Sodium hydroxide reacts with carbon dioxide as follows: 2 NaOH(s) + CO 2 (g) → Na 2 CO 3 (s) + H 2 O(l) How many moles of Na 2 CO 3 can be produced?

Hi everyone for this problem. It reads consider the reaction between potassium hydroxide and sulfur dioxide below. Starting with a 1.55 moles of potassium hydroxide and 2.60 moles of sulfur dioxide, calculate the amount in moles of potassium cell fight produced. Okay, so we want to know the amount and moles of potassium sulfide produced from these two react ints. Okay. And so what we want to do here is determine which one is the limiting reactant. The limiting reactant is going to be the one that is consumed first. And that moller value that we calculate determines the theoretical yield and the problem. Alright. So we want to know from the two reactant, given how much potassium sulfide do they produce individually. So we're going to do to calculations here and then the one that is the lesser value is going to be our limiting reactant and that is going to be the theoretical yield of potassium sulfide produced. So let's go ahead and get started with our first reactant. Our first reactant is potassium hydroxide. So we want to go from we want to calculate how The amount of product produced from our potassium hydroxide and we know we have 1.55 moles of potassium hydroxide. Alright, so our goal here is to go from moles of potassium hydroxide to moles of our product potassium sulfate. Alright, so let's do that now. So we're going to set up a dimensional analysis here and we want to go from moles of reactant, two moles of product and we can do that using a mult Immel ratio. So looking at our reaction for every two moles of potassium hydroxide consumed, We have one mole of potassium sulfide produced. So that's our multiple ratio. So let's go ahead and write that here. So for every two moles of potassium hydroxide consumed, there is one mole of potassium cell fight Produced. Alright, so making sure units cancel properly are moles of potassium hydroxide cancel. And we're left with 0.775 moles of potassium soul fight produced from that amount of potassium hide dioxide. Alright, so we need to do the same thing. But with our other reactant now are sulfur dioxide. So we're told we have 2.60 moles of sulfur dioxide. So, our goal here is to go from moles of sulfur dioxide, two moles of potassium sulfide. We want to know how much product this reactant is going to produce. Alright, so let's go ahead and do the same thing. Look at our reaction. Okay, so looking at our reaction for every one mole of sulfur dioxide consumed, there is one mole of potassium cell fight produced. So let's go ahead and write that here. So, for every one mole of sulfur dioxide consumed, one mole potassium sulfite is produced. All right, So, our units of moles of sulfur dioxide cancel. And we're left with moles of potassium sulfite. This calculation yields 2.60 moles of potassium sulfate. So now we see what is the amount of product produced from each of these reactant. And like we said in the beginning, the reactant that produces the lesser amount is going to be our limiting reactant. So this is going to get used up first and our reactant, that is the larger number is going to be our excess reactant. Okay, so our limiting reactant is actually the theoretical yield in this problem. So this is going to be the answer. This is the amount of potassium sulfide produced. Okay, and so this is going to be our final answer because this is the theoretical yield. Once this, once this, once the moles of potassium hydroxide run out, that's it. That's why it's our limiting reactant, because there's going to be no more left. And so that makes this our theoretical yield and the final answer for this problem, I hope this was helpful.

Ch.3 - Chemical Reactions and Reaction Stoichiometry

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Brown 15th Edition

Ch.3 - Chemical Reactions and Reaction Stoichiometry

Problem 77b

Chapter 3, Problem 77b

Sodium hydroxide reacts with carbon dioxide as follows: 2 NaOH(s) + CO₂(g) →Na₂CO₃(s) + H₂O(l) How many moles of Na₂CO₃ can be produced?

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Identify the balanced chemical equation: \(2 \text{NaOH} + \text{CO}_2 \rightarrow \text{Na}_2\text{CO}_3 + \text{H}_2\text{O}\).

Determine the stoichiometric relationship between NaOH and Na2CO3 from the balanced equation. Here, 2 moles of NaOH produce 1 mole of Na2CO3.

Calculate the moles of NaOH available, if not given, using the formula: \(\text{moles} = \frac{\text{mass}}{\text{molar mass}}\).

Use the stoichiometric ratio from the balanced equation to find the moles of Na2CO3 produced. For every 2 moles of NaOH, 1 mole of Na2CO3 is produced.

Verify that the amount of CO2 is sufficient to react with the available NaOH, ensuring that NaOH is the limiting reactant.

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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 amount of substances consumed and produced in a reaction based on balanced chemical equations. In this case, understanding the stoichiometric coefficients in the reaction is essential to determine how many moles of Na2CO3 can be produced from the given amounts of NaOH and CO2.

Balanced Chemical Equation

A balanced chemical equation represents a chemical reaction with equal numbers of each type of atom on both sides of the equation. This ensures the law of conservation of mass is upheld. In the provided reaction, the coefficients indicate that two moles of NaOH react with one mole of CO2 to produce one mole of Na2CO3 and one mole of H2O, which is crucial for calculating the moles of products formed.

Mole Concept

The mole concept is a fundamental principle in chemistry that relates the mass of a substance to the number of particles it contains. One mole of any substance contains Avogadro's number of entities (approximately 6.022 x 10^23). This concept is vital for converting between grams and moles, allowing us to determine how many moles of Na2CO3 can be produced based on the initial amounts of NaOH and CO2 used in the reaction.