The following diagram represents the reaction of A 2 (red spheres) with B 2 (blue spheres): <IMAGE> b. How many moles of product can be made from 1.0 mol of A 2 ? From 1.0 mol of B 2 ?

Welcome back everyone. The diagram below represents the reaction X two plus three moles of Y two to form two xy three, determine the number of moles of product that can form from moles of X two and 22 moles of Y. To notice that the reaction were given in the prompt is a balanced reaction. And we can use the ratios between our reactant and products as Tokyo metric conversion factors to get to our final answer for part one and two of our prompt beginning with part one of our prompt. We need to find our moles of our product XY 3 to 4 that are formed from two moles of X to our reactant. So we have beginning with two moles of X two. We're going to multiply by the ratio between moles of X to our reactant, two moles of xy three. Sorry, it's X capital Y three sub three, which is our product. We can see from our balanced equation that we have a ratio between for every one mole of X two reacted. We have two moles of XY three produced. So canceling out moles of X two were left with moles of our product xy three produced. And this is going to equal a total of four moles of product Xy three produced or we can say formed. So for part two, we're going to follow the same process where we begin now with two moles of Y to our second reactant. And we're going to multiply by the stoke geometric ratio between moles of Y two and our denominator two moles of our product X Y sub three in our numerator where from our balanced equation, we see that for every three moles of why to react reacted, we form two moles of xy three product. So canceling out moles of Y two, our reactant, we're left with moles of xy three, our product. And this is going to simplify to 1.3, 3 Moles of XY three that is formed Which we can just round two, two sig figs as 1.3 moles of xy three and sorry, just so this is visible, we'll move this over. So our final answers are our two moles of our product xy three that is formed from parts one and two of our prompt. And this will correspond to choice a in the multiple choice as the correct answer. So I hope that this made sense and let us know if you have any questions

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6. Chemical Reactions & Quantities

Stoichiometry

GOB Chemistry

6. Chemical Reactions & Quantities

Stoichiometry

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2:47 minutes

Problem 16b

Textbook Question

The following diagram represents the reaction of A₂(red spheres) with B₂(blue spheres):
<IMAGE>
b. How many moles of product can be made from 1.0 mol of A₂? From 1.0 mol of B₂?

Verified step by step guidance

Step 1: Analyze the chemical reaction depicted in the diagram. The reaction involves two reactants, A2 (red spheres) and B2 (blue spheres), forming a product XY3 (one blue sphere bonded to three red spheres). This indicates a stoichiometric relationship between the reactants and the product.

Step 2: Write the balanced chemical equation for the reaction. Based on the diagram, the reaction can be expressed as: A2 + 3B2 → 2XY3. This shows that 1 mole of A2 reacts with 3 moles of B2 to produce 2 moles of XY3.

Step 3: Determine the limiting reactant for each scenario. For 1.0 mol of A2, calculate how many moles of B2 are required using the stoichiometric ratio (1:3). Similarly, for 1.0 mol of B2, calculate how many moles of A2 are required using the stoichiometric ratio (3:1).

Step 4: Use the stoichiometric ratios to calculate the maximum moles of product (XY3) that can be formed. For 1.0 mol of A2, use the ratio from the balanced equation (1 A2 produces 2 XY3). For 1.0 mol of B2, use the ratio (3 B2 produces 2 XY3).

Step 5: Compare the results from both scenarios to determine the amount of product formed in each case. Ensure that the calculations respect the stoichiometric relationships and the limiting reactant concept.

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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 how many moles of products can be formed from given amounts of reactants based on the balanced chemical equation. Understanding stoichiometry is essential for solving problems related to the amounts of substances involved in reactions.

Mole Ratio

The mole ratio is a conversion factor derived from the coefficients of a balanced chemical equation. It indicates the proportion of moles of one substance to another in a reaction. For example, if the reaction shows that 1 mole of A2 reacts with 2 moles of B2 to produce 1 mole of XY3, the mole ratio can be used to determine how much product can be formed from a specific amount of reactants.

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 accurately calculating the yield of products. In the context of the given question, knowing which reactant limits the formation of XY3 will help determine how many moles of the product can be produced from the available amounts of A2 and B2.