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 C 2 H 2 are present after the reaction is complete?

Hey everyone in this example, we have hydrochloric acid solution reacting with silver nitrate to produce our products, silver chloride, which is a solid precipitate and nitric acid. We need to figure out the mass of hydrochloric acid RV agent that remains in solution. So we need to figure out our excess reactant leftover in grimm's. So we want to go ahead and make note of the molds of each of our re agents in our given reaction. And also there should be a three here next to the oxygen for silver nitrate. We also want to make sure that this equation is balanced and based on the total amount of atoms for each of our elements on both sides of our equation. This definitely is a balanced reaction. So, beginning with finding the moles of our hcl, we're told that according to this question, we use 15 g of hcl. So we're gonna start out with 15 g of hcl and we're gonna use we're gonna go from grams to moles of hcl. So we're going to use the periodic table to refer to our molar mass for hydrochloric acid, which we see is equal to a mass of 36.46 g for one mole of hcl. And this is going to give us 0.411 moles of our hcl re agent. We also want to find moles of our second re agent, which is our silver nitrate. And we are given the mass used as 10 g of silver nitrate from the prompt. So we want to go ahead and convert from grams of silver nitrate, two moles of silver nitrate. So sorry, that should be a three there. And this here says moles. So using our periodic tables, we would see that the molar mass for silver nitrate Is equal to a value of 169.87 g for one mole of silver nitrate. And so canceling out our units of g were left with moles of silver nitrate. Which we're going to get a value equal to 0.0589 moles of silver nitrate. And because we see that 0.0589 moles of silver nitrate Is less than 0. moles of hydrochloric acid. We can say that therefore hcl is left in access. So we have Hcl or hydrochloric acid left over after our reaction is complete. And so we need to find our moles of hydrochloric acid that is consumed to figure out how much is left over and excess and moles. So we're gonna take our .411 moles of our hydrochloric acid and subtract that from our second reactant, which we know is our silver nitrate. And we said above that we would Have 0. moles of silver nitrate reacting. And this difference gives us our moles of hydrochloric acid consumed equal to 0.352 moles. Or rather we can say that this is our moles of hcl that is remaining. And so now that we have this value in moles, we want to actually get this in grams to completely answer this question because it's asking for the mass of Hcl remaining in the solution. So we would say that the mass of Hcl that remains Is going to equal our moles which we just said leftover is 0.352 moles of hcl. And we want to go from moles of hcl two g of hcl. So we're going to utilize our periodic tables and find the molar mass of HcL which we can recall is equal to 36.46 g of Hcl for one mole of Hcl. Now we're able to cancel our units of moles leaving us with our massive hcl which is going to give us our final results equal to 12.8 g of hcl that is left over in excess and this is going to be our final answer to complete this example. So I hope that everything I explained was clear. If you have any questions, please leave them down below and I will 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 103c1

Chapter 3, Problem 103c1

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?

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Identify the balanced chemical equation for the combustion of acetylene: \( 2 \text{C}_2\text{H}_2 + 5 \text{O}_2 \rightarrow 4 \text{CO}_2 + 2 \text{H}_2\text{O} \).

Calculate the molar mass of \( \text{C}_2\text{H}_2 \) and \( \text{O}_2 \).

Determine the number of moles of \( \text{C}_2\text{H}_2 \) and \( \text{O}_2 \) initially present using their respective masses and molar masses.

Identify the limiting reactant by comparing the mole ratio of \( \text{C}_2\text{H}_2 \) to \( \text{O}_2 \) with the stoichiometric ratio from the balanced equation.

Calculate the amount of \( \text{C}_2\text{H}_2 \) remaining after the reaction by considering the limiting reactant and the initial moles of \( \text{C}_2\text{H}_2 \).

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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. Understanding stoichiometry is essential for determining how much of each reactant is needed and how much product can be formed.

Limiting Reactant

The limiting reactant is the substance that is completely consumed first in a chemical reaction, thus determining the maximum amount of product that can be formed. Identifying the limiting reactant is crucial for calculating the amounts of products and remaining reactants after the reaction. In the case of the combustion of acetylene and oxygen, one of these reactants will limit the formation of CO2 and H2O.

Combustion Reaction

A combustion reaction is a chemical process in which a substance (usually a hydrocarbon) reacts with oxygen to produce carbon dioxide and water, releasing energy in the form of heat and light. The general form of a combustion reaction can be represented as: hydrocarbon + O2 → CO2 + H2O. Understanding the products and the stoichiometry involved in combustion reactions is vital for solving problems related to the amounts of reactants and products.

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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 CO₂ and H₂O are 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 C2H2 are present after the reaction is complete?

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Key Concepts

Stoichiometry

Limiting Reactant

Combustion Reaction

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?