to produce nitrogen dioxide gas. (b) Both nitric oxide and nitrogen dioxide are pollutants that can lead to acid rain and global warming; collectively, they are called 'NOx' gases. In 2009, the United States emitted an estimated 19 million tons of nitrogen dioxide into the atmosphere. How many grams of nitrogen dioxide is this?

Textbook Question

The source of oxygen that drives the internal combustion engine in an automobile is air. Air is a mixture of gases, principally N₂(79%) and O₂(20%). In the cylinder of an automobile engine, nitrogen can react with oxygen to produce nitric oxide gas, NO. As NO is emitted from the tailpipe of the car, it can react with more oxygen to produce nitrogen dioxide gas. (c) The production of NOx gases is an unwanted side reaction of the main engine combustion process that turns octane, C₈H₁₈, into CO₂ and water. If 85% of the oxygen in an engine is used to combust octane and the remainder used to produce nitrogen dioxide, calculate how many grams of nitrogen dioxide would be produced during the combustion of 500 g of octane.

When a mixture of 10.0 g of acetylene (C2H2) and 10.0 g of oxygen (O2) is ignited, the resulting combustion reaction produces CO2 and H2O. (c) How many grams of CO2 and H2O are present after the reaction is complete?

Verified video answer for a similar problem:

Key Concepts

Stoichiometry

Combustion Reactions

Molar Mass

When a mixture of 10.0 g of acetylene (C₂H₂) and 10.0 g of oxygen (O₂) is ignited, the resulting combustion reaction produces CO₂ and H₂O. (c) How many grams of CO₂ and H₂O are present after the reaction is complete?