Consider a situation in which 235 g of P4 are exposed to 272 g of O2 . Part A What is the maximum number of moles of P2O5 that can theoretically be made from 235 g of P4 and excess oxygen? Express your answer to three significant figures and include the appropriate units. • View Available Hint(s) HA ? Value Units Submit Part B What is the maximum number of moles of P20; that can theoretically be made from 272 g of O2 and excess phosphorus? Express your answer to three significant figures and include the appropriate units. • View Available Hint(s) HA ? Value Units
Consider a situation in which 235 g of P4 are exposed to 272 g of O2 . Part A What is the maximum number of moles of P2O5 that can theoretically be made from 235 g of P4 and excess oxygen? Express your answer to three significant figures and include the appropriate units. • View Available Hint(s) HA ? Value Units Submit Part B What is the maximum number of moles of P20; that can theoretically be made from 272 g of O2 and excess phosphorus? Express your answer to three significant figures and include the appropriate units. • View Available Hint(s) HA ? Value Units
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.
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![**Learning Goal:**
To calculate theoretical and percent yields, given the masses of multiple reactants.
A balanced chemical reaction gives the mole ratios between reactants and products. For example, one mole of white phosphorus, \( P_4 \), reacts with five moles of oxygen, \( O_2 \), to produce two moles of diphosphorus pentoxide, \( P_2O_5 \):
\[ P_4 + 5O_2 \rightarrow 2P_2O_5 \]
In this example, if we know the number of moles of phosphorus, we know that twice that much product can be made, assuming we have enough oxygen. Similarly, if we know the number of moles of oxygen, we know that two-fifths that much product can be made, assuming we have enough phosphorus. In a situation where you are given the mole amounts of both reactants, you should do this type of calculation individually for each one, finding two different values for the amount of product. The smaller of these two values is the maximum amount of product that can be made, also known as the theoretical yield.
If you are given the masses of the reactants, you will first have to convert to moles. Once you have mole amounts, you can follow the procedure described above, applying the ratios shown in the balanced chemical equation.
**Consider a situation in which 235 g of \( P_4 \) are exposed to 272 g of \( O_2 \).**
**Part A**
What is the maximum number of moles of \( P_2O_5 \) that can theoretically be made from 235 g of \( P_4 \) and excess oxygen?
Express your answer to three significant figures and include the appropriate units.
\[ \text{Value} \quad \text{Units} \]
*Submit*
**Part B**
What is the maximum number of moles of \( P_2O_5 \) that can theoretically be made from 272 g of \( O_2 \) and excess phosphorus?
Express your answer to three significant figures and include the appropriate units.
\[ \text{Value} \quad \text{Units} \]
*Submit*
**Part C** Complete previous part(s)
**Part D** Complete previous part(s)](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fbcea870b-a558-4e25-bd85-f50b869e1110%2F74c1ff1d-836e-4410-9e89-12505a7cb5f1%2F0juptf6_processed.png&w=3840&q=75)
Transcribed Image Text:**Learning Goal:**
To calculate theoretical and percent yields, given the masses of multiple reactants.
A balanced chemical reaction gives the mole ratios between reactants and products. For example, one mole of white phosphorus, \( P_4 \), reacts with five moles of oxygen, \( O_2 \), to produce two moles of diphosphorus pentoxide, \( P_2O_5 \):
\[ P_4 + 5O_2 \rightarrow 2P_2O_5 \]
In this example, if we know the number of moles of phosphorus, we know that twice that much product can be made, assuming we have enough oxygen. Similarly, if we know the number of moles of oxygen, we know that two-fifths that much product can be made, assuming we have enough phosphorus. In a situation where you are given the mole amounts of both reactants, you should do this type of calculation individually for each one, finding two different values for the amount of product. The smaller of these two values is the maximum amount of product that can be made, also known as the theoretical yield.
If you are given the masses of the reactants, you will first have to convert to moles. Once you have mole amounts, you can follow the procedure described above, applying the ratios shown in the balanced chemical equation.
**Consider a situation in which 235 g of \( P_4 \) are exposed to 272 g of \( O_2 \).**
**Part A**
What is the maximum number of moles of \( P_2O_5 \) that can theoretically be made from 235 g of \( P_4 \) and excess oxygen?
Express your answer to three significant figures and include the appropriate units.
\[ \text{Value} \quad \text{Units} \]
*Submit*
**Part B**
What is the maximum number of moles of \( P_2O_5 \) that can theoretically be made from 272 g of \( O_2 \) and excess phosphorus?
Express your answer to three significant figures and include the appropriate units.
\[ \text{Value} \quad \text{Units} \]
*Submit*
**Part C** Complete previous part(s)
**Part D** Complete previous part(s)
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