17. 18. 24. N H (19-22) Given the equation: 4 NH3 +7 0₂ ----> 4 NO₂ + 6 H₂O 0 14 How many moles of NH, must react if 24.8 moles of water are produced? Determine the number of moles of H₂O that would be formed from the combustion of 86.0 grams of NH3. mot bar If 182 grams of NO₂ are formed, what number of moles of oxygen must have been consumed? Calculate the percent yield of H₂O if 80.0 g of H₂O are formed from reaction of 62.1 g of NH3. 19. 20. 21. 22. 23. What is the percent yield of Fe₂O3 if 2.90 g of Fe₂O3 are formed from reaction of 10.0 g of Fe(CrO₂)2? If 100.0 g of Fe(CrO2)2 is reacted with 50.00 g of K₂CO3 which reactant is limiting? 4 N 0 14 Given: 4 Al (s) + 3 02 (g) → 2 Al2O3(s) How many grams of Al2O3 could be produced from 225 grams of Al reacting with 429 grams of O₂? Given: 3 Mg(OH)2 (s) + 2 H3PO4 (aq) → 6 H₂0 (1) + Mg3(PO4)2 (s) How many moles of water could be produced from the reaction of 575 grams of Mg(OH)2 with 800. grams of H3PO4?
17. 18. 24. N H (19-22) Given the equation: 4 NH3 +7 0₂ ----> 4 NO₂ + 6 H₂O 0 14 How many moles of NH, must react if 24.8 moles of water are produced? Determine the number of moles of H₂O that would be formed from the combustion of 86.0 grams of NH3. mot bar If 182 grams of NO₂ are formed, what number of moles of oxygen must have been consumed? Calculate the percent yield of H₂O if 80.0 g of H₂O are formed from reaction of 62.1 g of NH3. 19. 20. 21. 22. 23. What is the percent yield of Fe₂O3 if 2.90 g of Fe₂O3 are formed from reaction of 10.0 g of Fe(CrO₂)2? If 100.0 g of Fe(CrO2)2 is reacted with 50.00 g of K₂CO3 which reactant is limiting? 4 N 0 14 Given: 4 Al (s) + 3 02 (g) → 2 Al2O3(s) How many grams of Al2O3 could be produced from 225 grams of Al reacting with 429 grams of O₂? Given: 3 Mg(OH)2 (s) + 2 H3PO4 (aq) → 6 H₂0 (1) + Mg3(PO4)2 (s) How many moles of water could be produced from the reaction of 575 grams of Mg(OH)2 with 800. grams of H3PO4?
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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Thermochemistry
Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.
Exergonic Reaction
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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19,20,21 please
![### Educational Chemistry Problems
#### Question 17
What is the percent yield of Fe₂O₃ if 2.90 g of Fe₂O₃ are formed from the reaction of 10.0 g of Fe(CrO₂)₂?
#### Question 18
If 100.0 g of Fe(CrO₂)₂ is reacted with 50.00 g of K₂CO₃, which reactant is limiting?
---
(19-22) **Given the equation**:
\[ 4 \text{NH}_3 + 7 \text{O}_2 \rightarrow 4 \text{NO}_2 + 6 \text{H}_2\text{O} \]
#### Question 19
How many moles of NH₃ must react if 24.8 moles of water are produced?
#### Question 20
Determine the number of moles of H₂O that would be formed from the combustion of 86.0 grams of NH₃.
#### Question 21
If 182 grams of NO₂ are formed, what number of moles of oxygen must have been consumed?
#### Question 22
Calculate the percent yield of H₂O if 80.0 g of H₂O are formed from the reaction of 62.1 g of NH₃.
---
#### Question 23
**Given**:
\[ 4 \text{Al} (s) + 3 \text{O}_2 (g) \rightarrow 2 \text{Al}_2\text{O}_3 (s) \]
How many grams of Al₂O₃ could be produced from 225 grams of Al reacting with 429 grams of O₂?
#### Question 24
**Given**:
\[ 3 \text{Mg(OH)}_2 (s) + 2 \text{H}_3\text{PO}_4 (aq) \rightarrow 6 \text{H}_2\text{O} (l) + \text{Mg}_3(\text{PO}_4)_2 (s) \]
How many moles of water could be produced from the reaction of 575 grams of Mg(OH)₂ with 800 grams of H₃PO₄?](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F89ca33f5-cb99-4448-ba96-35f6ac44a938%2F9ba467b2-b64e-479a-be31-06ec49d20678%2Fh2h7zz_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Educational Chemistry Problems
#### Question 17
What is the percent yield of Fe₂O₃ if 2.90 g of Fe₂O₃ are formed from the reaction of 10.0 g of Fe(CrO₂)₂?
#### Question 18
If 100.0 g of Fe(CrO₂)₂ is reacted with 50.00 g of K₂CO₃, which reactant is limiting?
---
(19-22) **Given the equation**:
\[ 4 \text{NH}_3 + 7 \text{O}_2 \rightarrow 4 \text{NO}_2 + 6 \text{H}_2\text{O} \]
#### Question 19
How many moles of NH₃ must react if 24.8 moles of water are produced?
#### Question 20
Determine the number of moles of H₂O that would be formed from the combustion of 86.0 grams of NH₃.
#### Question 21
If 182 grams of NO₂ are formed, what number of moles of oxygen must have been consumed?
#### Question 22
Calculate the percent yield of H₂O if 80.0 g of H₂O are formed from the reaction of 62.1 g of NH₃.
---
#### Question 23
**Given**:
\[ 4 \text{Al} (s) + 3 \text{O}_2 (g) \rightarrow 2 \text{Al}_2\text{O}_3 (s) \]
How many grams of Al₂O₃ could be produced from 225 grams of Al reacting with 429 grams of O₂?
#### Question 24
**Given**:
\[ 3 \text{Mg(OH)}_2 (s) + 2 \text{H}_3\text{PO}_4 (aq) \rightarrow 6 \text{H}_2\text{O} (l) + \text{Mg}_3(\text{PO}_4)_2 (s) \]
How many moles of water could be produced from the reaction of 575 grams of Mg(OH)₂ with 800 grams of H₃PO₄?
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