20. We allow 48.0 g methane, CH4, to undergo complete combustion with excess oxygen, 02. What mass of oxygen reacts? [A] What is the mass of CO2 produced? [5] Molar Mass: C: 12.01 g/mol H 1.01 gimol O: 18 g/mol
20. We allow 48.0 g methane, CH4, to undergo complete combustion with excess oxygen, 02. What mass of oxygen reacts? [A] What is the mass of CO2 produced? [5] Molar Mass: C: 12.01 g/mol H 1.01 gimol O: 18 g/mol
Introduction to Chemical Engineering Thermodynamics
8th Edition
ISBN:9781259696527
Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Chapter1: Introduction
Section: Chapter Questions
Problem 1.1P
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![19. Sulfur, S8, combines with oxygen at elevated temperatures to form sulfur dioxide.
If 200 g of oxygen are used up in this reaction, how many moles of sulfur react?
What is the mass of sulfur dioxide formed in part (a)?
Molar Mass:
S: 32.07 g/mol
O: 16 g/mol
20. We allow 48.0g methane, CH4, to undergo complete combustion
with excess oxygen, 02.
What mass of oxygen reacts? [A]
What is the mass of CO2 produced? [B]
Molar Mass:
C: 12.01 g/mol
H: 1.01 g/mol
O: 18 g/mol
21. What is the percent yield if 108 mg SO2 is isolated from the combustion of 82.7 mg of carbon disulfide
according to the reaction:
CS2 + 302 - C02 + 2502
Molar Mass:
S: 32.07 g/mol
O: 16 g/mol
C: 12.01 g/mol
22. What is the maximum amount of Ca3(PO4)2 that can be prepared from 12.9g of Ca(OH)2 and 18.37 g
of H3PO4?
Molar Mass:
Ca: 40.08 g/mol
P: 30.97 g/mol
0:16 g/mol
H:1.01 g/mol
23. The compound P4S3 is used in matches. It reacts with oxygen to produce P4010 and So.
The unbalanced chemical equation is shown below.
P4S3(s) + 02(g) – P4010(s) + SO2(g)
What mass of SO2 is produced from the combustion of 0.59 g P4S3?
MM of P4S3 = 220.09 g.mol
MM of SO2 = 64.07 g/mol
24. Solid silver nitrate undergoes thermal decomposition to form silver metal, nitrogen dioxide, and
oxygen. A 0.665-g sample of silver metal is isolated from the decomposition of a 1.099-g sample of
AGNO3. What is the percent yield of the reaction?
Molar Mass:
Ag: 107.87 g/mol
N: 14.01 g/mol
O: 16 g/mol](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F10a3a914-7d44-4939-b214-0f41094ef9c4%2Fcc121dcf-a8b3-4b85-a7a1-15098fc5496a%2F0qwsgrx_processed.jpeg&w=3840&q=75)
Transcribed Image Text:19. Sulfur, S8, combines with oxygen at elevated temperatures to form sulfur dioxide.
If 200 g of oxygen are used up in this reaction, how many moles of sulfur react?
What is the mass of sulfur dioxide formed in part (a)?
Molar Mass:
S: 32.07 g/mol
O: 16 g/mol
20. We allow 48.0g methane, CH4, to undergo complete combustion
with excess oxygen, 02.
What mass of oxygen reacts? [A]
What is the mass of CO2 produced? [B]
Molar Mass:
C: 12.01 g/mol
H: 1.01 g/mol
O: 18 g/mol
21. What is the percent yield if 108 mg SO2 is isolated from the combustion of 82.7 mg of carbon disulfide
according to the reaction:
CS2 + 302 - C02 + 2502
Molar Mass:
S: 32.07 g/mol
O: 16 g/mol
C: 12.01 g/mol
22. What is the maximum amount of Ca3(PO4)2 that can be prepared from 12.9g of Ca(OH)2 and 18.37 g
of H3PO4?
Molar Mass:
Ca: 40.08 g/mol
P: 30.97 g/mol
0:16 g/mol
H:1.01 g/mol
23. The compound P4S3 is used in matches. It reacts with oxygen to produce P4010 and So.
The unbalanced chemical equation is shown below.
P4S3(s) + 02(g) – P4010(s) + SO2(g)
What mass of SO2 is produced from the combustion of 0.59 g P4S3?
MM of P4S3 = 220.09 g.mol
MM of SO2 = 64.07 g/mol
24. Solid silver nitrate undergoes thermal decomposition to form silver metal, nitrogen dioxide, and
oxygen. A 0.665-g sample of silver metal is isolated from the decomposition of a 1.099-g sample of
AGNO3. What is the percent yield of the reaction?
Molar Mass:
Ag: 107.87 g/mol
N: 14.01 g/mol
O: 16 g/mol
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